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Honors Chemistry > Module 03: Molecules and Compounds > Flashcards

Module 03: Molecules and Compounds Flashcards

1
Q

An atom’s valence electrons are located in the atom’s innermost energy level. (3 points)

  1. True
  2. False
A

False

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2
Q

An atom has the following electron configuration.

1s22s22p63s23p4

How many valence electrons does this atom have? (4 points)

  1. 2
  2. 4
  3. 6
  4. 12
A
  1. 6
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3
Q

An atom’s Lewis dot structure has two dots. Which of the following elements could it be, and why? (4 points)

  1. Calcium, because it is an alkaline earth metal with two inner shell electrons.
  2. Carbon, because it has two electrons in its outermost p sublevel.
  3. Lithium, because it is a group 1 element with two bonding electrons.
  4. Magnesium, because it is a group 2 element with two valence electrons.
A

4. Magnesium, because it is a group 2 element with two valence electrons.

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4
Q

The electron configuration of an element is 1s22s22p4. Describe what most likely happens when two atoms of this element move toward each other. (5 points)

A

This element (oxygen) has a total of 8 electrons, 2 in the innermost electron level, and 6 (out of 8) in the valence shell. Since it is on the relative right side of the periodic table, the element will not be as reactive; furthermore, since it needs 2 electrons to fill its valence shell, it is an anion (negative ion). If an identical element moves towards it, which also wants two electrons, the two elements likely react chemically and create a covalent bond, where they share 2 electrons to fill their valence shells. Therefore, the most likely result would be that the elements form a diatomic molecule, with covalent bonds, sharing two electron pairs.

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5
Q

Valence electrons are involved in chemical bonding. (3 points)

  1. True
  2. False
A
  1. True
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6
Q

An atom’s Lewis dot structure has three dots. Which of the following elements could it be, and why? (4 points)

  1. Aluminum, because it is in group 13 and has three valence electrons.
  2. Lithium, because it is a group 1 element with three total electrons.
  3. Magnesium, because it is in period 3 and has three valence electrons.
  4. Potassium, because it is an alkali metal and has three inner shell electrons.
A
  1. Aluminum, because it is in group 13 and has three valence electrons.
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7
Q

The electron configuration of an element is 1s22s22p63s1. Describe what most likely happens when an atom of this element comes near an atom having seven valence electrons. (5 points)

A

The above atom has 11 total electrons, meaning that the first energy level has 2 electrons, the second 8 electrons, and the third 1 (valence) electron. Since there is one valence electron, this atom is in column one, meaning it is very reactive. For an atom to be stable (according to Lewis’s octet rule), the outermost energy shell requires 8 electrons. Therefore, if this element comes into contact with 7 valence electrons, it will give up the outer electron so that the original element only has 8 valence electrons. The other element has 8 as well. The elements will have an ionic bond because one gave away an electron to become a negative ion, and one gained an electron to become a positive ion.

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8
Q

What type of ions do nonmetals naturally form? (3 points)

  1. Negative ions, by gaining electrons to fill the valence shell
  2. Negative ions, by losing electrons to empty the valence shell
  3. Positive ions, by gaining electrons to fill the valence shell
  4. Positive ions, by losing electrons to empty the valence shell
A
  1. Negative ions, by gaining electrons to fill the valence shell
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9
Q

What is the formula of the compound formed between chlorine (Cl) and calcium (Ca)? (3 points)

  1. CaCl, because calcium loses one electron and chlorine gains one electron.
  2. ClCa, because chlorine gains one electron and calcium loses one electron.
  3. CaCl2, because calcium loses two electrons and chlorine gains one electron.
  4. ClCa2, because chlorine gains one electron and calcium loses two electrons.
A

3. CaCl2, because calcium loses two electrons and chlorine gains one electron.

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10
Q

Which of the following is a correct formula unit of an ionic compound? (3 points)

  1. Al2O3
  2. Ca2O
  3. MgOH
  4. NaCl2
A
  1. Al2O3
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11
Q

What is the formula unit for a compound made from Pb4+ and oxygen? (3 points)

  1. PbO2
  2. O2Pb
  3. Pb4O2
  4. O4Pb2
A
  1. PbO2
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12
Q

A student made the Lewis dot diagram of a compound as shown.

What is the error in the Lewis dot diagram? (3 points)

  1. The number of dots around Cl should be six because it is receiving two electrons from Mg.
  2. The number of dots around Mg should be one because there is only one Cl around Mg atom.
  3. Another Cl should be shown around Mg that will transfer its unpaired electron to Mg.
  4. Another Cl should be shown around Mg that will receive the second electron on Mg.
A

4. Another Cl should be shown around Mg that will receive the second electron on Mg.

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13
Q

Potassium has a 1+ charge, and oxygen has a 2− charge. A Lewis dot diagram should contain two potassium atoms and one oxygen atom to show how these atoms form an ionic bond. (1 point)

True

False

A

True

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14
Q

Define Chemical Bond:

A

Link between 2 atoms resulting in mutual attraction of nuclei for valence electrons

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15
Q

Define Valence Electrons:

A

Electrons in outermost shell of atom → lost or shared with another atom

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16
Q

What is Octet Rule (Specifically for group 01, 02, and 18)?

A

Gilbert Lewis

Electrons outer shell key chemical bonding

“Atoms of all elements have between 1- 8 valence electrons”

Group 01: 1 valence

  • reactive
  • transfer of electrons = chemical reaction

Group 02: 2 valence

Group 18: 8 valence

  • must unreactive
  • (according to Lewis) due to full outer shell
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17
Q

What is the difference between a ionic bond and a covalent bond?

A

Ionic Bonds

Results from:

  1. electrostatic attraction between + & - ions
  2. Electrons given up by one elements to be gained by another

= atoms attracted

mostly metals

Covalent Bonds

Electrons shared between 2 atoms

  • neither completely gaining/losing electrons
  • Outer energy shells overlap

Nonmetals

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18
Q

How does reactivity decrease/increase across the periodic table?

A

Decrease from left to right

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19
Q

How do the valence electrons appear on:

  1. Column 01
  2. Column 02
  3. Transition Metals
  4. Colum 3-7
  5. Colum 08
A

Column 01: 1 valence electron

Column 02: 2 valence electrons

Transition Metals:

columns not indicate valence electron

Go along group → increase of one electron

  • left: reactive
  • right: less reactive

Column 03 - 07: column = nom. valence electrons

Column 08:

  • helium = 2 valence electrons
  • others = 8 valence electrons
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20
Q

How does valence electrons compare in the subshell s & p and d & f?

A

subshell s & p: often

d and f → harder to bond → rarly reactive

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21
Q

What is Ionization Energy?

A

Ionization Energy: required to remove an electron (gas)

  • remove highest energy electron
  • left to right: increase
  • top to bottom: decrease

Indicate how they react to change:

the difference in first energy = indicate type of bond form

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22
Q

Define Electronegativity:

A

Electronegativity: (opposite) Measures tendency to attract electrons

  • left to right: increase
  • top to bottom: decrease

Elements similar E energy: Covalent

Similar E energy: Ionic

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23
Q

What is Noble Gas Notation and what are the three steps?

A

Full atomic configurations = very long

  • rather focus valence electrons
  • abbreviated from = Noble Gas Notation

Step 01: Fist the last element (noble gas) from previous row

Step 02: use noble gas in shorthand; write in brackets

Step 03: Delete the noble gas full notation and only write the elements configuration from there.

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24
Q

What are Cations, Neutral Atoms, and Anions?

A

Ionic Bond: transferral of 1+ electrons between atoms

  • Cations (+) and anions (-) attract
  • due to electrostatic forces

Cations

  1. losses electron
  2. more protons

Neutral Atoms

protons = electrons

Anions

  1. gains electron
  2. more negative
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25
Q

How do metals and nonmetals compare in their electronegativity?

A

Metals positive charge = number valence electrons

Nonmetals negative charge = number electron need fill valence shell

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26
Q

Which two factors influence ionic bonds?

A
  1. Electronegativity
  2. Ionization energy
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27
Q

How does electronegativity relate to ionic and covalent bonding?

A

Ionic Bond: difference in electronegativity of 1.7 - 4.0

Covalent Bond: difference of less than 1.7

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28
Q

Define Ionization energy?

A

The energy required to remove an electron

Few electrons → lose electrons

generally metals

Almost full → attract electrons

generally nonmetals

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29
Q

What are the steps to determine the Formula Unit?

A

Chemical formula used to determine ionic compounds

Step 01: Identify the charge of each ion

Step 02: Write cation first + anion

(corresponds to most metals then nonmetals)

Step 03: determine the ratio of positive to negative ions needed to make the compound neutral

Crossing the charges method:

  • number of the charge of cation subscript of anion
  • visa versa

Step 04: Subscripts represent the lowest whole number ratio

Step 05: Check to see if the net charge is zero

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30
Q

What are polyatomic Ions?

A

Polyatomic Ions: atoms bond together in a covalent bond → overall +/- charge

Due to attraction to opposite charged ions → join with single-atom ions/polyatomic ions = ionic compound

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31
Q

Explain the nature of non-metal covalent bonding:

A

Nonmetals → share electrons that overlap in half-filled orbitals from their valence shell

  • Gasses, liquids → covalent
  • gives both a full outer shell
  • stable configuration of noble gasses
  • attracted to nucleus of other atoms
  • Double/Tripple Covalent Bonds: share 2/3 electrons
  • Form between atoms → similar electronegativity
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32
Q

Define Diatomic molecules and the 7 types:

A

Diatomic Molecules: molecule 2 atoms of the same/different chemical element

7 diatomic molecules: (I Bought Clay For Our New House)

  1. Iodine
  2. Bromine
  3. Chlorine
  4. Fluorine
  5. Oxygen
  6. Nitrogen
  7. Hydrogen
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33
Q

What is the difference between single, double, and triple covalent bonding?

A

Single Bonds

  • Covalent bond one pair of electrons are shared

Double Bonds

  • Covalent bond two pairs of electrons shared

Triple Bonds

  • Covalent bond three pairs are shared between

Incease in shared electrons → increase bong strength

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34
Q

What are the 4 steps to create a Lewis Dot Structure?

A

Step 01: Count the number of valence electrons

Step 02: Determine the amount needed to complete the octet rule

Step 03: Place least electronegative element in the center of the molecule

except hydrogen

Step 04: Indicate shared electron

shared electron pair: H — H (line)

Lines increase with amount of shared electrons: H = H

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35
Q

What is the difference between Polar and Nonpolar Covalent Bonding?

A

Polar Covalent Bonds

  • Nonmetals share electrons nonequally
  • one higher electronegativity than other (0.5 < x - y < 1.7)
  • electrons spend more time near higher electronegative element

Otherside: partially positive

Nonpolar Covalent Bonds

  • Nonmetals share electrons equally
  • bonded atoms same elements
  • similar electronegavitity (x-y < 0.5)
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36
Q

How do ionic and covalent bonds compare when dissolving in water?

A

Ionic: Yes

Covalent: Varies

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37
Q

How do ionic and covalent bonds compare in the compound of consistency?

A

Ionic: Brittle

Covalent: Soft

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38
Q

Melting and boiling points of ionic and covalent bonds?

A

Ionic: high

Covalent: low

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39
Q

What is true of a covalent bond? (4 points)

  1. It is the electrostatic attraction between oppositely charged particles.
  2. It is the sharing of electrons by overlapping orbitals.
  3. It involves the exchange of electrons from one atom to another.
  4. It involves the sharing of neutrons between two nuclei.
A

2. It is the sharing of electrons by overlapping orbitals.

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40
Q

A single covalent bond involves two atoms sharing one pair of electrons. (2 points)

True or False

A

True

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41
Q

The molecule CH2O contains two single bonds and one double bond. (2 points)

True or False

A

True

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42
Q

When two fluorine atoms bond together in F2, what type of covalent bond do they form? (4 points)

  1. A double bond, because they overlap orbitals to share one pair of electrons.
  2. A double bond, because they overlap orbitals to share two pairs of electrons.
  3. A single bond, because they overlap orbitals to share one pair of electrons.
  4. A single bond, because they overlap orbitals to share two pairs of electrons.
A

3. A single bond, because they overlap orbitals to share one pair of electrons.

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43
Q

The table provides the number of valence electrons for each of the two atoms that form an ionic and a covalent compound.

Composition of Compounds

Compound C

  1. Atom 1 has seven
  2. Atom 2 has two

Compound D

  1. Atom 1 has six
  2. Atom 2 has five

Which of the following statements is true about one of the compounds? (4 points)

  1. Compound C is ionic because both atoms are in need of electrons.
  2. Compound D is covalent because both atoms are in need of electrons.
  3. Compound D is ionic because one atom is in need of electrons and the other needs to lose electrons.
  4. Compound C is covalent because one atom is in need of electrons and the other needs to lose electrons.
A

2. Compound D is covalent because both atoms are in need of electrons.

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44
Q

An induced dipole occurs when one molecule with a permanent dipole repels another molecule’s electrons, causing the electrons to be more concentrated on one end of the molecule than another. (4 points)

True

False

A

True

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45
Q

What type of intermolecular force occurs between polar molecules? (4 points)

  1. Dipole-dipole force
  2. Hydrogen bonding
  3. Induced dipole force
  4. Polar covalent bonding
A

1. Dipole-dipole force

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46
Q

What is the strongest intermolecular force that occurs between molecules of H2S? (4 points)

  1. Covalent bonding
  2. Dipole-dipole force
  3. Hydrogen bonding
  4. London dispersion force
A
  1. Dipole-dipole force
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47
Q

The electronegativity values of fluorine, oxygen, and hydrogen are compared in the table.

Comparison of Electronegativity

Fluorine: 4.0

Oxygen: 3.5

Hydrogen: 2.1

Which of the following statements is true about the strength of the hydrogen bonding in HF and H2O? (4 points)

  1. HF ≥ H2O because δ− on O in the HO bond is greater than δ− on F in the HF bond.
  2. HF < H2O because the radius of H in HO is shorter than the radius of H in HF.
  3. HF < H2O because F in HF has an extra lone pair compared with O in H2O.
  4. HF ≥ H2O because the HF bond is more polar than the HO bond.
A

4. HF ≥ H2O because the HF bond is more polar than the HO bond.

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48
Q

An induced dipole occurs when a molecule’s moving electrons are briefly more concentrated in one place than another, causing the molecule to become temporarily polarized. (4 points)

True or False

A

False

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49
Q

When comparing H2, NH3, O2, and CH4, which of the following statements is correct? (4 points)

  1. CH4 has the highest boiling point because it experiences dipole-dipole forces.
  2. H2 has the strongest intermolecular forces because it has the lowest mass.
  3. NH3 has the highest boiling point because it experiences hydrogen bonding.
  4. O2 has the strongest intermolecular force because it experiences London dispersion forces.
A

3. NH3 has the highest boiling point because it experiences hydrogen bonding.

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50
Q

Which statement is true for dipole-dipole forces? (4 points)

  1. They are stronger than hydrogen bonding forces.
  2. They are weaker than London dispersion forces.
  3. They occur between ions and polar molecules.
  4. They occur between polar molecules.
A

4. They occur between polar molecules.

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51
Q

How does the electronegativity indicate the type of bonding?

A

Covalent: elements difference in electronegativity < 1.7

Ionic bond: elements difference in electronegavitity > 1.7

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52
Q

What are the general trend in the periodic table regarding type of bonding?

A

nonmetals → covalently

metals → ionically with nonmetals

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53
Q

What are Binary Ionic Compounds?

A
  1. compound composed of two different elements
  2. bond due to electrostatic attraction and transferral or electrons
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54
Q

What are the two steps in naming binary ionic compounds?

A

Step 01: Element form cation = first word in compound

Step 02: negative ion named second

  • shorten root word
  • add -ide end
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55
Q

What is the Stock system to name metal ionic compounds?

A

Used for transition metals in the d block → multiple possible names for positive ions

Stock system: use roman numeral after first element in compound to indicate the amount of change in the atom

Roman numeral (I) → 1+ charge in first compound

Roman numeral (II) → 2+ charge second compound

….

In copper (I) oxide, the final ratio is 2:1.

In copper (II) oxide, the ratio of 2:2 →1:1.

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56
Q

What are the three steps to naming covalent compounds?

A

Step 01: Add prefix to name the first element

  • Represent the number of atoms of an element in bonds*
  • one atom in the first element: no prefix

Step 02: Add prefix to represent the number atoms second element

add to the root

  • add even if the second element has only one atom (mono)
  • Step 03: Add the ending -ide to the last element
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57
Q

Sulfur dioxide is a covalent compound. (3 points)

True

False

A

True

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58
Q

What is the correct name for CH4? (3 points)

  1. Carbon tetrahydride
  2. Carbon (IV) hydride
  3. Monocarbon tetrahydride
  4. Monocarbon hydroxide
A

1. Carbon tetrahydride

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59
Q

What is the correct name for FeCl3? (3 points)

  1. Iron (I) chloride
  2. Iron (III) chloride
  3. Iron trichloride
  4. Iron chlorate
A

2. Iron (III) chloride

60
Q

What is the formula for potassium nitrate? (3 points)

  1. KN
  2. K3N
  3. KNO2
  4. KNO3
A

4. KNO3

61
Q

Formula for Lithium perchlorate:

A

LiClO4

62
Q

Formula for Lithium chlorite:

A

LiClO2

63
Q

Formula for Lithium chloride

A

LiCl

64
Q

Pure carbon commonly occurs in two forms: strong diamonds and soft, brittle graphite. The graphite is much more brittle because its carbon atoms are held together by single bonds, compared to double bonds in diamonds. (2 points)

True

False

A

False

65
Q

What functional group consists of a carbon atom double-bonded to an oxygen atom? (3 points)

  1. Carbohydrate group
  2. Carbonyl group
  3. Hydroxyl group
  4. Ketone group
A

2. Carbonyl group

66
Q

CH2OCH2 is an organic compound with an oxygen atom bonded between the two carbon atoms, and it is not very soluble in water. What type of compound is this? (3 points)

  1. Alcohol
  2. Amine
  3. Carbohydrate
  4. Ether
A

4. Ether

67
Q

What organic compound it:

Contains a nitrogen bonded to carbon(s) and is usually basic

A

Amine

68
Q

What organic compound it:

Extremely long molecule chain with repeated molecular units

A

Polymer

69
Q

What type of organic compound is:

Makes up cell walls, fats, or amino acids

A

Carbohydrate

70
Q

What type of organic compound is:

Organic compound with an oxygen bonded between two carbons

A

Ether

71
Q

In a certain organic compound, one of the carbon atoms is bonded to four atoms. One of these is a carbon atom, and the other three are hydrogen atoms. What type of bond exists between the two carbon atoms? (3 points)

  1. Ionic
  2. Dispersion force
  3. Double covalent
  4. Single covalent
A

4. Single covalent

72
Q

A compound has the molecular formula C3H7OH. Which class of organic compounds does it belong to? (3 points)

  1. Alcohols
  2. Amines
  3. Carbohydrates
  4. Hydrocarbons
A

1. Alcohols

73
Q

The polarity of an oxygen-hydrogen bond is higher than the polarity of a nitrogen-hydrogen bond, allowing amines to be more soluble than alcohol. (2 points)

True or False

A

False

74
Q

Carbon atoms naturally bond with each other in chains, rings, or networks, but they cannot bond with oxygen or nitrogen. (2 points)

True

False

A

False

75
Q

What functional group consists of a carbon atom double-bonded to an oxygen atom? (3 points)

  1. Carbohydrate group
  2. Carbonyl group
  3. Hydroxyl group
  4. Ketone group
A

2. Carbonyl group

76
Q

CH3CH2OH is an organic compound that is soluble in water. What type of compound is this? (3 points)

  1. Alcohol
  2. Amine
  3. Ether
  4. Hydrocarbon
A

1. Alcohol

77
Q

In a certain organic compound, one of the carbon atoms is bonded to four atoms. One of these is a carbon atom, and the other three are hydrogen atoms. What type of bond exists between the two carbon atoms? (3 points)

  1. Ionic
  2. Dispersion force
  3. Double covalent
  4. Single covalent
A

4. Single covalent

78
Q

A compound has the molecular formula C3H8. Which class of organic compounds does it belong to? (3 points)

  1. Alcohols
  2. Amines
  3. Ethers
  4. Hydrocarbons
A

4. Hydrocarbons

79
Q

Hydrocarbons, the carbonyl group, and carbohydrates all have carbon, and they only differ based on the type of carbon-carbon bonds that exist in the molecule. (2 points)

True

False

A

False

80
Q

Define the properties of carbon’s electrons:

A
  • 4 valence electrons
  • Strong tendency to make 4 bonds
  • Bonds: plates, networks, chains, rings
  • What: hydrogen, oxygen, nitrogen, sulfur, phosphorous
81
Q

What are the two types of pure carbon

A
  1. Diamond
  2. Graphine
82
Q

What are the properties of diamonds?

A

Hardest known substance

Solid: colorless & high density

Bond:

  • single
  • three-dimensional tetrahedral

No intermolecular forces (is covalent)

83
Q

What are the properties of graphine?

A

Looks: Soft solid, black

Conductivity: good

Arrangement:

  • layers of thin hexagonal “plates”
  • 1 double bond & 2 single bonds
  • trigonal planar shape

Intermolecular forces:

  • weak London dispersion forces
  • soft and easily broken
84
Q

What is organic chemistry?

A

Study of carbon

85
Q

What are the functional groups of carbon (definition)?

A

Functional Groups: covalently bonded atoms within molecules responsible for chemical characteristics

  • unique molecular structures
  • undergo similar chemical reactions no matter what molecule it bonds with
  • Exception: functional group bonded to another functional graph*
86
Q

What are the types of Functional Groups? [7]

A
  1. Hydrocarbons
  2. Alcohols
  3. Amines
  4. Ethers
  5. Carbonyl Groups
  6. Carbohydrates
  7. Polymers
87
Q

What are hydrocarbons?

A

Contains only carbon and hydrogen

Examples

  1. Methane (CH4)
    • simplest
    • main component natural gas
  2. Octane (C8H18)
    • component of gasoline

Large diversity → of different type of bonding

  • chains or rings

Bonding:

  • single, double, triple
88
Q

What are alcohols?

A

Hydroxyl group bonded with the carbon atom

Polarity in hydrogen-oxygen bonds → smaller alcohol compounds soluble in water

  • ex: ethanol (C2H5OH)
89
Q

Define “hydroxyl group:”

A

oxygen atom bonded with a hydrogen atom

90
Q

What are the Amine Groups?

A

Amine Groups: Nitrogen atom bonded with 1,2,3 carbon(s)

less soluble in water than alcohol

lower polarity

basic

Ex: Alkaloids

  • in plants or marine organisms
  • medical effects

Ex: caffeine

91
Q

What are “Ethers?”

A

Oxygen atom bonded between two carbon atoms

  • not soluble in water (not form hydrogen bonds with oxygen)
  • Little polarity
  • little attraction
  • bow boiling points
92
Q

What are Carbonyl Groups?

A

Carbon atom double-bonded to oxygen atom

Categories:

  • ketone, aldehyde, amide, carboxylic acid, or ester
  • Ex: Acetone (CH3COCH3)
    • nail polish remover
93
Q

What are polymers?

A

Repeated molecular units → monomers

  • very long (4-100 atoms)
  • too small to see with the eye

Synthetic Polymers:

  • human-made plastic
  • variety of uses
94
Q

What are “Carbohydrates?”

A

Carbon, hydrogen, and oxygen atoms

  • most abundant
  • forms more complex structures

Empirical Formula: CH2O

Ex:

  • cell walls of bacteria
  • exoskeletons of invertebrates
  • energy storage
  • makes up fats and amino acids
95
Q

An instantaneous dipole occurs when a molecule’s moving electrons are briefly more concentrated in one place than another, causing the molecule to become temporarily polarized. (4 points)

True

False

A

True

96
Q

What is the strongest intermolecular force that occurs between molecules of CO2? (4 points)

  1. Dipole-dipole
  2. Induced dipoles
  3. Ionic bonding
  4. London dispersion
A

4. London dispersion

97
Q

The boiling points of diatomic halogens are compared in the table.

Which of the following statements best explains the trends in boiling points? (4 points)

  1. The atomic size increases down the group, and this decreases the strength of the intermolecular forces.
  2. The total number of electrons decreases down the group, and this decreases the strength of the intermolecular forces.
  3. The total number of electrons increases down the group, and this increases the strength of the intermolecular forces.
  4. The chances of forming a permanent dipole increase down the group, and this increases the strength of the intermolecular forces.
A

3. The total number of electrons increases down the group, and this increases the strength of the intermolecular forces.

98
Q
A
99
Q

Define ‘Chemical Bond:’

A

Link between 2 atoms resulting in mutual attraction of nuclei for valence electrons

100
Q

Define Valence Electron:

A

Electrons in outermost shell of atom → lost or shared with another atom

101
Q

What rule did Gibert Lewis come up with in 1916

A

Octet Rule:

Electrons outer shell key chemical bonding

“Atoms of all elements have between 1- 8 valence electrons”

Group 01: 1 valence

  • reactive
  • transfer of electrons = chemical reaction

Group 02: 2 valence

Group 18: 8 valence

  • must unreactive
  • (according to Lewis) due to full outer shell
102
Q

What are the two types of chemical bonding?

A
  1. Ionic Bonding
  2. Covalent Bonding
103
Q

What is Ionic Bonding?

A
  1. electrostatic attraction between + & - ions
  2. Electrons are given up by one element to be gained by another

= atoms attracted

mostly in metals

104
Q

What are covalent bonds?

A

Electrons shared between 2 atoms

  • neither completely gaining/losing electrons
  • Outer energy shells overlap
  • Mostly nonmetals
105
Q

How does the outermost energy shell relate to electron configuration?

A

highest energy level

electrons move between atoms & shared = chemical change

106
Q

What periodic trend is seen between reactivity and valence electrons?

A

Reactivity decreases from left to right

Valence electrons increase from left to right

107
Q

How does columns convey the nature of an element’s valence electrons?

A

Column 01: 1 valence electron

Column 02: 2 valence electrons

Transition Metals:

  • columns not indicate valence electron
  • Go along group → increase of one electron

left: reactive
right: less reactive

Column 03 - 07: column = nom. valence electrons

Column 08:

  • helium = 2 valence electrons
  • others = 8 valence electrons
108
Q

How does the type of subshell relate to valence electrons and reactivity?

A

Valence electrons:

  • subshell s & p: often
  • d and f → harder to bond → rarly reactive
109
Q

How does ionization energy compare to electronegativity?

A

Ionization Energy: requried to remove an electron (gas)

  • remove highest energy electron
    • left to right: increase
    • top to bottom: decrease
  • Indicate how they react to change:
  • difference in first energy = indiate type of bond form

Electronegativity: (opposite) Measures tendency to attract electrons

  • left to right: increase
  • top to bottom: decrease
    • Elements similar E energy: Covalent
    • Similar E energy: Ionic
110
Q

How does electronegativity relate to chemical bonding?

A

Elements similar E energy: Covalent

Similar E energy: Ionic

111
Q

Neon is located in the last group of the periodic table. How many valence electrons does the element neon have? (4 points)

  1. 1
  2. 2
  3. 4
  4. 8
A

4. 8

112
Q

The table shows the total number of electrons in Atom A and Atom B.

Which statement is correct? (4 points)

  1. A will give up electrons to form bonds.
  2. B will give up electrons to form bonds.
  3. Both A and B will be chemically unreactive.
  4. Both A and B will gain electrons to become stable
A

3. Both A and B will be chemically unreactive.

113
Q

What is the charge on an atom after it gains two electrons during the formation of a bond? (4 points)

  1. One positive charge
  2. Two positive charges
  3. Two negative charges
  4. One negative charge
A

3. Two negative charges

114
Q

What happens when the compound MgO is formed? (4 points)

  1. Oxygen transfers two electrons to magnesium.
  2. Oxygen receives two electrons from magnesium.
  3. Magnesium forms an ion with −1 charge; oxygen forms an ion with +1 charge.
  4. Magnesium forms an ion with +1 charge; oxygen forms an ion with −1 charge.
A

2. Oxygen receives two electrons from magnesium.

115
Q

Define ionization energy.

Describe how ionization energy impacts ionic bonding.

A

Ionization energy is the energy required to remove an electron from an atom, and on the periodic table, the trend is that ionization energy (similar to electronegativity) increases from left to right and increases from the bottom to the top. Ionization energy is very relevant in ionic bonding. For example, metals on the left side of the periodic table require less ionization energy than the nonmetals on the right to lose an electron, which is why metals are cation rather than anions because they are very willing to give up electrons. In contrast, noble gasses which already are in a “noble gas state” and do not need to lose or gain electrons to fill their valence electron shells, require immense ionization energy to remove electrons.

116
Q

What is the formula unit for a compound made from Li and Cl? (4 points)

  1. LiCl because the total negative charge on Cl is one.
  2. LiCl because the total negative charge on Li is two.
  3. Li2Cl because the total positive charge on Cl is one.
  4. Li2Cl because the total positive charge on Li is two.
A

1. LiCl because the total negative charge on Cl is one.

117
Q

The Lewis dot notation for two atoms is shown.

What is represented by this notation? (4 points)

  1. Mg gains two protons from O.
  2. Mg donates two protons to O.
  3. Mg gains two electrons from O.
  4. Mg donates two electrons to O.
A

4. Mg donates two electrons to O.

118
Q

Which phrase best describes the bond in O2? (4 points)

  1. Double covalent bond
  2. Single covalent bond
  3. Double ionic bond
  4. Single ionic bond
A

1. Double covalent bond

119
Q

What best describes the bonding in a water molecule? (4 points)

  1. An oxygen atom shares an electron pair with each H atom.
  2. An oxygen atom shares a single electron with each H atom.
  3. An oxygen atom receives an electron from each H atom.
  4. An oxygen atom transfers an electron to each H atom.
A

1. An oxygen atom shares an electron pair with each H atom.

120
Q

What best explains the formula unit for a compound made from fluorine and hydrogen? (4 points)

  1. HF, because fluorine is short of one electron, and hydrogen is in excess of one electron.
  2. HF, because both fluorine and hydrogen are capable of forming only one covalent bond.
  3. H2F, because fluorine is short of two electrons, and hydrogen is short of one electron.
  4. H2F, because fluorine is capable of forming one, and hydrogen is capable of forming two covalent bonds.
A

2. HF, because both fluorine and hydrogen are capable of forming only one covalent bond.

121
Q

Look at this image.

What do the lines in this image represent? (4 points)

  1. Ionic bonds between carbon and oxygen
  2. Non-bonded valence electrons of oxygen
  3. Double covalent bonds in carbon dioxide
  4. Valence electrons donated in carbon dioxide
A

3. Double covalent bonds in carbon dioxide

122
Q

What does the second word in the name of a binary ionic compound represent? (4 points)

  1. The group 1 element
  2. The negative ion
  3. The positive ion
  4. The metal
A

2. The negative ion

123
Q

What is the name of a compound having the formula CaCl2? (4 points)

  1. Calcium chloride
  2. Calcium dichloride
  3. Calcium chlorate
  4. Calcium perchlorate
A

1. Calcium chloride

124
Q

What does this image represent? (4 points)

  1. Linear molecule with one domain
  2. Linear molecule with two domains
  3. Tetrahedral molecule with four domains
  4. Trigonal planar molecule with three domains
A

4. Trigonal planar molecule with three domains

125
Q

Which of the following explains the VSEPR geometry of an ammonia molecule? (4 points)

  1. It is tetrahedral because there are four bonded pairs around nitrogen.
  2. It is trigonal pyramidal because there are four bonded pairs around nitrogen.
  3. It is tetrahedral because there are three bonded pairs and one lone pair around nitrogen.
  4. It is trigonal pyramidal because there are three bonded pairs and one lone pair around nitrogen.
A

4. It is trigonal pyramidal because there are three bonded pairs and one lone pair around nitrogen.

126
Q

Which of the following are electrostatic interactions of permanent dipoles in polar molecules? (4 points)

  1. Ion-dipole forces
  2. Hydrogen bonding
  3. Dipole-dipole forces
  4. London dispersion forces
A

3. Dipole-dipole forces

127
Q

The boiling point of chlorine is −34 °C. Which of the following best predicts the boiling point of iodine? (4 points)

  1. Higher than −34 °C because dispersion forces are stronger in iodine due to a greater number of electrons.
  2. Lower than −34 °C because chlorine is more polar than iodine on account of its higher electronegativity.
  3. Higher than −34 °C because dipole-dipole interactions in iodine are stronger than dispersion forces in chlorine.
  4. Lower than −34 °C because permanent dipoles created in chlorine are stronger than temporary dipoles in iodine
A
  1. Higher than −34 °C because dispersion forces are stronger in iodine due to a greater number of electrons.
128
Q

What type of element is carbon? (4 points)

  1. Chemically unreactive
  2. Impure
  3. Metal
  4. Nonmetal
A

4. nonmetal

129
Q

What is organic chemistry? Name at least three categories of compounds that are studied as a part of organic chemistry. (8 points)

A

Organic chemistry is the study of carbon and its presence in the environment. There are different “functional groups under organic chemistry,” which are groups of covalently bonded atoms with molecules responsible for chemical characteristics that make that molecular structure unique. There are 6 types of functional groups in organic chemistry, namely Hydrocarbons, Alcohols, Amines, Ethers, Polymers, Carbonyl Groups, and Carbohydrates.

Hydrocarbons are compounds that contain both carbon and hydrogen atoms, such as methane. Alcohols are compounds that consist of the Hydroxyl group (an oxygen and hydrogen atom) bonded with carbon, which is quite soluble in water and has high polarity due to the hydrogen-oxygen bonding. Amines consist of a nitrogen atom bonded with up to three carbon atoms; they are less soluble and less polar than alcohol. Ethers consist of an oxygen atom between two carbon atoms, which are not soluble in water, have little polarity, and have a low boiling point.

130
Q

What does this image represent? (4 points)

  1. Alcohol group
  2. Carbonyl group
  3. Ether group
  4. Hydroxyl group
A

1. Alcohol group

131
Q

In an experiment, two unknown compounds (one an alcohol and the other an amine) of equal molecular mass were heated. The result of the experiment shows that Compound A boiled at a lower temperature than Compound B.

Which of the following correctly explains the identity of Compound A and why this was the result? (4 points)

  1. It is an amine; it contains nitrogen-hydrogen bonds that are less polar and oxygen-hydrogen bonds.
  2. It is an alcohol; it contains nitrogen-hydrogen bonds that are less polar and oxygen-hydrogen bonds.
  3. It is an alcohol; it contains oxygen-hydrogen bonds that are less polar and nitrogen-hydrogen bonds.
  4. It is an amine; it contains oxygen-hydrogen bonds that are less polar and nitrogen-hydrogen bonds.
A
  1. It is an amine; it contains nitrogen-hydrogen bonds that are less polar and oxygen-hydrogen bonds.
132
Q

Lithium is located in the first group of the periodic table. How many valence electrons does the element lithium have? (4 points)

1

2

4

8

A

1

133
Q

The electron configuration of an element is shown below.

1s22s22p63s1

Name the group this element belongs to in the periodic table and explain your answer.

Based on the electron configuration, write one chemical property of this element. (8 points)

A

The element above has 11 electrons, 2 in the innermost energy-level, 8 in the middle energy-level, and 1 valence electron. The Octet Rule, posed by Gilbert Lewis in 1916, states that valence electrons are equal to their corresponding group on the periodic table (except transition metals, which has some variation). Therefore, according to the Octet Rule, this element is in Group 1 of the periodic table (Alkali Metals).

The Alkali Metals are the most reactive elements on the periodic table, and since it has one valence electron, it will likely become a cation (a positive ion) by transferring the electron, in order to be in a stable state. Therefore, this element is very reactive and will likely not occure in its pure form in nature (because it requires little ionization energy to remove an electron).

134
Q

What is the charge on an atom after it gains two electrons during the formation of a bond? (4 points)

  1. One positive charge
  2. Two positive charges
  3. Two negative charges
  4. One negative charge
A

3.

  1. Two positive charges
  2. Two negative charges
135
Q

What happens when the compound NaCl is formed? (4 points)

  1. Sodium transfers an electron to chlorine.
  2. Sodium receives two electrons from chlorine.
  3. Sodium forms an ion with −1 charge and chlorine forms an ion with +1 charge.
  4. Sodium forms an ion with +2 charge and chlorine forms an ion with −2 charge.
A

1. Sodium transfers an electron to chlorine.

136
Q

Which of these statements best describes the formula unit for a compound made from Mg and Cl? (4 points)

  1. It is MgCl2 because the total negative charge on Cl is one.
  2. It is Mg2Cl because the total negative charge on Mg is one.
  3. It is MgCl2 because the total positive charge on Mg is two.
  4. It is Mg2Cl because the total positive charge on Mg is two.
A

3. It is MgCl2 because the total positive charge on Mg is two.

137
Q

What is represented by this notation? (4 points)

  1. Na loses one proton to Cl.
  2. Na loses one electron to Cl.
  3. Na gains two protons from Cl.
  4. Na gains one electron from Cl.
A

2. Na loses one electron to Cl.

138
Q

Which phrase best describes the bond in H2? (4 points)

  1. Double covalent bond
  2. Single covalent bond
  3. Double ionic bond
  4. Single ionic bond
A

2. Single covalent bond

139
Q

What best describes the bonding in a carbon dioxide molecule? (4 points)

  1. Carbon shares two of its electrons, and each oxygen shares four of its electrons.
  2. Carbon shares four of its electrons, and each oxygen shares two of its electrons.
  3. Carbon receives two electrons from each of the two oxygen atoms.
  4. Carbon transfers two electrons to each of the two oxygen atoms.
A

2. Carbon shares four of its electrons, and each oxygen shares two of its electrons

140
Q

What best explains the formula unit for a compound made from nitrogen and hydrogen? (4 points)

  1. NH4, because nitrogen needs four electrons, and each hydrogen needs one electron.
  2. NH4, because nitrogen needs one electron, and each hydrogen needs four electrons.
  3. NH3, because nitrogen forms a single bond with each hydrogen atom.
  4. NH3, because nitrogen forms a triple bond with each hydrogen atom.
A

3. NH3, because nitrogen forms a single bond with each hydrogen atom.

141
Q

What is the name of the compound CaS? (4 points)

  1. Calcium sulfur
  2. Calcium sulfide
  3. Calcium sulfite
  4. Calcium sulfate
A

2. Calcium sulfide

142
Q

What does this image represent? (4 points)

H — H

  1. Linear molecule with one domain
  2. Linear molecule with two domains
  3. Tetrahedral molecule with four domains
  4. Trigonal planar molecule with three domains
A

1. Linear molecule with one domain

143
Q

Which of the following explains the VSEPR geometry of a carbon tetrachloride molecule? (4 points)

  1. It is bent because there are four bonded pairs around carbon.
  2. It is tetrahedral because there are four bonded pairs around carbon.
  3. It is bent because there are two bonded pairs and two lone pairs around carbon.
  4. It is tetrahedral because there are two bonded pairs and two lone pairs around carbon.
A

2. It is tetrahedral because there are four bonded pairs around carbon.

144
Q

Which of the following are dipole-dipole interactions that occur only between molecules containing N-H, O-H or F-H bonds? (4 points)

  1. Ion-dipole forces
  2. Hydrogen bonding
  3. Dipole-dipole forces
  4. London dispersion forces
A

2. Hydrogen bonding

145
Q

The boiling point of bromine is 59 °C. Which of the following best predicts the boiling point of iodine monochloride, a polar compound? (4 points)

  1. Higher than 59 °C because dipole-dipole interactions in iodine monochloride are stronger than dispersion forces in bromine.
  2. Lower than 59 °C because ionic bonding in bromine is stronger than covalent bonding in iodine monochloride.
  3. Lower than 59 °C because dipole-dipole interactions in iodine monochloride are weaker than in bromine.
  4. Higher than 59 °C because ionic bonding in iodine monochloride is stronger than H-bonding in bromine.
A

1.

  1. Higher than 59 °C because dipole-dipole interactions in iodine monochloride are stronger than dispersion forces in bromine.
146
Q

How many valence electrons does carbon have? (4 points)

1

2

4

8

A

4

147
Q

Explain what makes carbon so essential to the life on planet Earth. (8 points)

A

Carbon is the 17th most abundant element in the environment, and in air, water, rocks, fossil fuels, and life on earth (which are all carbon-based molecules). The atom’s unique ability to bond in long chains, plates, networks, and rings makes it the base for multiple larger molecules. Since carbon has 4 valence electrons, it has a strong tendency to create 4 bonds with other atoms, which makes it so essential to life.

Carbon can form 7 different types of functional groups (hydrocarbons, carbonyl groups, carbohydrates, alcohols, amines, polymers, and ethers), which makes it so relevant to life on earth. For example, amines (a nitrogen atom bonded with 1-3 carbon atom(s)) which is prevalent in marine organisms and plants. Carbohydrates, made up of carbon, hydrogen, and oxygen atoms, are the basis for most complex - living - structures, such as cell walls, exoskeletons, and amino acids.

Honors Chemistry (8 decks)

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