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INORGANIC AND ORGANIC CHEMISTRY > CHEMICAL BONDS AND COMPOUNDS > Flashcards

CHEMICAL BONDS AND COMPOUNDS Flashcards

1
Q

Four periodic table sections

A
  • Representative Elements
  • Noble - gas Elements
  • Transition Elements
  • Inner Transition Elements
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2
Q

Compounds are divided into two broad categories:

A

Ionic compounds
Molecular compounds (Covalent)

Note: Certain combinations of elements produces ionic compounds, some other combinations form molecular compounds

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3
Q

the attractive force that holds two atoms together in a more complex unit

A

Chemical bond

note: It is important to note that most bonds are not 100% ionic or 10% covalent

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4
Q

Two types of chemical bond

A

Ionic bonds
Covalent bonds

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5
Q

formed through transfer of one or more electrons from one atom or group of atoms to another

A

Ionic bonds

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6
Q

formed through the sharing of one or more pairs of electrons between two atoms

A

Covalent bonds

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7
Q

There are two fundamental concepts to understanding ionic and covalent bonding models

A
  1. Not all electrons in an atom participate in bonding. Those that do are called valence electrons
  2. Certain arrangements of electrons are more stable than others, as is explained by the octet rule
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8
Q

an electron in the outer-most electron shell of a representative or noble-gas element

A

Valence electron

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9
Q

The number of valence electrons in an atom of a representative element can be determined from the atom’s what

A

electron configuration

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10
Q

the chemical symbol of an element surrounded by dots equal in number to the number of valence electrons present in atoms of the element

A

Lewis symbol

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11
Q

The General Practice in writing lewis symbol

A

The general practice in writing these symbols is to place the first four dots separately on the four sides of the chemical symbol and then begin pairing the dots are further dots are added

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12
Q

Lewis Symbol: Three things to note:

A
  1. Representative elements in the same group of the periodic table have the same number valence electrons
  2. The number of valence electrons for the representative elements is the same as the Roman numeral periodic-table group number
  3. The maximum number of valence electrons for any element is eight
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13
Q

produced as a result of ionic bonding

A

Ions

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14
Q

an atom (or group of atoms) that is electrically charged as a result of the loss or gain of electrons

A

An ion

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15
Q

If an atom gains one or more electrons, it becomes

A

a negatively charged

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16
Q

if an atom loses one or more electrons, it becomes

A

a positively charged

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17
Q

Loss of one, two, or three electrons gives ions

A

with +1, +2, or +3 charges, respectively

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18
Q

Gain of one, two, or three electrons gives ions

A

with -1, -2, or -3 charges, respectively

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19
Q

This kind of atom is containing one, two, or three valence electrons
(Groups IA, IIA, and IIIA) tend to lose electrons to acquire a noble gas electron configuration

A

Metal Atoms

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20
Q

Group IA metals form how many ions

A

1+ ions

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21
Q

Group IIA metals form how many ions

A

2+ ions

22
Q

Group IIIA metals form how many ions

A

3+ ions

23
Q

This kind of atom is containing five, six, or seven electrons
(Groups VA, VIA, and VIIA) tend to gain electrons to acquire a noble gas electron configuration

A

Non-metal atoms

24
Q

Group VIIA nonmetals form how many atoms

A

1- atoms

25
Q

Group VIA nonmetals form how many atoms

A

2- ions

26
Q

Group VA nonmetals form how many ions

A

3- ions

27
Q

Elements in this group would have to gain or lose four electrons to attain stability, but in most cases the bonding that results is more adequately described by the covalent bond model

A

Group IVA

28
Q

Ion formation requires the presence of two elements:

A

a metal that can donate electrons and a nonmetal that can accept electrons

29
Q

The positive and negative ions simultaneously formed from such electron transfer attract one another, forming an

A

ionic compound

30
Q

a combination of Lewis symbols that represents either the transfer or sharing of electrons in chemical bonds

A

Lewis structure

31
Q

Ionic compounds are always

A

NEUTRAL

note: The ratio in which positive and negative ions combine is the ratio that achieves charge neutrality for the resulting compound

32
Q

Formula Writing Rules for Ionic Compounds

A
  1. The symbol for the positive ions is always written first
  2. the charges on the ions that are present are not shown in the formula
  3. The numbers in the formula (subscripts) give the combining ratio for the ions
33
Q

In the solid state, this compound consists of positive and negative ions in such a way that each ion is surrounded by nearest neighbors of the opposite charge

A

Ionic Compound

34
Q

Ionic compounds do not have ______molecules, only an alternating array of positive and negative ions

A

discreet

35
Q

represent the simplest combining ratio for the ions present

A

chemical formulas

36
Q

the smallest whole-number repeating ratio of ions present in an ionic compound that results in charge neutrality

A

formula unit

37
Q

The compounds NaCl, CO2, P4O10 are all what kind of compounds

A

binary compounds

38
Q

an ionic compound in which one element present is a metal and the other element present is a nonmetal

A

binary ionic compound

39
Q

Recognizing and Naming Binary Ionic Compounds: NAMING RULE:

A

the full name of the metallic element is given first, followed by a separate word containing the stem of the nonmetallic element and the suffix –ide.

Ex. NaF - sodium fluoride

40
Q

Name the ff. binary ionic compounds:

A.) MgO
B. Al2S3
C. K3N
D. CaCl2

A

Answers:
a.) magnesium oxide
b.) aluminum sulfide
c.) potassium nitride
d.) calcium chloride

41
Q

Naming Binary Compounds: metals and nonmetals

A
  • So far, it has been assumed that the only behavior allowable for an element is that predicted by the octet rule
  • It is a good assumption for nonmetals and for most representative element metals
  • However, there are other metals that exhibit a less predictable behavior because they are able to form more than one type of ion.
  • For example, iron forms both Fe2+ and Fe3+ ions, depending on the chemical circumstances
  • When naming compounds that contain metals with variable ionic charges, the charge on the metal ion must be incorporated into the name. This is accomplished using Roman numerals
42
Q

Naming Binary Compounds: The chlorides of Fe2+ and Fe3+ (FeCl2 and FeCl3, respectively) are named

A

iron(II) chloride and iron(III) chloride

43
Q

Naming Binary Compounds: CuO is named

A

copper(II) oxide

44
Q

Naming Binary Compounds note

A
  • If you are uncertain about the charge on the metal ion in an ionic compound, use the charge on the nonmetal ion (which does not vary) to calculate it
  • For example in CuO, you can note that the oxide ion carries a -2 charge (because oxygen is in group VIA), this means that the copper ion must have a +2 charge to counterbalance the -2 charge
45
Q

Naming Binary Compounds: how to calculate the metal ion charge

A

For example: AuCl

  1. To calculate the metal ion charge, use the fact that the total ionic charge (both + and -) must add to zero

(gold charge) + (chlorine charge) = 0

  1. The chlorine has a -1 charge (group VIIA), therefore
    (gold charge) + (-1) = 0
  2. Thus, Gold charge = +1
  3. The name of the compound is gold(I) chloride
46
Q

Name the ff. binary ionic compound, each of which contains a metal whose ionic charge can vary:

A. Fe2O3
B. PbO2
C. Cu2S

A

Answers:
A. Iron(III) oxide
B. Lead(IV) oxide
C. Copper(I) sulfide

47
Q

Naming Binary Compounds: Fixed Charge

A
  • You must know which metals exhibit variable ionic charge and which have a fixed ionic charge.
  • The fixed charge metals are those in group IA (+1 ionic charge), those in group IIA (+2 ionic charge) and five others (Al3+, Ga3+, Zn2+, Cd2+, and Ag+)
  • Metals from the diagram form ionic compounds without roman numerals in their names
48
Q

an ion formed from a single atom through loss or gain of electrons (Cl-, Na+, Ca2+)

A

Monoatomic ion

49
Q

an ion formed from a group of atoms (held together by covalent bonds) through loss or gain of electrons (SO42-)

A

Polyatomic ion

50
Q

This ion contains four O atoms and one S atom, and the whole group of five atoms has acquired a charge of -2

A

Polyatomic Ion

51
Q

form between atoms of dissimilar elements (metal + nonmetal)

A

Ionic bonds

52
Q

occurs between similar or even identical atoms (often two nonmetals are involved)

A

Covalent bond

INORGANIC AND ORGANIC CHEMISTRY (7 decks)

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