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Chemistry 101 > Structure & Properties of Ionic & Covalent Compounds > Flashcards

Structure & Properties of Ionic & Covalent Compounds Flashcards

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1
Q

What is an ionic bond?

A

Attractive force due to transfer of 1 or more electrons from one atom to another

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2
Q

What is a covalent bond?

A

Attractive force due to sharing of electrons between atoms

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3
Q

Ionic Bonding

A
  • Electron lost by a metal
  • Electron gained by by a nonmetal
  • two ions formed: cation and anion (of opposite charge =attracted)
  • opposite charged ions held together by electrostatic force
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4
Q

What is a crystal lattice?

A

Positive and negative ions arrange themselves in regular 3D repeating array to produce stable arrangement

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5
Q

Covalent Bonding

A
  • Each atom attains noble gas configuration by sharing electrons
  • Tend to form between atoms with similar tendencies to gain or lose electrons
  • Polar and nonpolar covalent bonding
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6
Q

What are the diatomic elements?

A

Completely covalent bonds (totally equal sharing)
Example: Doctor BrINClHOF
Br2, I2, N2, Cl2, H2, O2, F2

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7
Q

What is polar covalent bonding?

A

Bonds made up of unequally shared electron pairs

Reference notes for symbols

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8
Q

What is electronegativity?

A

Measure of ability of atom to attract electrons in a chemical bond
- higher EN = greater ability to attract electrons than elements with low EN

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9
Q

What is bond polarity?

A

Difference in electronegativity
Bond is:
-Ionic Bond: 🔺EN>1.9
- Polar Covalent Bond: .5🔺EN

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10
Q

What does nomenclature mean? What are the two naming systems?

A

Assignment of correct & unambiguous name to each & every chemical compound

  • ionic compound
  • covalent compound
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11
Q

How do you write the formula for an ionic compound?

A
  1. Determine charge of each ion
    - metals: charge = group #
    - nonmetals: charge = group #-8
    - cations and anions combine to give formula with net change of 0
  2. Name the cation followed by name of anion (change anion suffix to -ide)
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12
Q

What is the stock system?

A

If a cation of the element has several ions of different charges (i.e. transition metals) use a Roman numeral following metal name
- Roman numerals give charge of metal

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13
Q

What are common nomenclature system?

A
  • use -ic to indicate higher of charges that ion might have

- use -ous to indicate lower of charges that ion might have

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14
Q

What are monatomic ions?

A

Ions consisting of a single charged atom

Ex: all alkali metals, all halogen metals, be, ca, al, ag, ba, mg, o, s, n, p

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15
Q

What are polyatomic ions?

A

Jons composed of 2 or more atoms bonded together with an overall positive or negative charge

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16
Q

How to write formulas of an ionic compound from its name?

A
  1. Determine charge of each ion

2. Write formula so resulting compound is neutral

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17
Q

How do you name covalent bonds?

A
  1. Write in order in which they appear in formula
  2. Greek prefix indicates # of each kind of atom:
    - mono=1; di=2; tri=3; tetra=4; penta=5; hexa= 6; hepta=7; octa=8; nona=9; deca=10
  3. If only one atom of a particular element is present in a molecule, prefix mono- is usually omitted in first element
  4. Stem of name of last element is used with suffix -ide
  5. Final vowel in prefix is often dropped before vowel in stem name
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18
Q

What are the physical states of ionic and covalent compounds?

A
  • ionic compound: usually solids at room temp

- covalent compound: usually solids, liquids, gases

19
Q

What is melting point?

A

Temperature at which solid is converted into a liquid

20
Q

What is boiling point?

A

Temperature at which a liquid is converted into a gas

21
Q

What are the melting points of ionic and covalent compounds?

A
  • ionic compounds have higher melting points and boiling points
  • covalent compounds have lower melting points and boiling points
22
Q

What are the structure of ionic and covalent compounds at solid state?

A
  • ionic compounds are crystalline (organized)

- covalent compounds are crystalline (organized) or amorphous (unorganized)

23
Q

What is the difference between covalent and ionic compounds electrical conductivity?

A

Electrolytes: ions present in solution allowing solution to conduct electricity
Nonelectrolytes: covalent solids usually do not dissociate and do not conduct electricity

24
Q

How to draw a Lewis structure?

A
  1. Use chemical symbols for various elements to write skeletal structure of compound
    - least electronegative atom will be placed in central position
  2. Determine number of valence electrons associated with each atom in compound
    - combine valence electrons to determine total # of valence electrons in compound
  3. Connect central atom to each of surrounding atoms with single bonds
  4. Complete octets of all atoms bonded to central atom
    - lone pair: electrons not involved in bonding
  5. If not enough valence electrons to give central atom an octet, move lone pair electrons from terminal atoms to form new bond with central atom
  6. Recheck that all atoms have octet rule satisfied and total # of valence electrons used
25
Q

What are single bonds, double bonds, and triple bonds?

A
  • single bond: one pair of electrons are shared between 2 atoms
  • double bond: 2 pairs of electrons are shared between 2 atoms
  • triple bond: 3 pairs of electrons are shared between z atoms
26
Q

What is bond energy?

A

Amount of energy required to break a bond holding 2 atoms together
Triple bond> double bonds>single bond

27
Q

What is bond length?

A

Distance separating nucleI of 2 adjacent atoms

- single bond>double bond>triple bond

28
Q

What is resonance?

A

Two or more Lewis structures contribute to real structure

29
Q

What are the three exceptions to the octet rule?

A
  1. Incomplete octet: less than 8 electrons around an atom other H
  2. Odd electron: if there is an odd # of valence electrons, it is not possible to give every atom 8 electrons
  3. Expanded octet: an element in 3rd period or below may have 10 and 12 electrons around it
30
Q

What is the VSEPR Theory?

A

Valence shell electron pair repulsion theory

  • used to predict shape of molecules
  • electrons arrange themselves as far away as possible to minimize electronic repulsion
31
Q

How does a linear structure look like?

A

-bonded atoms:2
-non binding lone electron pairs:0
-bond angle:180°
-molecular geometry: linear
Ex: CO2

32
Q

How does a trigonal planar structure look like?

A 
Bonded Atoms: 3
Non bonding lone electron pairs: 0
Bond Angle: 120°
Molecular Geometry: Trigonal planar
Ex: SO3
33
Q

How does a bent structure look like?

A 
Bonded Atoms: 2
Non bonding lone electron pairs: 1
Bond Angle: < 120°
Molécula Geometry: Bent
Ex: SO2
34
Q

How does a tetrahedral structure look like?

A 
Bonded Atoms: 4
Non bonding lone electron pairs: 0
Bond Angle: 109.5°
Molecular Geometry: tetrahedral
Ex: CH4
35
Q

How does a trigonal pyramidal structure look like?

A 
Bonded Atoms: 3
Non bonding lone electron pairs: 1
Bond Angle: 107°
Molecular Geometry: trigonal pyramidal
Ex: NH3
36
Q

How does a different bent structure look like?

A 
Bonded Atoms: 2
Non bonding lone electron pairs: 2
Bond Angle: 104.5°
Molecular Geometry: bent
Ex: H2O
37
Q

How do you determine molecular shape?

A
  1. Write Lewis structure
  2. Count number of bonded atoms & lone pairs around central atom
  3. If no lone pairs are present, geometry is:
    - 2 bonded atoms: linear
    - 3 bonded atoms: trigonal planar
    - 4 bonded atoms: tetrahedral
  4. If there are lone pairs, look at the arrangement of atoms & name geometry
38
Q

How do you determine polarity?

A
  1. Write Lewis structure
  2. Draw geometry
  3. Use following symbol to denote polarity of each bond
    Positive end of bond= less electronegative atom
    Negative end of bond= more electronegative atom attracts electrons more strongly towards it
39
Q

What are the guidelines for determining polarity?

A
  • molecules that have no lone pair on central atom & all terminal atoms are same are non polar
  • molecules with one lone pair on central atom are polar
  • molecules with more than one pair on central atom usually polar
40
Q

What are intramolecular forces and intermolecular forces?

A

-Intramolecular Forces: attractive forces within molecules
Ex: chemical bonds
-Intermolecular Forces: attractive forces between molecules

41
Q

What is solubility?

A

Max amount of solute that dissolves in given amount of solvent at specific temperature
Polar molecules: most soluble in polar solvents
No polar molecules: most soluble in nonpolar solvents

42
Q

What is hydrogen bonding?

A

Attractive forces, called hydrogen bonds pull ammonia into water distributing ammonia molecules throughout water, forming homogeneous solution

43
Q

What factors influence boiling and melting points?

A
  1. Strength of attractive force holding substance in its current physical state
  2. Molecular mass
    - larger molecules have higher m.p. and b.p. than smaller molecules
  3. Polarity
    - polar molecules have higher m.p. and b.p. than non polar molecules of similar molecular mass due to its strong attractive force

Chemistry 101 (4 decks)

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