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CHEM110 > EXAM 2: 06 Bonding > Flashcards

EXAM 2: 06 Bonding Flashcards

1
Q

What is the octet rule

A

In forming bonds, many main group elements gain, lose or share electrons to achieve a stable electron configuration, characterized by 8 valence electrons

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2
Q

What is ionic bonding

A

Formed by ions of opposite charges
Found between atoms from opposite ends of the periodic table
Metals + nonmetals
Electrons are transferred

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3
Q

Metals characteristics

A

Low ionization energy (can easily lose electrons), forms cations with noble gas configurations

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4
Q

Nonmetal characteristics

A

Negative electron affinities (can easily gain electrons), forms anions

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5
Q

What is metallic bonding

A

There are too few electrons to satisfy the octet rule, so valence electrons are shared among all metal atoms
The nuclei and core electrons are immersed in an electron sea composed of all valence electrons

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6
Q

What is covalent bonding

A

Based on the sharing of electron pairs among directly bonded atoms
Forms when nonmetals share electrons
The number of desired covalent bonds must match the number of unpaired electrons in the Lewis structure

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7
Q

Characteristics of metals

A

Good conductors of heat and electricity
Malleability and ductility

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8
Q

Is the formation of ions of opposite charges from neutral atoms in the gas phase energetically favorable or unfavorable?

A

Energetically unfavorable

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9
Q

What is atomization

A

To reduce or separate into atoms

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10
Q

What is lattice energy

A

The amount of energy (enthalpy) required to convert a mole of ionic solid to its constituent ions in the gas phase
- measure the strength of ionic bonding

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11
Q

What is a lattice

A

A 3d array of cations and anions in crystalline solids

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12
Q

What is the trend for determining lattice energy

A

Increasing size = decreasing lattice energy
Increasing charge = increasing lattice energy

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13
Q

Are there any direct bonds between ions?

A

No, just electrostatic attractions

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14
Q

_____ melting point is associated with _______ lattice energy

A

High, high

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15
Q

What are 2 rules for bonding

A
  1. Only valence electrons are used in bonding
  2. Atoms will gain, lose or share electrons to reach a noble gas configuration (filled shell)
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16
Q

What is NH4+ called

A

Ammonium

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17
Q

What is H3O+ called

A

Hydronium

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18
Q

What is HO- called

A

Hydroxide

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19
Q

What is O2- called

A

Peroxide

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20
Q

What is CH3COO- called

A

Acetate

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21
Q

What is C2O42- called

A

Oxalate

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22
Q

What is CN- called

A

Cyanide

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23
Q

What is SCN- called

A

Thiocyanate

24
Q

What is N3- called

25
Q

What is ClO- called

A

Hypochlorite

26
Q

What is ClO2- called

27
Q

What is ClO3- called

28
Q

What is ClO4- called

A

Perchlorate

29
Q

What is SO32- called

30
Q

What is SO42- called

31
Q

What is NO2- called

32
Q

What is NO3- called

33
Q

What is H2PO4- called

A

Dihydrogen phosphate

34
Q

What is HPO42- called

A

Hydrogen phosphate

35
Q

What is PO43- called

36
Q

What is HCO3- called

A

Hydrogen carbonate

37
Q

What is CO32- called

38
Q

What is MNO4- called

A

Permanganate

39
Q

What is CrO42- called

40
Q

What is Cr2O72- called

A

Dichromate

41
Q

Characteristics of ionic compounds

A

High melting points, hard, brittle

42
Q

Increased repulsion = _______ energy

43
Q

What do Lewis structures illustrate

A

The apportionment of bonding and nonbonding electron pairs to atoms in molecules

44
Q

What are multiple bonds

A

A chemical bond in which two atoms share two or more pairs of electrons

45
Q

What is bond order

A

The number of electron pairs shared

46
Q

What do bond lengths depend on

A

Atomic bonding radii and bonding

47
Q

What is the relationship between bond order and bond length

A

The higher the bond order the shorter the bond

48
Q

What is the strength of a covalent bond defined by

A

The energy needed to break that exact bond while leaving other parts of the molecule intact - bond dissociation energy

49
Q

What is the relationship between strength of bond and bond dissociation energy

A

Stronger the bond, higher the BDE

50
Q

What is there relationship between bond length, bond order, bond strength and intermolecular forces

A

The shorter the bond length, and the higher the bond order, the stronger the bond is holding the atoms together within the molecule, and the weaker the intermolecular forces

51
Q

What is a polyatomic atom

A

An electrically charged group of two or more atoms; a molecule that has lost or gained one or more electrons

52
Q

How are atoms in polyatomic ions held together

A

Covalent bonding

53
Q

What is salt

A

An ionic compound

54
Q

Salt characteristics

A

Brittle at room temp, high melting points

55
Q

What are covalent substances and their characteristics

A

Often found as gases or liquids at room temp and pressure
- in solid state: soft and melt easily
- low melting and boiling points

CHEM110 (9 decks)

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