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Chem final > Chapter 4 > Flashcards

Chapter 4 Flashcards

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1
Q

What is the difference between a compound and a molecule?

A

A molecule is made of 2+ atoms, but
A compound is made of
2+ elements

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2
Q

Molecular formulas give the

A

exact number of
atoms of each element in a compound.

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3
Q
  • Empirical formulas give the
A

lowest whole-number
ratio of atoms of each element in a compound.

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4
Q

A structural formulas is a

A

sketch or diagram of how
the atoms in the molecule are bonded to each other.

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5
Q

A molecular model is a more __________
A ball-and-stick molecular model
represents atoms as _____ and
chemical bonds as ______
− The balls are typically color-coded
to specific __________.
− How the atoms connect reflects a
____________.
6
© 2018 Pearson Education, Inc. © 2022 Tophatmonocle Corp.

A

accurate
& complete way to specify a compound.

balls, sticks

elements

molecule’s shape

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6
Q

What happens to e- in an ionic bond?

A

e- transferred

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7
Q

What happens to e- in a covalent bond?

A

e- shared

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8
Q

What happens to e- in a metallic bond?

A

e- pooled

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9
Q

What does an ionic bond look like in the solid state?

A

Lattice of cations and anions

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10
Q

Lattice energy

A

The energy
required to
completely
separate a
mole of a solid
ionic compound
into its gaseous
ions.

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11
Q

Coulomb’s law

A

Distance increases, attraction decrases, charge is also higher but correlation, not causation

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12
Q

What state are ionic compounds in at room temp?

A

Solid

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13
Q

What teture are ionic compounds?

A

Brittle

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14
Q

What are ionic compounds melting/boiling temp?

A

High

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15
Q

What are covalent molecules also known as?

A

Molecular compound

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16
Q

How is bond length determined?

A

By which molecule has the lowest energy configuration

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17
Q

What is the melting/boiling point of molecular compounds?

A

Low

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18
Q

What state is molecular compounds found in at room temp?

A

All 3

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19
Q

What needs to be overcome to boil covalent substances?

A

Intermolecular attraction

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20
Q

What is the charge of zinc?

A

+2

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21
Q

What is the charge of silver?

A

+1

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22
Q

What is the charge of Aluminum (Need to know?)

A

+3

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23
Q

How do you name binary ionic compounds?

A

Metal + Nonmetal-ide

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24
Q

How do you name multivalent cations?

A

Metal (charge) + Nonmetal-ide

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25
What are polyatomic ions? What do they have in common?
Molecules that contain multiple types of atoms, most are oxyanions
26
What are oxyanions?
Have O and one other element
27
More O atoms
per-, -Ate
28
Less O atoms
hypo, -Ite
29
How many O atoms do 2nd row -ate ions have?
3
30
How many O atoms do 3rd row -ate ions have?
4
31
How do you predict charges of 2nd row ions?
Relative to Oxygen
32
How do you predict charges of 3rd row ions?
Relative to Argon
33
How do you name molecular compounds?
Prefix- name of 1st element + Prefix-base name-ide. Put left one first.
34
Do you put mono for 1st element of molecular compounds?
No
35
What are the 2 different types of acids? How do you separate them?
Binary (2 elements) or Oxy (Contain oxygen)
36
How do you name binary acids?
Hydro + Base name of nonmetal + -ic acid
37
How do you name oxyacids if it ends in -ate?
Change -ate to -ic and add acid
38
How do you name oxyacids if they end in -ite?
Change -ite to -ous and add acid
39
What are organic compounds?
Hydrocarbons
40
Who discovered that most main group elements gain, lose, or share electrons to achieve 8 valence electrons (2 s & 6 p e− s)? What is this called?
G.N. Lewis, the octet rule
41
What e- are involved in chemical bonding? Where are they?
Valence electrons, outer-shell
42
What are inner e- aka?
Core e-
43
Electrons shared by atoms are called
bonding pairs
44
− Electrons belonging to 1 particular atom are called
lone pairs
45
What is a a polar covalent bond?
Bond that doesn't share e- equally
46
Electro- negativity is the ability of atoms in a molecule
to attract e−s to themselves.
47
Who discovered the concept of electronegativity?
Linus Pauling
48
What is a dipole?
Molecule with positively and negatively charged ends
49
What is the dipole moment?
measure of the bond polarity (how big difference in e-negativity is)
50
Nonpolar covalent –∆EN
∆EN is 0 to 0.4.
51
Polar covalent – ∆EN
is 0.5 to 1.9.
52
Ionic – ∆EN
is 2.0 or greater.
53
Then formal charge of an atom is the charge it would have if all of the bonding electrons were shared equally between the bonded atoms.
54
What is the formula for formal charge?
Total VE-nonbonding e- - (bonding/2)
55
How do you find the best lewis structure?
Fewest charges, - charge on most e-negative atom
56
What scientist proposed that the electron in a hydrogen atom can only have certain energies (i.e., the electron is quantized)?
Bohr
57
What are resonance structures?
Alternate forms of a molecule that differ in e- placement
58
What happens to e- in double and single bonds?
They're delocalized
59
What are the exceptions to the octet rule?
Ions with odd # of e (rare and unstable, called radicals)-, less than an octet, or more than 8 VE.
60
What do you prioritize when being forced to choose between filling octet of outer atoms or making double bonds?
Filling octet (slide 79)
61
What atoms can have more than 8 e-?
Atoms in D orbital
62
When should you expand an octet? (81)
When the central atom in on the 3rd row or below and expanding its octet eliminates some formal charges
63
What are FCs values normally?
0
64
How many bonds does Nitrogen make?
3
65
How many bonds does Oxygen make?
2
66
How many bonds do halogens make?
1

Chem final (6 decks)

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