Brainscape's Knowledge GenomeTM

Browse over 1 million classes created by top students, professors, publishers, and experts.


See full index

Chem final > Chapter 4 > Flashcards

Chapter 4 Flashcards

You may prefer our related Brainscape-certified flashcards:
Periodic Table flashcards Chemistry 101 flashcards AP® Chemistry flashcards Organic Chemistry 101 flashcards
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

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
2
Q

Molecular formulas give the

A

exact number of
atoms of each element in a compound.

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
3
Q
  • Empirical formulas give the
A

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

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
4
Q

A structural formulas is a

A

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

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
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

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
6
Q

What happens to e- in an ionic bond?

A

e- transferred

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
7
Q

What happens to e- in a covalent bond?

A

e- shared

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
8
Q

What happens to e- in a metallic bond?

A

e- pooled

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
9
Q

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

A

Lattice of cations and anions

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
10
Q

Lattice energy

A

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

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
11
Q

Coulomb’s law

A

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

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
12
Q

What state are ionic compounds in at room temp?

A

Solid

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
13
Q

What teture are ionic compounds?

A

Brittle

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
14
Q

What are ionic compounds melting/boiling temp?

A

High

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
15
Q

What are covalent molecules also known as?

A

Molecular compound

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
16
Q

How is bond length determined?

A

By which molecule has the lowest energy configuration

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
17
Q

What is the melting/boiling point of molecular compounds?

A

Low

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
18
Q

What state is molecular compounds found in at room temp?

A

All 3

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
19
Q

What needs to be overcome to boil covalent substances?

A

Intermolecular attraction

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
20
Q

What is the charge of zinc?

A

+2

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
21
Q

What is the charge of silver?

A

+1

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
22
Q

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

A

+3

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
23
Q

How do you name binary ionic compounds?

A

Metal + Nonmetal-ide

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
24
Q

How do you name multivalent cations?

A

Metal (charge) + Nonmetal-ide

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
25
Q

What are polyatomic ions? What do they have in common?

A

Molecules that contain multiple types of atoms, most are oxyanions

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
26
Q

What are oxyanions?

A

Have O and one other element

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
27
Q

More O atoms

A

per-, -Ate

28
Q

Less O atoms

A

hypo, -Ite

29
Q

How many O atoms do 2nd row -ate ions have?

A

3

30
Q

How many O atoms do 3rd row -ate ions have?

A

4

31
Q

How do you predict charges of 2nd row ions?

A

Relative to Oxygen

32
Q

How do you predict charges of 3rd row ions?

A

Relative to Argon

33
Q

How do you name molecular compounds?

A

Prefix- name of 1st element + Prefix-base name-ide. Put left one first.

34
Q

Do you put mono for 1st element of molecular compounds?

A

No

35
Q

What are the 2 different types of acids? How do you separate them?

A

Binary (2 elements) or Oxy (Contain oxygen)

36
Q

How do you name binary acids?

A

Hydro + Base name of nonmetal + -ic acid

37
Q

How do you name oxyacids if it ends in -ate?

A

Change -ate to -ic and add acid

38
Q

How do you name oxyacids if they end in -ite?

A

Change -ite to -ous and add acid

39
Q

What are organic compounds?

A

Hydrocarbons

40
Q

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?

A

G.N. Lewis, the octet rule

41
Q

What e- are involved in chemical bonding? Where are they?

A

Valence electrons, outer-shell

42
Q

What are inner e- aka?

A

Core e-

43
Q

Electrons shared by atoms are called

A

bonding pairs

44
Q

− Electrons belonging to 1
particular atom are called

A

lone pairs

45
Q

What is a a polar covalent bond?

A

Bond that doesn’t share e- equally

46
Q

Electro-
negativity is
the ability of
atoms in a
molecule

A

to
attract e−s to
themselves.

47
Q

Who discovered the concept of electronegativity?

A

Linus
Pauling

48
Q

What is a dipole?

A

Molecule with positively and negatively charged ends

49
Q

What is the dipole moment?

A

measure of the bond polarity (how big difference in e-negativity is)

50
Q

Nonpolar covalent –∆EN

A

∆EN is 0 to 0.4.

51
Q

Polar covalent –
∆EN

A

is 0.5 to 1.9.

52
Q

Ionic – ∆EN

A

is
2.0 or greater.

53
Q

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.

A
54
Q

What is the formula for formal charge?

A

Total VE-nonbonding e- - (bonding/2)

55
Q

How do you find the best lewis structure?

A

Fewest charges, - charge on most e-negative atom

56
Q

What scientist proposed that the electron in a hydrogen atom can only have certain energies (i.e., the electron is quantized)?

A

Bohr

57
Q

What are resonance structures?

A

Alternate forms of a molecule that differ in e- placement

58
Q

What happens to e- in double and single bonds?

A

They’re delocalized

59
Q

What are the exceptions to the octet rule?

A

Ions with odd # of e (rare and unstable, called radicals)-, less than an octet, or more than 8 VE.

60
Q

What do you prioritize when being forced to choose between filling octet of outer atoms or making double bonds?

A

Filling octet (slide 79)

61
Q

What atoms can have more than 8 e-?

A

Atoms in D orbital

62
Q

When should you expand an octet? (81)

A

When the central atom in on the
3rd row or below and expanding its octet
eliminates some formal charges

63
Q

What are FCs values normally?

A

0

64
Q

How many bonds does Nitrogen make?

A

3

65
Q

How many bonds does Oxygen make?

A

2

66
Q

How many bonds do halogens make?

A

1

Chem final (6 decks)

Brainscape helps you reach your goals faster, through stronger study habits.
© 2024 Bold Learning Solutions. Terms and Conditions