Brainscape's Knowledge GenomeTM

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


See full index

Chemistry 12 > Structure and Properties Test > Flashcards

Structure and Properties Test Flashcards

You may prefer our related Brainscape-certified flashcards:
Chemistry 101 flashcards AP® Chemistry flashcards Periodic Table flashcards Organic Chemistry 101 flashcards
1
Q

The Principal Quantum Number

A

(n) all orbitals that have the same value of n are said to be in the same shell

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

The values of n can range from…

A

n = 1 to n = infinity

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

What happens as the value of n increases?

A

the energies of the orbitals also increases

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

The Secondary Quantum Number

A

(l) divides the shell into smaller groups of orbitals called subshells, determines the shape of the orbital

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

The number of subshells in a given shell = ?

A

n

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

When n = 1, l = ?

A

s

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

When n = 2, l = ?

A

s or p

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

When n = 3, l = ?

A

s, p, or d

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

When n = 4, l = ?

A

s, p, d, or f

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

Letter designation s = ?

A

l = 0

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

Letter designation p = ?

A

l = 1

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

Letter designation d = ?

A

l = 2

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

Letter designation f = ?

A

l = 3

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

The values of l can range from…

A

l = n-1

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

The values of ml can range from…

A

-l to +l

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

Max # of electrons per orbital =

A

2

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

of orbitals per shell =

A

n(squared)

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

of electrons per shell =

A

2n(squared)

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

Electron spin occurs because?

A

electrons behave as tiny magnets in which the revolving electrical charge of the electron creates its own magnetic field

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

The Spin Quantum Number

A

(ms) the spin can take on either of 2 possible values:
ms = +1/2
ms = –1/2

there can only be 2 electrons in one orbital with each spinning in the opposite direction

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

of orbitals =

A

n + value of letter

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

Value of letter: s =?

A

0

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

Value of letter: p =?

A

1

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

Value of letter: d =?

A

2

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

Value of letter: f =?

A

3

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

What are the 4 types of solids?

A
  1. Ionic
  2. Molecular
  3. Covalent Network
  4. Metallic
How well did you know this?
1
Not at all
2
3
4
5
Perfectly
27
Q

Ionic Metals

A
  • metal bonded to a non-metal
  • CATION: metal atoms that lose their electrons and become positively charged
  • ANION: non-metal atoms that gain electrons and become negatively charged
How well did you know this?
1
Not at all
2
3
4
5
Perfectly
28
Q

Ionic Solids

A
  • metal bonded to a non-metal
  • CATION: metal atoms that lose their electrons and become positively charged
  • ANION: non-metal atoms that gain electrons and become negatively charged
How well did you know this?
1
Not at all
2
3
4
5
Perfectly
29
Q

What type of attraction is involved in an Ionic Solid?

A

Electrostatic Attraction: the oppositely charged ions are attracted to each other (aka ionic bonds)

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
30
Q

What type of structure do Ionic Solids make?

A

Crystal Lattice Structure

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
31
Q

Properties of Ionic Solids

A
  • hard and brittle
  • high melting point bc ionic bonds require lots of energy to break
  • in solid form, poor conductors
  • in liquid form, they conduct electricity because the ions separate and are free to move around
How well did you know this?
1
Not at all
2
3
4
5
Perfectly
32
Q

Molecular Solids

A
  • non-metal bonded to non-metal

- held together by intermolecular forces (hydrogen bonds, dipole-dipole interactions, London dispersion forces)

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
33
Q

Properties of Molecular Solids

A
  • soft and flexible bc intermolecular forces are weaker than both ionic and covalent bonds
  • low melting points
  • don’t conduct electricity bc the electrons are shared within the molecules so there are no ions

(the individual molecules don’t break apart, the intermolecular forces do)

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
34
Q

Covalent Network Solids

A
  • made of a network (chain of atoms) held together by covalent bonds

(there are no intermolecular forces, everything is connected by covalent bonds)

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
35
Q

Properties of Covalent Network Solids

A
  • non-metals
  • extremely hard
  • covalent bonds are very strong, giving the solids a high melting point bc it takes a lot of energy to break the bonds
  • have the highest melting point of all 4 types of solids
  • usually don’t conduct electricity bc there are no available ions
  • insoluble in water
How well did you know this?
1
Not at all
2
3
4
5
Perfectly
36
Q

Metallic Solids

A
  • made of metal atoms held together with metallic bonds
  • metallic bonds occur between free valence electrons moving freely throughout the solid
  • uniform distribution of atoms within a “sea of electrons”
    (nuclei are fixed and electrons can flow around them)
How well did you know this?
1
Not at all
2
3
4
5
Perfectly
37
Q

Properties of Metallic Solids

A
  • melting points vary
  • shiny
  • malleable
  • ductile
  • can conduct electricity due to their free electrons
How well did you know this?
1
Not at all
2
3
4
5
Perfectly
38
Q

Mostly Ionic

A

bonds with a ∆EN between 1.7 - 3.3

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
39
Q

Polar Covalent

A

bonds with a ∆EN between 0.4 - 1.7

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
40
Q

Mostly Covalent

A

bonds with a ∆EN between 0.0 - 0.4

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
41
Q

What happens when metal atoms interact with atoms of the same or different metals? Why?

A

Since metal atoms cannot attract and hold electrons of other atoms, well enough to form filled valence shells, the valence electrons of metals in the solid or liquid state HAVE THE ABILITY TO MOVE FREELY FROM ONE ATOM TO THE NEXT

The electrons are said to be delocalized, because they do not remain in one location

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
42
Q

What factors affect the way in which ions pack as they form crystals?

A

relative size and charge of the ions

–––> the point is so that oppositely charged ions are as close together as possible

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
43
Q

Forces involved in a covalent bond

A

Electrostatic Forces

Repulsive Forces

44
Q

Electrostatic Forces

A

The nuclei of both atoms exert attractive forces on both of the shared electrons

45
Q

Repulsive Forces

A

exist between 2 positive nuclei and 2 negative electrons

The bond between 2 atoms occurs at a distance where the REPULSIVE FORCES BALANCE THE ATTRACTIVE FORCES

46
Q

The Pauli Exclusion Principle

A

No 2 electrons in an atom have the same 4 quantum numbers

  • relates back to the spin quantum
  • we show this in an energy level diagram with the 2 opposing arrows in a circle (each circle represents an orbital)
47
Q

The Aufbau Principle

A

Electrons are placed into orbitals by filling the lowest energy orbitals first

  • means you must fill energy sublevels before moving on to the higher sublevel
48
Q

Hund’s Rule

A

if there are several orbitals at the same energy level (e.g. for p, d, or f orbitals), place an electron in each orbital before pairing any up

49
Q

Drawing Energy Level Diagrams for Anions

A
  1. add the amount of the negative charge ( = the amount of extra electrons) to the atomic number of the element
  2. then place the electrons in the orbitals using the proper filing order
50
Q

Drawing Energy Level Diagrams for Cations

A
  1. draw the energy level diagram for the NEUTRAL atom first
  2. remove the number of electrons corresponding with the HIGHEST principle quantum number, n
    * these may not always be the highest energy electrons at the top of the diagram*
51
Q

When you are drawing a Lewis Structure for a polyatomic ion with a negative charge, do you add or take away 1 electron?

A

ADD another electron

52
Q

When you are drawing a Lewis Structure for a polyatomic ion with a positive charge, do you add or take away 1 electron?

A

TAKE AWAY 1 electron

53
Q

Coordinate Covalent Bonds

A

bonds created when 1 atom contributes BOTH ELECTRONS to a bond

54
Q

Expanded Octets

A

an exception to the octet rule where an atom shares more than 8 electrons with its bonding partners

55
Q

Incomplete Octet

A

an exception to the octet rule where the central atom had less than 8 electrons in its valence shell

56
Q

What are the 2 elements that have incomplete octets?

A

Boron and Beryllium

57
Q

Resonance Structures

A

Different Lewis Structures that represent the same molecular compound

58
Q

How do VSEPR structures work?

A

atoms are able to spread around the central atom due to repulsion forces

59
Q

VSEPR

A

Valence Shell Electron Pair Repulsion

60
Q

electrons in a molecule repel each other and will try and get as far away from each other as possible

A

this explains molecular geometry and structure

61
Q

Lone pairs repel more than what kind of bond?

A

they repel more than a sigma bond, which affects bond angles slightly

62
Q

Bonding Pairs

A

set of 2 electrons involved in a bond

–––> this applies to single, double, and triple bonds

63
Q

Nonbonding Pairs/Lone Pairs

A

set of 2 electrons that are not bonded with another atom

64
Q

Single Electrons

A

a single, nonbonding electron

rarely seen

65
Q

A

A

central atom

66
Q

X

A

ligands/surrounding atoms

67
Q

E

A

nonbonding electron pairs

68
Q

e

A

lone nonbonding electrons

69
Q

When drawing VSEPR Structures

A

only include lone pairs on the central atom

70
Q

Valence Bond Theory

A

states that a covalent bond is formed when 2 orbitals overlap to produce a new combined orbital (HYBRID) containing 2 electrons of opposite spins

71
Q

What type of hybrid orbitals are equivalent in shape and energy?

A

hybrid orbitals created in molecules

72
Q

sp Hybrids

Initial atomic orbitals:

Shape:

Degree:

A

Initial atomic orbitals: s, p

Shape: Linear

Degree: 180˚

73
Q

sp Hybrids

Initial atomic orbitals:

Shape:

Degree:

A

Initial atomic orbitals: s, p

Shape: Linear

Degree: 180˚

74
Q

sp^2 Hybrids

Initial atomic orbitals:

Shape:

Degree:

A

Initial atomic orbitals: s, p, p

Shape: Trigonal Planar

Degree: 120˚

75
Q

sp^2 Hybrids

Initial atomic orbitals:

Shape:

Degree:

A

Initial atomic orbitals: s, p, p

Shape: Trigonal Planar

Degree: 120˚

76
Q

sp^3 Hybrids

Initial atomic orbitals:

Shape:

Degree:

A

Initial atomic orbitals: s, p, p, p

Shape: Tetrahedral

Degree: 109.5˚

77
Q

sp^3d Hybrids

Initial atomic orbitals:

Shape:

Degree:

A

Initial atomic orbitals: s, p, p, p, d

Shape: Trigonal Bipyramidal

Degree: 90˚, 120˚

78
Q

sp^3d^2 Hybrids

Initial atomic orbitals:

Shape:

Degree:

A

Initial atomic orbitals: s, p, p, p, d, d

Shape: Octahedral

Degree: 90˚

79
Q

Sigma Bond σ

A

a bond created by the end to end overlap of atomic orbitals

  • it is a SINGLE bond
80
Q

Pi Bond π

A

a bond created by the side-by-side overlap of atomic orbitals, usually p orbitals

  • second and third lines in a DOUBLE or TRIPLE bond
81
Q

Polar Covalent Bond

A

a bond where electrons are not shared equally

82
Q

Electronegativity Difference: Ionic

A

1.7 –––> 3.3

83
Q

Electronegativity Difference: Polar Covalent

A

0.4 –––> 1.7

84
Q

Electronegativity Difference: Covalent

A

0–––>0.4

85
Q

Electronegativity Difference: Ionic

A

1.7 –––> 3.3

VERY POLAR

86
Q

Electronegativity Difference: Polar Covalent

A

0.4 –––> 1.7

SOMEWHAT POLAR

87
Q

Electronegativity Difference: Covalent

A

0–––>0.4

NONPOLAR

88
Q

When drawing dipoles, the vector points towards the more electronegative atom

A

from the positive to the negative end

89
Q

The more electronegative atom

A

g–

90
Q

The less electronegative atom

A

g+

91
Q

Polar Molecules

A

have an unequal distribution of electrons.

92
Q

When are bonds polar?

A

they are polar if the 2 atoms have DIFFERENT electronegativities

93
Q

When are molecules polar?

A

when oppositive sides have opposite charges

94
Q

Bond Dipole

A

the difference in electronegativity between atoms

95
Q

If the dipoles/vectors point in opposite directions (pointing in together or pointing out together), they are…

A

nonpolar because they cancel each other out

96
Q

If the dipoles/vectors point in the same direction, they are…

A

polar

97
Q

Highly symmetrical molecules are usually

A

NONPOLAR

98
Q

Are intermolecular forces greater or weaker than intramolecular forces?

A

much weaker

99
Q

Dipole-Dipole Attractions

A

depend on the strength of the molecular dipole. Molecular dipoles will be attracted to surrounding dipoles

LIKE DISSOLVES LIKE

100
Q

London Forces/Dispersion Forces

A

are due to the attraction of electrons in one molecule to the nuclei of another

strength depends on the number of electrons

101
Q

Hydrogen Bonds

A

are particularly strong and occurs when hydrogen is bonded to a highly electronegative element and the slight positive charge on the hydrogen is concentrated on a small atom so the dipole effect is greater

N, O, F all have lone pairs that attract the slight positive charge on the H

102
Q

Why can dipoles/vectors cancel out?

A

Because they are equal in magnitude and opposite in direction, meaning they are NONPOLAR

103
Q

What atom becomes the central atom (is put in the middle) of a Lewis structure?

A

the least electronegative atom

104
Q

Steps to Determine Polarity:

A
  1. draw lewis structure for the molecule
  2. use the number of electron pairs and VSEPR rules to determine the shape around each atom
  3. use electronegativities to determine the polarity of each bond
  4. add the bond dipole vectors to determine if the final result is zero (nonpolar molecule) or nonzero (polar molecule)
105
Q

of orbitals = n + value of letter

A 
s = 0
p = 1
d = 2
f = 3

Chemistry 12 (4 decks)

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