Brainscape's Knowledge GenomeTM


Top Flashcards (Certified)
All Flashcards

AP Chemistry > Chemical Bonding > Flashcards

Chemical Bonding Flashcards

(85 cards)

Start Studying
1
Q

In n=1, a full octet consists of how many electrons?

A

2

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

Created when a metallic cation forms an electrostatic bond with a non-metal anion

A

Ionic compound

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

Metals are ________

A

Cations

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

Non-metals are _________

A

Anions

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

Cations ________ electrons

A

Lose

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

Anions _________ electrons

A

Gain

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

These elements lose electrons from their highest s-sublevel first before losing from their d-sublevel

A

D-block cations

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

How strong are ionic bonds?

A

Very strong

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

Since it ionic bonds are very strong, a lot of energy had to be put in to break them apart. This makes them very ___________

A

Endothermic

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

In ionic solids, a higher energy correlates with a _________ melting point

A

Higher

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

The energy required to keep a bond together is ________ to the energy required to break a bond apart

A

Energy

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

The smaller the ion, the ____________ the melting point

A

Higher

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

The larger the ion, the __________ the bond

A

Weaker

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

Ionic solids generally have ______ melting points

A

High

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

Are ionic solids typically very soft or hard?

A

Hard

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

How well do ionic solids evaporate?

A

Not well

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

Ionic solids are not malleable or ductile and _________ along planes

A

Cleave

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

Most ionic solids are _______ in polar solvents

A

Soluble

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

Ionic solids conduct electricity only when molten or ____________ in a polar solvent

A

Dissolved

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

The higher the concentration of ions in a solution, the ________ the electrical conductivity

A

Higher

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

A bond in which one atom shares one or more pairs of electrons with another atom so that they both acquire full octets

A

Covalent bonds

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

___________ are not transferred in covalent bonds

A

Electrons

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

Covalent bonds occurs between two ____________

A

Non-metals

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

As two atoms get closer to each other, the attraction between the __________ of one atom and the ________________ of the other atom increases

A

Nucleus, valence electrons

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
25
An elements ability to attract electrons in a chemical bond
Electronegativity
26
Electrons spend more time around an atom with a ________ electronegativity
High
27
What type of bond does a compound with an electronegativity difference of less than 0.5 have?
Nonpolar covalent bond
28
What type of bond does a compound with an electronegativity difference of 0.5-1.9 have?
Polar covalent bond
29
What type of bond does a compound with an electronegativity difference of more than 1.9 have?
Ionic bond
30
In polar covalent bonds, the atom with the higher higher electronegativity develops a ________________ as the valence electrons from both atoms spend more time around it
Partial negative charge
31
In polar covalent bonds the atom with the lower electronegativity develops a ___________________ which is equal in magnitude to the partial negative charge of the more electronegative atom
Partial positive
32
_____________ increase as electronegativity differences increase
Partial charges
33
The sum of the partial charges in any molecule or ion is always equal to the ________________ of the species
Overall
34
Two or more non-metals bonded together to form a compound
Molecules
35
Lewis structures are only used for _____________
Covalent compounds (molecules)
36
When making Lewis structures, the __________ electronegative atom should go in the center
Least
37
Hydrogen is always a __________ atom
Terminal
38
Beryllium and boron are examples of ______________ atoms
Electron deficient
39
Atoms in periods __________ can bond with other atoms in such a way that they end up with more than 8 electrons in their octets
3-7
40
How are expanded octets possible?
They have d-orbitals in their outer shells that can accept electrons
41
The more likely Lewis structure will have formal charges that are closer to or equal to ________
Zero
42
Negative formal charges should reside on the more __________ elements in the structure
Electronegative
43
How do you calculate formal charge?
(# of valence electrons assigned to the neutral atom) - (# of atoms assigned to the electron in the atomic structure)
44
The potential energy of valence electrons _____________ as they approach the nucleus of another atom
Decreases
45
Energy is _________ during the formation of a bond
Released
46
The more energy released during the formation of a bond the ________ the bond will be
Stronger
47
The amount of energy that is required to break the bond between two specific atoms in a molecule
Bond energy
48
As the atomic radii of bonding atoms increase, the bond length ___________
Increases
49
As the number of bonds between two atoms increases, the bond length __________
Decreases
50
Why does the number of bonds between atoms correlate with the bond length?
As the electron density between the atoms increases, the attractive forces between the protons and valence electrons increases
51
How do you find bond order?
of bonds/ # of terminal atoms
52
A higher bond order correlates with a __________ bond length
Shorter
53
Higher bond order correlates with a __________ bond energy
Higher
54
How many bonds does carbon have?
4
55
How many bonds does nitrogen have?
3
56
How many bonds does oxygen have?
2
57
How many bonds do fluorine, chlorine, bromine, iodine, and hydrogen have?
1
58
Elements tend to gain or lose electrons to acquire a full _________
Octet
59
What does VSEPR theory stand for?
Valence Shell Electron Pair Repulsion Theory
60
Charge clouds repel each other do to _____________________
Coulombic repulsion
61
____________ move as far away from each other as possible
Terminal atoms
62
Theory that states that bonding occurs when atomic orbitals overlap
Valence bond theory
63
What is the problem with valence bond theory?
It gets the bond angle wrong
64
What is the solution to valence bond theory?
Hybrid orbitals
65
____ bonds have side to side overlap
Pi
66
________ bonds have head to head overlap
Sigma
67
Single bonds are ______ ponds
Sigma
68
How many pi and sigma bonds does a double bond have?
1 pi, 1 sigma
69
How many pi and sigma bonds does a triple bond have?
2 pi, 1 sigma
70
What type of bonds are able to spin on an axis?
Single bonds
71
Why can't double bonds spin?
Pi bonds are rigid and prevents the sigma bonds from spinning, locking the molecule in place
72
What are isomers?
Molecules with similar formulas but different shapes
73
Why do pi bonds cause isomers?
They creat a lack of flexibility in the molecule
74
Type of isomer where the carbon chain follows the same side
Cis
75
Type of isomer where the carbon chain follows opposite sides
Trans
76
What type of bond is shorter?
Sigma
77
A molecule is polar when the molecule has a _____________ moment
Dipole
78
The normal configuration of the electron about the atom or ion of an element
Ground state
79
At the ground state, electrons are at their ________ possible energy level
Lowest
80
When particles absorb energy (ex. heat) they leave their ground state and become __________
Excited
81
Excited state is ______
Unstable
82
As electrons return to their ground state, they release the absorbed energy in the form of _____________
Electromagnetic energy
83
A red color light possesses ______ energy
Low
84
Violet possesses _________ energy
High
85
Metallic ions possess electrons that are _________ excited
Easily

AP Chemistry (18 decks)

Brainscape helps you reach your goals faster, through stronger study habits.
© 2025 Bold Learning Solutions. Terms and Conditions