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AP Chemistry > Chemical Bonding > Flashcards

Chemical Bonding Flashcards

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1
Q

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

A

2

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2
Q

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

A

Ionic compound

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3
Q

Metals are ________

A

Cations

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4
Q

Non-metals are _________

A

Anions

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5
Q

Cations ________ electrons

A

Lose

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6
Q

Anions _________ electrons

A

Gain

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7
Q

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

A

D-block cations

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8
Q

How strong are ionic bonds?

A

Very strong

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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

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10
Q

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

A

Higher

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11
Q

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

A

Energy

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12
Q

The smaller the ion, the ____________ the melting point

A

Higher

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13
Q

The larger the ion, the __________ the bond

A

Weaker

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14
Q

Ionic solids generally have ______ melting points

A

High

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15
Q

Are ionic solids typically very soft or hard?

A

Hard

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16
Q

How well do ionic solids evaporate?

A

Not well

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17
Q

Ionic solids are not malleable or ductile and _________ along planes

A

Cleave

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18
Q

Most ionic solids are _______ in polar solvents

A

Soluble

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19
Q

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

A

Dissolved

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20
Q

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

A

Higher

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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

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22
Q

___________ are not transferred in covalent bonds

A

Electrons

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23
Q

Covalent bonds occurs between two ____________

A

Non-metals

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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

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25
Q

An elements ability to attract electrons in a chemical bond

A

Electronegativity

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26
Q

Electrons spend more time around an atom with a ________ electronegativity

A

High

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27
Q

What type of bond does a compound with an electronegativity difference of less than 0.5 have?

A

Nonpolar covalent bond

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28
Q

What type of bond does a compound with an electronegativity difference of 0.5-1.9 have?

A

Polar covalent bond

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29
Q

What type of bond does a compound with an electronegativity difference of more than 1.9 have?

A

Ionic bond

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30
Q

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

A

Partial negative charge

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31
Q

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

A

Partial positive

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32
Q

_____________ increase as electronegativity differences increase

A

Partial charges

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33
Q

The sum of the partial charges in any molecule or ion is always equal to the ________________ of the species

A

Overall

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34
Q

Two or more non-metals bonded together to form a compound

A

Molecules

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35
Q

Lewis structures are only used for _____________

A

Covalent compounds (molecules)

36
Q

When making Lewis structures, the __________ electronegative atom should go in the center

A

Least

37
Q

Hydrogen is always a __________ atom

A

Terminal

38
Q

Beryllium and boron are examples of ______________ atoms

A

Electron deficient

39
Q

Atoms in periods __________ can bond with other atoms in such a way that they end up with more than 8 electrons in their octets

A

3-7

40
Q

How are expanded octets possible?

A

They have d-orbitals in their outer shells that can accept electrons

41
Q

The more likely Lewis structure will have formal charges that are closer to or equal to ________

A

Zero

42
Q

Negative formal charges should reside on the more __________ elements in the structure

A

Electronegative

43
Q

How do you calculate formal charge?

A

(# of valence electrons assigned to the neutral atom) - (# of atoms assigned to the electron in the atomic structure)

44
Q

The potential energy of valence electrons _____________ as they approach the nucleus of another atom

A

Decreases

45
Q

Energy is _________ during the formation of a bond

A

Released

46
Q

The more energy released during the formation of a bond the ________ the bond will be

A

Stronger

47
Q

The amount of energy that is required to break the bond between two specific atoms in a molecule

A

Bond energy

48
Q

As the atomic radii of bonding atoms increase, the bond length ___________

A

Increases

49
Q

As the number of bonds between two atoms increases, the bond length __________

A

Decreases

50
Q

Why does the number of bonds between atoms correlate with the bond length?

A

As the electron density between the atoms increases, the attractive forces between the protons and valence electrons increases

51
Q

How do you find bond order?

A

of bonds/ # of terminal atoms

52
Q

A higher bond order correlates with a __________ bond length

A

Shorter

53
Q

Higher bond order correlates with a __________ bond energy

A

Higher

54
Q

How many bonds does carbon have?

A

4

55
Q

How many bonds does nitrogen have?

A

3

56
Q

How many bonds does oxygen have?

A

2

57
Q

How many bonds do fluorine, chlorine, bromine, iodine, and hydrogen have?

A

1

58
Q

Elements tend to gain or lose electrons to acquire a full _________

A

Octet

59
Q

What does VSEPR theory stand for?

A

Valence Shell Electron Pair Repulsion Theory

60
Q

Charge clouds repel each other do to _____________________

A

Coulombic repulsion

61
Q

____________ move as far away from each other as possible

A

Terminal atoms

62
Q

Theory that states that bonding occurs when atomic orbitals overlap

A

Valence bond theory

63
Q

What is the problem with valence bond theory?

A

It gets the bond angle wrong

64
Q

What is the solution to valence bond theory?

A

Hybrid orbitals

65
Q

____ bonds have side to side overlap

A

Pi

66
Q

________ bonds have head to head overlap

A

Sigma

67
Q

Single bonds are ______ ponds

A

Sigma

68
Q

How many pi and sigma bonds does a double bond have?

A

1 pi, 1 sigma

69
Q

How many pi and sigma bonds does a triple bond have?

A

2 pi, 1 sigma

70
Q

What type of bonds are able to spin on an axis?

A

Single bonds

71
Q

Why can’t double bonds spin?

A

Pi bonds are rigid and prevents the sigma bonds from spinning, locking the molecule in place

72
Q

What are isomers?

A

Molecules with similar formulas but different shapes

73
Q

Why do pi bonds cause isomers?

A

They creat a lack of flexibility in the molecule

74
Q

Type of isomer where the carbon chain follows the same side

A

Cis

75
Q

Type of isomer where the carbon chain follows opposite sides

A

Trans

76
Q

What type of bond is shorter?

A

Sigma

77
Q

A molecule is polar when the molecule has a _____________ moment

A

Dipole

78
Q

The normal configuration of the electron about the atom or ion of an element

A

Ground state

79
Q

At the ground state, electrons are at their ________ possible energy level

A

Lowest

80
Q

When particles absorb energy (ex. heat) they leave their ground state and become __________

A

Excited

81
Q

Excited state is ______

A

Unstable

82
Q

As electrons return to their ground state, they release the absorbed energy in the form of _____________

A

Electromagnetic energy

83
Q

A red color light possesses ______ energy

A

Low

84
Q

Violet possesses _________ energy

A

High

85
Q

Metallic ions possess electrons that are _________ excited

A

Easily

AP Chemistry (18 decks)

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