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Chemistry (My Deck) > Chapter 6 and p. Chapter 7 > Flashcards

Chapter 6 and p. Chapter 7 Flashcards

1
Q

What is an ionic bond?

A

A transfer of electrons from a metal to a nonmetal.

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2
Q

Why do ionic bonds transfer electrons?

A

To form a stable compound

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3
Q

What is a covalent bond?

A

The sharing of electrons between two or more nonmetals.

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4
Q

Why do covalent bonds share electrons?

A

To form a stable compound

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5
Q

What is a metallic bond?

A

A bond between metals forming a sea of electrons.

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6
Q

What is notable about metallic bonds?

A

The electrons are free

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7
Q

What must all covalent bonds satisfy?

A

the Octet Rule

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8
Q

What is the octet rule?

A

All elements/polyatomic ions are stable with eight valence electrons.

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9
Q

A ______ has a positive charge.

A

A cation has a positive charge.

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10
Q

A(n) _____ has a negative charge.

A

A anion has a negative charge.

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11
Q

Compounds made of two elements are what?

A

binary compounds

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12
Q

How are polyatomic ions bonded?

A

Covalently.

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13
Q

A polyatomic ion has an _______ charge.

A

A polyatomic ion has an overall charge.

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14
Q

List the order of the prefix/suffix from least to greatest oxygen.

A

per–ate
ate
ite
hypo–ite

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15
Q

Where are metals with multiple charges located on the periodic table?

A

Metals with multiple charges are located in the d, f, and p sections of the periodic table.

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16
Q

What is Zinc’s charge?

A

+2

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17
Q

What is Silver (Ag)’s charge?

A

+1

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18
Q

What are the prefixes for for 1-9 for covalent bonds?

A 
1 - Mono
2 - Di
3 - Tri
4 - Tetra
5 - Penta
6 - Hexa
7 - Hepta
8 - Octa
9 - Nona
10 - Deca
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19
Q

Covalent bonds are between what?

A

Two nonmetals

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20
Q

What are diatomic molecules?

A

Diatomic molecules are molecules of 2 of the same type of atom.

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21
Q

What are elements that can be diatomic?

A

H, N, O, and column 7

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22
Q

What are the three types of covalent bonds and how many electrons do they share?

A

single (2 e-)
double (4 e-)
triple (6 e-)

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23
Q

As the covalent bonds increase (single to triple) what happens?

A

The bonds become stronger and shorter.

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24
Q

What does a lewis structure represent?

A

A lewis structure represents valence electrons in the bonds present of the covalent bond.

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25
Q

True or False: A covalent bond must satisfy the octet rule.

A

True

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26
Q

What is resonance?

A

Resonance means that there is more than one possible bond structure.

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27
Q

How can there be resonance?

A

There can be resonance if a double or triple bond can be moved to another place, without interfering with the structure.

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28
Q

What are the valence electrons (on a lewis structure) called that are not bonded to another element/polyatomic ion?

A

Lone pairs

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29
Q

How many electrons does hydrogen need to be stable?

A

2 e-

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30
Q

Name three properties of an acid?

A

sour
turns litmus red
reacts with some metals to produce hydrogen gas

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31
Q

If the acid is an anion ending in “ide,” how is it named?

A

hydro____ic acid

i.e. hydrofluoric acid (H2S)

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32
Q

If the acid is a polyatomic ion ending in
“ate,”
how is it named?

A

______ic acid

i.e. nitric acid (HNO3)

33
Q

If the acid is a polyatomic ion ending in
“ite,”
how is it named?

A

_______ous acid

i.e. chlorous acid (HCLO2)

34
Q

If the acid is a polyatomic ion like
“per–ate,”
how is it named?

A

per–ic acid

35
Q

If the acid is a polyatomic ion like
“hypo–ite,”
how is it named?

A

hypo–ous acid

36
Q

An acid can also be labeled what?

A

aqueous (aq.)

37
Q

Why are acids aqueous?

A

The acid is aqueous since it can be dissolved in a solution of water.

38
Q

When is an ion with an H not an acid?

A

when a state of matter is given (gas, solid, liquid)

39
Q

What are hydrates?

A

Hydrates are compounds containing water.

40
Q

What does anhydrous mean?

A

Anhydrous is a compound with out water.

41
Q

What is the water removed from heating a hydrate called?

A

Water of hydration

42
Q

Substances that pull water from the air are what?

A

Hygroscopic

43
Q

Substances that release water from the air are what?

A

Efflorescent

44
Q

A substance that absorbs enough water in the air to form a solution is what?

A

deliquescent

45
Q

Do you use roman numerals in hydrates?

A

Yes.

46
Q

When do you use roman numerals in naming?

A

Use roman numerals after the first element in an ionic compound if

  • the element is not in group 1 or 2
  • the element is not aluminum
47
Q

What is the structure of a hydrate?

A

_ _ • _ H20

48
Q

What is electronegativity?

A

Electronegativity is the ability to attract electrons.

49
Q

Why does electronegativity (EN) increase?

A

Due to increasing nuclear charge

50
Q

What is a nonpolar covalent bond?

A

A bond that shares electrons evenly between atoms.

51
Q

The electronegativity range for nonpolar covalent bonds is what?
What is the charge?

A

0 up to 0.3

No charge

52
Q

What is a polar covalent bond?

A

A bond that shares electrons, but the electrons shift toward the higher EN element.

53
Q

The electronegativity range for polar covalent bonds is what?

A

0.3 to 1.7

54
Q

The transfer of electrons to create a cation (+) and anion (-) is what?

A

Tonic

55
Q

What is Van der Waals forces?

A

The forces of attraction between particles.

56
Q

What are the four types of forces based on electronegativity?

A

London Dispersion Forces
Dipole-Dipole
H-bond
Ion-Ion

57
Q

In the same order, what increases down the list?

A

melting point, strength, and brittleness

58
Q

When electrons from one atom are attracted to the close positive force from another, it is called ______ __________ ______.

A

When electrons from one atom are attracted to the close positive force from another, it is called London Dispersion Forces (LDF) .

59
Q

Are Dipole-Dipole forces only polar or nonpolar?

A

Dipole-Dipole are only polar.

60
Q

What are Dipole-Dipole forces?

A

An end of one molecule is attracted to the positive end of the adjacent molecule.

61
Q

An H-bond is when molecules contain Hydrogen bonds to _, _, or _.

A

An H-bond is when molecules contain Hydrogen bonds to N, O, or F.

62
Q

H-bonds are stronger than dipole-dipole. This means that they are harder to what?

A

Melt or boil

63
Q

An Ion-Ion force is what?

A

A cation/anion attraction

64
Q

If the EN-EN=0, then what force is at work?

A

London Dispersion Forces (LDF)

65
Q

A ______ ____ is made with hydrogen and one other element.

A

A binary acid is made with hydrogen and one other element.

66
Q

An anion containing oxygen is what?

A

Oxyanion

67
Q

An acid containing oxygen is what?

A

Oxyacid

68
Q

Nomenclature is a what?

A

naming system

69
Q

The oxidation state is the ______.

A

The oxidation state is the charge.

70
Q

What is the smallest particle of an Ionic substance called?

A

formula unit

71
Q

What is the smallest particle of a covalent substance called?

A

molecule

72
Q

What type of force is related to Ionic substances?

A

Van der Waals and Ion-Ion

73
Q

What type of force is related to nonpolar Covalent substances?

A

London Dispersion Forces

74
Q

What type of force is related to polar Covalent substances?

A

dipole-dipoe

75
Q

When do Ionic compounds conduct electricity?

A

at a solid or molten state

76
Q

Do covalent compounds conduct electricity?

A

No, covalent compounds do not conduct electricity.

77
Q

Which has a strong odor because it vaporizes quickly: covalent vs ionic?

A

Covalent

78
Q

________ compounds have a low melting/boiling point.

A

Covalent compounds have a low melting/boiling point.

Chemistry (My Deck) (8 decks)

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