Chapter 5 Flashcards

(95 cards)

1
Q

[Binary Ionic Compounds]

_____ compounds are composed of two elements.

A

Binary

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2
Q

[Binary Ionic Compounds]

When one of these elements is a metal and one is a _____, an ionic compound is formed.

A

nonmetal

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3
Q

[Binary Ionic Compounds]

_____ give off electrons and form cations in ionic compounds.

A

Metals

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4
Q

[Binary Ionic Compounds]

_____ gain electrons and form anions in ionic compounds.

A

Nonmetals

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5
Q

[Binary Ionic Compounds]

Ionic compounds are named by stating the cation name and then the _____ name.

A

anion

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6
Q

[Binary Ionic Compounds]

The number of cations or anions is _____ specified. The number of each is understood because the overall charge must equal zero.

A

not

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7
Q

[Binary Ionic Compounds]

The charge of each ion in a binary compound is determined from the _____ _____.

A

periodic table

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8
Q

[Binary Ionic Compounds]

For the main group elements, the

_____ = name of element

A

Cation name

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9
Q

[Binary Ionic Compounds]

For the main group elements, the

_____ _____ = Group number

A

Cation Charge

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10
Q

[Binary Ionic Compounds]

For the main group elements, the

_____ name = element name with the ending replaced by the suffix “ide”

A

Anion

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11
Q

[Binary Ionic Compounds]

For the main group elements, the

Anion Charge = _____ _____ (+/-) _____

A

Group number - 8

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12
Q

[Binary Ionic Compounds]

For the main group elements, the

Compound name = _____ name (+/-) _____ name

A

cation name + anion name

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13
Q

[Binary Ionic Compounds]

For the main group elements, the

compound charge = _____

A

0

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14
Q

[Binary Ionic Compounds:
Multiple Oxidation States]

The cations from group 1A and 2A metals always have charges of (+/-) ___ and (+/-) ___.

A

+1 and +2

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15
Q

[Binary Ionic Compounds:
​Multiple Oxidation States]

In addition to group 1A and 2A, a few other metals display only one oxidation state.

These are:

a. _____
b. _____
c. _____
d. _____

A

a. Ag+ silver
b. Zn2+ zinc
c. Cd2+ cadmium
d. Al3+ aluminum

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16
Q

[Binary Ionic Compounds:
​Multiple Oxidation States]

If you are naming a metal cation that has only one oxidation state, do you use Roman numerals in the name? True/False

A

false

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17
Q

[Covalent Compounds:
Name and Formula]

The _____ bonds are when nonmetals can combine with others nonmetals.

A

Covalent

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18
Q

[Covalent Compounds:
​Name and Formula]

Binary covalent compounds contain two _____.

A

nonmetals

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19
Q

[Covalent Compounds:
​Name and Formula]

Because nonmetals can share electrons in covalent bonds in many different ways, it is necessary to specify the number of each _____ in the compound.

A

element

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20
Q

[Covalent Compounds:
​Name and Formula]

The number 1 prefix is called _____.

A

mono

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21
Q

[Covalent Compounds:
​Name and Formula]

The number 2 prefix is called _____.

A

di

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22
Q

[Covalent Compounds:
​Name and Formula]

The number 3 prefix is called _____.

A

tri

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23
Q

[Covalent Compounds:
​Name and Formula]

The number 4 prefix is called _____.

A

tetra

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24
Q

[Covalent Compounds:
​Name and Formula]

The number 5 prefix is called _____.

A

penta

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25
[Covalent Compounds: ​Name and Formula] The number 6 prefix is called \_\_\_\_\_.
hexa
26
[Covalent Compounds: ​Name and Formula] The number 7 prefix is called \_\_\_\_\_.
hepta
27
[Covalent Compounds: ​Name and Formula] The number 8 prefix is called \_\_\_\_\_.
octa
28
[Covalent Compounds: ​Name and Formula] The number 9 is called \_\_\_\_\_.
nona
29
[Covalent Compounds: ​Name and Formula] The number 10 prefix is called \_\_\_\_\_.
deca
30
[Covalent Compounds: ​Name and Formula] Binary covalent compounds always end in \_\_\_\_\_.
ide
31
[Covalent Compounds: ​Name and Formula] In binary covalent compounds, the exceptions to the 'ide' prefix are when the name is \_\_\_\_\_.
common additionally: emphasizing that it is well known
32
[Polyatomic Ions: Nomenclature of other Polyatomic ions] \_\_\_\_\_ ions contain more than one kind of atom.
polyatomic
33
[Polyatomic Ions: ​Nomenclature of other Polyatomic ions] Ions can be \_\_\_\_\_, composed of a group of atoms
polyatomic
34
[Polyatomic Ions: ​Nomenclature of other Polyatomic ions] The hydrogen ion (H+) can be coupled with ___ or ___ anions to create new ions. Ex: **NH3 + H+ = NH4+**
2 - or 3 -
35
[Polyatomic Ions: ​Nomenclature of other Polyatomic ions] H+ can also be combined with the molecule ammonia to make the _____ ion ammonium. Ex: **O2- + H+ = OH-**
POSITIVE
36
[Polyatomic Ions: ​Nomenclature of other Polyatomic ions] The cyanide ion, **CN-**, _____ fit in any of these categories but is an important ion all the same.
doesn't
37
[Polyatomic Ions: ​Nomenclature of other Polyatomic ions] What is the formula for Ammonium?
**NH4+**
38
[Polyatomic Ions: ​Nomenclature of other Polyatomic ions] What is the formula for Hydroxide?
**OH-**
39
[Polyatomic Ions: ​Nomenclature of other Polyatomic ions] What is the formula for Cyanide?
**CN-**
40
[Polyatomic Ions: ​Nomenclature of other Polyatomic ions] What is the formula for Hydrogen carbonate?
**HCO3-**
41
[Polyatomic Ions: ​Nomenclature of other Polyatomic ions] What is the formula for Hydrogen sulfate?
**HSO4-**
42
[Polyatomic Ions: ​Nomenclature of other Polyatomic ions] What is the formula for Dihydrogen phosphate?
**H2PO4-**
43
[Polyatomic Ions: ​Nomenclature of other Polyatomic ions] What is the formula for Hydrogen phosphate?
**HPO42**
44
[Ionic Compounds: A few more to learn] What is the formula for Cyanide?
**CN -**
45
[Ionic Compounds: ​A few more to learn] What is the formula for Hydroxide?
**OH -**
46
[Ionic Compounds: ​A few more to learn] What is the formula for Hydrogen carbonate or Bicarbonate?
HCO3-
47
[Ionic Compounds: ​A few more to learn] What is the formula for Hydrogen sulfate or Bisulfate
**HSO4-**
48
[Ionic Compounds: ate] Ionic compounds are named by stating the cation name and then the anion name. The number of _____ and anions is not specified in an ionic compound. The number of each is understood because the overall charge must equal zero.
cations
49
[Ionic Compounds: ate] \_\_\_\_\_ anions are composed of an element with one or more oxygens attached to it.
Oxo
50
[Ionic Compounds: ate] You must treat the oxo anion as a \_\_\_\_\_.
group Never break it up into elements.
51
[Ionic Compounds: ate] Oxo anions always have the suffix ___ or \_\_\_.
'ate' or 'ite'.
52
[Ionic Compounds: ate] What is the formula to this Oxoanions group? **Nitrate**
**NO3-**
53
[Ionic Compounds: ate] What is the formula to this Oxoanions group? **Acetate**
**CH3COO-** **\*CH3CO2−**
54
[Ionic Compounds: ate] What is the formula to this Oxoanions group? **Carbonate**
**CO32-**
55
[Ionic Compounds: ate] What is the formula to this Oxoanions group? **Sulfate**
**SO42-**
56
[Ionic Compounds: ate] What is the formula to this Oxoanions group? **Chromate**
CrO42-
57
[Ionic Compounds: ate] What is the formula to this Oxoanions group? **Phosphate**
**PO43-**
58
[Polyatomic Ions: Oxo Anions] \_\_\_\_\_ _____ are negatively charged ions containing oxygen plus another element.
'Oxo' anions
59
[Polyatomic Ions: Oxo Anions] 'Oxo' anions are negatively charged ions containing oxygen plus ____ element.
another
60
[Polyatomic Ions: Oxo Anions] oxoanion have the suffix ___ or \_\_\_.
'ate' or 'ite'.
61
[Polyatomic Ions: Oxo Anions] This ends with ate/ite or hpyo+\_\_\_+ite ? **ClO3-**
Chlorate
62
[Polyatomic Ions: Oxo Anions] This ends with ate/ite or hpyo+\_\_\_+ite ? **ClO2-**
Chlorite
63
[Polyatomic Ions: Oxo Anions] This ends with ate/ite or hpyo+\_\_\_+ite ? **ClO-**
Hypochlorite
64
[Ionic Compounds: Acids and Anions of Chlorine] [Acid Model] What is this molecules name? Formula: **HClO3**
chloric acid
65
[Ionic Compounds: Acids and Anions of Chlorine] [Acid Model] What is this molecules name? Formula: **HNO3**
nitric acid
66
[Ionic Compounds: Acids and Anions of Chlorine] [Acid Model] What is this molecules name? Formula: **H2SO4**
sulfuric acid
67
[Ionic Compounds: Acids and Anions of Chlorine] [Acid Model] What is this molecules name? Formula: **H2CO3**
carbonic acid
68
[Ionic Compounds: Acids and Anions of Chlorine] [Acid Model] What is this molecules name? Formula: **H3PO4**
phosphoric acid
69
[Ionic Compounds: Acids and Anions of Chlorine] [Anion Model] What is this molecules name? Formula: **ClO3-**
chlorate ion
70
[Ionic Compounds: Acids and Anions of Chlorine] [Anion Model] What is this molecules name? Formula: **NO3-**
nitrate ion
71
[Ionic Compounds: Acids and Anions of Chlorine] [Anion Model] What is this molecules name? Formula: **SO42-**
sulfate ion
72
[Ionic Compounds: Acids and Anions of Chlorine] [Anion Model] What is this molecules name? Formula: **CO32-**
carbonate ion
73
[Ionic Compounds: Acids and Anions of Chlorine] [Anion Model] What is this molecules name? Formula: **PO43-**
phosphate ion
74
[Ionic Compounds: Acids and Anions of Chlorine] [Acids Model of Chlorine] What is this molecules name? Formula: **HClO4**
perchloric acid
75
[Ionic Compounds: Acids and Anions of Chlorine] [Acids Model of Chlorine] What is this molecules name? Formula: **HClO3**
chloric acid
76
[Ionic Compounds: Acids and Anions of Chlorine] [Acids Model of Chlorine] What is this molecules name? Formula: **HClO2**
chlorous acid
77
[Ionic Compounds: Acids and Anions of Chlorine] [Acids Model of Chlorine] What is this molecules name? Formula: **HClO**
hypochlorous acid
78
[Ionic Compounds: Acids and Anions of Chlorine] [Acids Model of Chlorine] What is this molecules name? Formula: **HCl**
hydrochloric acid
79
[Ionic Compounds: Acids and Anions of Chlorine] [Anion Model of Chlorine] What is this molecules name? Formula: **ClO4-**
perchlorate ion
80
[Ionic Compounds: Acids and Anions of Chlorine] [Anion Model of Chlorine] What is this molecules name? Formula: **ClO3-**
chlorate ion
81
[Ionic Compounds: Acids and Anions of Chlorine] [Anion Model of Chlorine] What is this molecules name? Formula: ClO2-
chlorite ion
82
[Ionic Compounds: Acids and Anions of Chlorine] [Anion Model of Chlorine] What is this molecules name? Formula: **ClO-**
hypochlorite ion
83
[Ionic Compounds: Acids and Anions of Chlorine] [Anion Model of Chlorine] What is this molecules name? Formula: **Cl-**
chloride ion
84
[Ionic Compounds: ite, per, hypo] The ___ anions are formed from the 'ate' anions by removing one oxygen.
ite
85
[Ionic Compounds: ite, per, hypo] **NO3 -** What type of Oxo Anions is this _____ ?
Chlorate
86
[Ionic Compounds: ite, per, hypo] **NO3-** What type of Oxo Anions is this _____ ?
nitrate
87
[Ionic Compounds: ite, per, hypo] **NO2-** What type of Oxo Anions is this _____ ?
Nitrite
88
[Ionic Compounds: ite, per, hypo] **ClO2-** What type of Oxo Anions is this _____ ?
chlorite
89
[Ionic Compounds: ite, per, hypo] The 'per' and 'hypo' Oxo Anions Some elements are able to combine with oxygen to form a range of oxo anions. When this happens, _____ are used.
prefixes
90
[Ionic Compounds: ite, per, hypo] If there is one ____ oxygen than the 'ate' anion, use the prefixper.
MORE
91
[Ionic Compounds: ite, per, hypo] If there is one ____ oxygen than the 'ite' anion, use the prefix hypo.
FEWER
92
[Ionic Compounds: ite, per, hypo] **ClO3 -** What is the name to this formula?
Chlorate
93
[Oxo Acids: Name and Formula] ate anions formic \_\_\_\_\_.
acids
94
ite anions form _____ acids.
ous
95