Ch. 8 Ionic Compounds Flashcards

1
Q

Chemical bond

A
  • The force that holds two atoms together
  • an attachment may form by the attraction of the positively charged nucleus of one atom for the negatively charged electrons of another atom or by the attraction of charged atoms which are called ions
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2
Q

Valence electrons

A
  • the electrons in the outermost energy level

- also in the chemical bond attraction

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3
Q

Noble gasses

A

Are a family of elements that have very little tendency to react

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4
Q

Stable Octet

A

Elements have a set of eight outermost electrons

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5
Q

Pseudo- noble gas formations

A

Relatively stable electrons structures developed by loss of electrons in certain elements of groups 1B, 2B, 3A, and 4A

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6
Q

True or false ?

A positively charged ion is called an anion

A

False

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7
Q

True or false ?

Elements in group 1A lose the I one valence electron, forming an ion with a 1+ charge

A

True

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8
Q

True or false ?

Elements tend to react so that they acquire the electron structure of a halogen

A

False

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9
Q

True or false ?

A sodium atom tends to lose one electron When it reacts

A

True

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10
Q

True or false ?

The electron structure of a zinc ion (Zn2+) is an example of a pseudo noble gas formation

A

True

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11
Q

True or false ?

A CI- ion is an example of a cation

A

False

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12
Q

True or false ?

The ending -ide is used to designate an anion

A

True

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13
Q

True or false ?

Non metals form a stable outer electron configuration by losing electrons and becoming anions

A

False

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14
Q

Ionic bond

A

Is a force that holds together atoms that are oppositely charged

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15
Q

The formula unit of an ionic compound shows the

A

Simplest ratio of the ions

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16
Q

The overall charge of a formula unit of an ionic compound

A

Is always zero

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17
Q

Ionic bonds generally occur between

A

A metal and a non metal

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18
Q

salts are ex’s of

A

Ionic compounds

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19
Q

Crystal lattice

A

A three dimensional arrangement of particles In an ionic solid

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20
Q

In a crystal lattice of an ionic compound

A

Ions are surround by ions of the opposite charge

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21
Q

What is the relationship between lattice em where and the strength of the attractive force holding ions in place ?

A

The more negative the lattice energy is the greater the force

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22
Q

The formation of a stable ionic compound from ions

A

Is always exothermic

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23
Q

In electron transfer involving a metallic atom and a nonmetallic atom during ion formation, _________________________________________

A

The nonmetallic atom gains electrons from the metallic atom

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24
Q

Melting point

A

High

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25
Boiling point
High
26
Hardness
Hard
27
Brittleness
Brittle
28
Electrical conductivity in a sold state
Poor
29
Electrical conductivity in the liquid state
Good
30
Electrical conductivity when dissolved in water
Good
31
True or false ? | The crystal lattice of an ionic compound affects their melting and boiling points
True
32
True or false ? | The lattice energy is the energy required to separate the ions of an ionic compound
True
33
True or false ? | The energy of an ionic compound is higher than that of the separate elements that formed it
False
34
True or false ? | Large ions tend to produce more negative value for the lattice energy thanthe smaller ions do
False
35
True or false ? | Ions that have larger charges tend to produce a more negative lattice energy than ions with smaller charges do
True
36
Monatomic ion
A one atom ion
37
Oxidation number
- The number of electrons transfers to or from the atom to form the ion - the charge of such an ion is equal to the atoms^
38
In ionic compounds the sum of the charges of all the ions equals ________
0
39
Polyatomic ions
Ions made up of more than one atom
40
Oxyanion
An ion negatively charged and includes one or more oxygen atoms
41
Suffix - ate
Two such ions can be formed that contain different number of oxygen atoms, the name for the ion with more oxygen atoms
42
Suffix - ite
The name for the ions with fewer oxygen atoms
43
Chemical formula for any ionic compound
The chemical symbol for the CATION is written first followed by the chu kcal symbol for the ANION
44
Subscript
- Is a small number used to represent the number of ions of a given element in a chemical formula - these numbers are written to the lower right of symbol for the element
45
Chlorate
C1O¥3-
46
Hypochlorite
C1O-
47
Chloride
C1-
48
Perchlorate
C1O¥4-
49
Chlorite
C1O¥2-
50
NaI
Sodium Ludide
51
CaC1,2
Calcium chloride
52
K,2S
Potassium sulfide
53
MgO
Magnesium oxide
54
LiHSO
Lithium hydrogen sulfate
55
NH,4Br
Ammonium bromide
56
Ca,3N,2
Calcium nitride
57
Cs,3P
Cesium phosphide
58
KBrO,3
Potassium bromate
59
Mg(CIO),2
Magnesium hypo chloride
60
Li,2O,2
Lithium peroxide
61
Be,3(PO,4),2
Beryllium carbonate
62
(NH,4),2CO,3
Amuonium carbonate
63
NaBrO,3
Sodium bromate
64
Fr,2O,3
Iron (111) oxide
65
Fe(IO,3),2
Iron (111) lodate
66
Beryllium nitride
Be,3N,2
67
Nickel (11) chloride
NiCI,2
68
Potassium chlorite
KcIO,2
69
Copper (1) oxide
Cu,2O
70
Magnesium sulfite
MgSO,3
71
Ammonium sulfide
(NH,4) ,2S
72
Calcium iodate
Ca (IO,3) ,2
73
Iron (111) perchlorate
Iron (CIO,4),3
74
Sodium nitride
Na,3N
75
Why are the electrons in a metallic solid described as delocalized?
They move from one atom to another