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Chemistry > Unit Four > Flashcards

Unit Four Flashcards

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1
Q

Polyatomic ion

A

An ion made up of two or more atoms

PO4-3

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2
Q

Cation

A 
A positive ion
Forms from the loss of electrons
Metals
Mg2+
Li+
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3
Q

Anion

A 
A negative ion
Forms from the gain of electrons
Nonmetals
N3-
S2-
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4
Q

Naming cations

A

Keep the name of their parent ion, add ion to the end

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5
Q

Name an ion of Mg

A

Magnesium ion

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6
Q

Naming anions

A

Keep the root of their name but change the ending to ide

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7
Q

Name a nitrogen ion

A

Nitride ion

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8
Q

Chemical bond

A

An attractive force between atoms or ions that binds them together as a unit

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9
Q

Why do bonds form?

A

Decrease potential energy

Increase stability

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10
Q

Compound

A

A pure substance made of two or more elements that are chemically combined

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11
Q

Monotmic ion

A

An ion made up of one atom

Na+

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12
Q

Molecule

A

A special term used to describe compounds that are made by the sharing of electrons (covalent bond)

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13
Q

Binary compound

A

A compound containing two different elements

CaF2

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14
Q

Ionic bonds

A

A bond formed from the transfer of electrons (one atom loses electrons and the other one gains them)
Often referred to as salts

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15
Q

What types of atoms can form ionic bonds?

A

Metal and a nonmetal
Metal and a polyatomic ion
Polyatomic ion and a nonmetal
Two polyatomic ions

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16
Q

Structure of an ionic bond

A

Crystal lattice

Result of positive and negative ions stacking themselves up so they will be near an ion of opposite charge

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17
Q

Strength of ionic bonds

A

Very strong because the opposite charges inside attract each other, making it hard to pull them apart

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18
Q

Melting and boiling point of ionic bond

A

High melting and boiling point because their bonds are very strong so they require a lot of energy to break

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19
Q

Conductivity of ionic bonds

A

Can conduct electricity when they are dissolved in water or molten, don’t conduct electricity when solid because the ions are locked in place and can’t allow the electrons to flow

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20
Q

Are ionic compounds soft?

A

No they are hard but very brittle—energy required to break is large, it will shatter whole structure instead of breaking just one

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21
Q

Covalent bond

A

Forms when two atoms share electrons so they can both satisfy the octet rule. Because they are sharing electrons, there is no cation or anion in a covalent molecule (no charges).

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22
Q

What types of atoms can form covalent bonds?

A

Formed between nonmetals only

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23
Q

Structure of covalent bonds

A

Structure can vary

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24
Q

Strength of covalent bonds

A

Weak—there are positive and negative ions being attracted to each other

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25
Q

Melting and boiling point of covalent bonds

A

Low melting and boiling point—weak type of bond so less energy to break them

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26
Q

Conductivity of covalent bonds

A

Don’t conduct electricity—don’t break into ions so electrons can’t flow through

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27
Q

Acids

A

First element is Hydrogen (H) can be bonded to a nonmetal or polyatomic ion
Technically an ionic bond where H gives away its one valence electron
Only exception is water

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28
Q

Polar covalent bond

A

Atoms are not equally sharing electrons (this is because one of the atoms is stronger)

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29
Q

Nonpolar covalent bond

A

Atoms are equally sharing electrons

Get partial charges

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30
Q

Polarity is determined by…

A

The electronegativity of the atoms bonded together

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31
Q

Electronegativty

A

The ability for an atom to pull shared electrons towards itself (strength)0

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32
Q

Difference of electronegativities is:
0.5?
_>0.5
_>1.7?

A

Nonpolar
Polar
Ionic

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33
Q

Bond length from lowest to highest

A

Ionic

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34
Q

Bond strength from lowest to highest

A

Nonpolar covalent

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35
Q

Ternary compound

A

A compound containing three or more different elements

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36
Q

Two rules for writing formulas

A

Cation has to come before the anion (positive comes before negative)
The charges of the ions have to cancel out, use criss cross rule

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37
Q

Acetate

A

(CH3COO)-1

(C2H3O2)-1

38
Q

Ammonium

A

(NH4)+1

39
Q

Carbonate

A

(CO3)-2

40
Q

Cyanide

A

(CN)-1

41
Q

Hydroxide

A

(OH)-1

42
Q

Phosphate

A

(PO4)-3

43
Q

Phosphite

A

(PO3)-3

44
Q

Nitrate

A

(NO3)-1

45
Q

Nitrite

A

(NO2)-1

46
Q

Sulfate

A

(SO4)-2

47
Q

Sulfite

A

(SO3)-2

48
Q

For ionic compounds, what do you do?

A

Leave the first ion normal and change the ending of the second one to ide

49
Q

Naming formulas with polyatomic ions

A

Normal—put the positive one in front and negative in back, keep names of both, except if normal ion is in back, then change its ending to ide

50
Q

What is always the charge on silver?

A

Ag+

51
Q

What is always the charge on zinc?

A

Zn+2

52
Q

What is always the charge on cadmium?

A

Cd+2

53
Q

What is always the charge on aluminum?

A

Al+3

54
Q

What is always the charge on gallium?

A

Ga+3

55
Q

What is the number in Roman numerals in naming transition metals?

A

The charge of an atom

56
Q

Naming covalent molecules

A

Add a prefix if they have a prefix
If there is only one of the second element, add mono (but not if there is only one of the first element)
The second element ends in ide
Oxygen drops some of the prefix endings

57
Q

Prefix for 1

A

Mono

58
Q

2

A

Di

59
Q

3

A

Tri

60
Q

4

A

Tetra

61
Q

5

A

Penta

62
Q

6

A

Hexa

63
Q

7

A

Hepta

64
Q

8

A

Octa

65
Q

9

A

Nona

66
Q

10

A

Deca

67
Q

Naming acids that don’t have oxygen

A

Add prefix hydro and suffix ic to the anion

Add acid after that

68
Q

Naming acids with oxygen

A

If it ends in ate, change to ic
If it ends in ite, change it to ous
Add acid

69
Q

Exceptions for acids

A 
Phosphorus without oxygen:
Phosphoric
Sulfur without oxygen:
Sulfuric
Phosphate:
Phosphoric
Phosphite:
Phosphorous 
Sulfate:
Sulfuric
Sulfite:
Sulfurous
70
Q

Lewis dot structures

A

Show the number of valence electrons for a given atom

71
Q

Octet rule

A

Atoms will gain, lose, or share atoms in order to have a full valence shell

72
Q

How to draw a Lewis dot structure for an atom

A

Each atom is represented by its symbol
No more than two electrons may go on each side of the atom
Only valence electrons appear in Lewis dot structures

73
Q

How to draw a Lewis dot structure for a compound

A

Each bond represents two electrons being shared between two atoms

  1. Count the total number of valence electrons for all atoms in the compound
  2. Draw a single bond from the central atom to each of the attached atoms. The central atom is typically the atom written first in a chemical formula
  3. Complete each outer atoms octet first
  4. Put any extra electrons on the central atom
  5. If your central atom did not obtain a stable octet with the previous step, you must create multiple bonds to satisfy the octet rule for all atoms
74
Q

Single bond is…
Double bond is…
Triple bond is…

A

2 electrons
4 electrons
6 electrons

75
Q

Bond length

Bond strength

A

Length decreases with an increased number of bonds

Strength increases as you increase the number of bonds

76
Q

Multiple bonds are common between

A

Carbon, nitrogen, oxygen, and sulfur

77
Q

How many electrons does hydrogen need to have a full valence shell?

A

2

78
Q

How many electrons does boron need to be stable?

A

Only 6

79
Q

The central atom forms…

A

The most bonds—it is usually the element that you only have one of, but not always

80
Q

Draw some Lewis dot structures for practice

A

Hopefully you got them right

81
Q

Polyatomic ion

A

Multiple ions bonded together

82
Q

What do you do if the compound has a charge?

A

Add or subtract electrons to the total depending on the charge

83
Q

Polyatomic ion Lewis dot structures

A

Same thing but put the charge into the total number of electrons and put it in brackets and put the charge outside the brackets

84
Q

What does VSEPR stand for?

A

Valence shell electron pair repulsion (theory)

85
Q

VSEPR theory

A

The negative charges on electrons causes them to repel each other. As a result, the atoms in a molecule try to spread out as far as possible.
Shapes are determined by the repulsion forces between shared and unshared electron pairs.
Before determining a shape, you must draw the Lewis dot structure.

86
Q

MXE formulas

A 
M = middle or central atom
X = attached atoms
E = lone electron PAIRS on the central atom
87
Q

MX2 whole thing

A 
Example = CO2
Draw Lewis dot structure
Molecular geometry (shape) =linear
Polarity = nonpolar (as long as all attached atoms are the same element)
Bond angle = 180°
88
Q

MX3 whole thing

A 
Example = BH3
Draw Lewis dot structure
Molecular geometry (shape) = trigonal planar
Polarity = nonpolar (as long as all attached atoms are the same)
Bond angle = 120°
89
Q

MX4 whole thing

A 
Example = CH4
Draw Lewis dot structure
Molecular geometry (shape) = tetrahedral
Polarity = nonpolar (as long as all attached atoms are the same)
Bond angle = 109.5°
90
Q

MX2E whole thing

A 
Example = SO2
Draw Lewis dot structure
Molecular geometry (shape) = bent
Polarity = polar
Bond angle = n/a
91
Q

MX2E2 whole thing

A 
Example = H2O
Draw Lewis dot structure
Molecular geometry (shape) = bent
Polarity = polar
Bond angle = n/a
92
Q

MX3E whole thing

A 
Example = NH3
Draw Lewis dot structure
Molecular geometry (shape) = trigonal pyramid
Polarity = polar
Bond angle = n/a

Chemistry (12 decks)

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