Chemistry Test 2 Flashcards
1
Q
abbreviation for an element
A
symbol
2
Q
abbreviation for a compound
A
formula
3
Q
abbreviation for a chemical change
A
chemical equation
4
Q
a whole number written to the left or in front of a symbol or formula
A
coefficient
5
Q
a coefficient represents…
A
number of molecules of that element
6
Q
a number written to the right and slightly below a symbol or formula
A
subscript
7
Q
a Subscript represents
A
total number of atoms in the element
8
Q
in a chemical equation, the substances which are on the left side of the equation are called…
A
reactants
9
Q
in a chemical equation, the substances which are on the right side of the equation are called
A
product
10
Q
formulas are usually expressed as the _________ portion written first; and a ___________ portion written last.
A
metallic
non-metallic
11
Q
__________ usually have positive oxidation numbers; whereas ___________ usually have negative oxidation numbers.
A
metals
non-metals
12
Q
in the expression of formulas, the products are obtained from the ___________; and essence “change partners”- that is _________ to _______ and __________ to _______.
A
reactants
plus to minus
minus to plus
13
Q
sometimes a group of atoms behaves as if it were a single atom. this group has its own charge and name and is called a ______________
A
Polyatomic Ion or Radical
14
Q
NH4 is the formula for __________
A
ammonium
15
Q
ammonium has a charge of ________
A
+1
16
Q
HCO3 is the formula for ________
A
Bicarbonate
17
Q
Bicarbonate has a charge of ______
A
-1
18
Q
C103 is the formula for______
confirm this formula
A
chlorate
19
Q
Chlorate has a charge of ______
A
-1
20
Q
OH is the formula for ________
A
Hydroxide
21
Q
Hydroxide has a charge of _________
A
-1
22
Q
NO3 is the formula for ________
A
Nitrate
23
Q
Nitrate has a charge of ________
A
-1
24
Q
NO2 is the formula for _______
A
Nitrite
25
Nitrite has a charge of ________
-1
26
CO3 is the formula for _______
Carbonate
27
Carbonate has a charge of _____
-2
28
SO4 is the formula for _______
Sulfate
29
Sulfate has a charge of ______
-2
30
SO3 is the formula for _________
Sulfite
31
Sulfite has a charge of _____
-2
32
BO3 is the formula for ________
Borate
33
Borate has a charge of ____
-3
34
B4O7 is the formula for _______
Tetraborate
35
Tetraborate has a charge of _____
-2
36
PO4 is the formula for _________
Phosphate
37
Phosphate has a charge of
-3
38
CN is the formula for _______
Cyanide
39
Cyanide has a charge of _____
-1
40
OC1 is the formula for __________
Hypochlorite
41
Hypochlorite has a charge of ______
-1
42
To determine the total number of ________ present in a compound, take the ______ number of the compound (if present) and multiply it by the _________ number of the element (if present) and finally multiple that by the number _______ the parenthesis (if present)
Atoms
Coefficient
Subscript
Outside
43
The only time parenthesis are used in Chemistry is when there is a ____________
polyatomic ion
44
atomic number of Hydrogen is ____ and atomic weight is _____
1
| 1
45
the most abundant element in the universe.....
hydrogen
46
what percentage of all elements in the universe contains hydrogen?
93%
47
hydrogen is the ONLY element on the periodic table that routinely contains NO ________
NEUTRONS
48
What elements are listed as OCCURENCE?
Hydrogen
Nitrogen
Halogen
Oxygen
49
common name for Halogen
salt formers (group VII elements)
50
all Halogens have _____ valence electrons in the outer most shell
7
51
In their ionic state, Halogens have a __________ number
negative
52
Types of Halogen
1. Chlorine
2. Fluorine
3. Bromine
4. Iodine
53
most abundant or common element in the earth's atmosphere
nitrogen
54
most abundant element on the surface of the earth. Present in the air that we breathe
oxygen
55
water is a___________
compound
56
Most abundant compound on the surface of the earth
H2O (water)
57
presence of calcium and magnesium salts within water
hardness
58
hard water will cause blood to _______ in a dead human body
clot
59
water hardness that can be removed by boiling
temporary hardness
60
water hardness that can not be removed by boiling
permanent hardness
61
compounds in which there is a chemical union between water and certain substances when they crystallize
hydrates
62
the splitting or tearing apart of compounds by the addition of water.
hydrolysis
63
chemical reaction between salt and water which yields or produces an acid and base of unequal strength
another definition for hydrolysis
64
removal or loss of water from a substance/dead human body. especially the face and lips
dehydration
65
dehydration is also called________________
desiccation
66
the disassociation of substances in solution into ions
ionization
67
disassociation means _______
breaking apart
68
example of ionization would be like putting a teaspoon of granulated salt into _________
water
69
a positively charged atom or group of atoms
cation
70
example of cation....
sodium
71
a negatively charged atom or group of atoms
anion
72
example of anion
chlorine
73
percentage of hydrogen ion in solution
pH
74
7 on the pH scale is _______
neutral
75
Below 7 on the pH scale is _________
acidic
76
Above 7 on the pH scale is _______ or ________
alkaline
| basic
77
to check a solution to being acidic or alkaline is by an indicator paper called ______________
litmus paper
78
The end color of any ACIDIC solution in chemistry would be.....
red
79
The end color of any ALKALINE or BASIC solution in chemistry would be.....
blue
80
water is a __________--
compound
81
Water will turn any color litmus paper _____________
white
82
litmus paper comes in what two colors?
blue
| red
83
the chemical reaction between acid and a base which always forms a salt and water
neutralization
84
ammonia will _________ formaldehyde
neutralizee
85
ammonia to formaldehyde reacts to form ________ and ________
urotropin (salt)
| water (by product)
86
CH2O (2 is a subscript) is the chemical formula for_____________
formaldehyde
87
compounds formed, other than water in the chemical reaction between acids and bases
salts
88
have a pH of less than 7
acids
89
3 types of acids
1. Arrhenius
2. Bronsted-Lowry
3. Lewis
90
yields or produces hydrogen or hydronium ions in aqueous solution.
Arrhenius acids
91
a solution which contains water
aqueous solution
92
this acid is chemically correct
arrhenius acid
93
acids which donates a proton
Bronsted-Lowry acid
94
Bronsted-Lowry acid is a ________ theory
false
95
substances that ACCEPT a pair of electrons
lewis acid
96
have a pH above 7
bases
97
3 types of bases
1. Arrhenius
2. Bronsted-Lowry
3. Lewis
98
substance which yields are produces hydroxide ions in aqueous solution
arrhenius base
99
a substance that accepts or gains a proton
Bronsted-Lowry base
100
Bronsted-Lowry base is a ________ theory
false
101
a substance that DONATES a pair of electrons
Lewis base
102
Physical properties of Oxygen
1. Odorless gas
2. Colorless gas
3. Tasteless gas
103
oxygen is heavier than
air
104
O2 is the formula for _____
oxygen
105
chemical properties of oxygen
1. combines with most elements to produce compounds called oxides
2. supports combustion
3. acts as oxidizing agent
106
compounds which contain two or more elements...one of which is oxygen
oxides
107
rapid oxidation in which heat and light are produced...usually accompanied by a flame
combustion
108
oxygen does not__________
burn
109
oxygen supports ___________
combustion
110
a slow oxidation that develops by itself into combustion
spontaneous combustion
111
REDuction & OXidation is known as...
REDOX
112
4 Properties of oxidation....
1. ADDITION of oxygen from a substance
2. LOSS of hydrogen from a substance
3. LOSS of electrons in an atom
4. INCREASE in oxidation number of a substance in a compound
113
Two ways to remember properties of oxidation
LEO
| OIL
114
LEO stands for...
Loss Of Electrons
115
OIL stands for...
Oxidation Is Loss of electrons
116
4 Properties of Reduction
1. LOSS of oxygen from a substance
2. GAIN of hydrogen to a substance
3. GAIN of electrons during reaction
4. DECREASE in the charge or oxidation number of an atom
117
which property is most important in oxidation?
LOSS of electrons in an atom
118
which property is most important in reduction?
GAIN of electrons during reaction
119
REDOX will never occur _________________ of each other
independently
120
In REDOX reaction, one substance is ______ and another is __________.
oxidized
| reduced
121
a comparison of oxidation numbers can be made of the elements on the _________ side of the equation to the same elements on the _____________ side. This comparison will determine which substance has been ______________ and which substance has been ____________.
reactant
product
oxidized
reduced
122
oxidizing agent is ____________
reduced
123
reducing agent is _________
oxidized
124
whatever is oxidized....
loses
125
whatever is reduced....
gains
126
two ways to remember properties of Reduction
GERs
| RIG
127
GERs stands for
Gain of Electrons
128
RIG stands for
Reductiion Is Gain of electrons
129
True solutions
crystalloids
130
Homogenous mixtures of two or more substances
true solutions (crystalloids)
131
solid solution that is a metallic substance composed of two or more metallic substances
alloy
132
component of a solution that is present in greatest quantity
solvent
133
solutions which contain relatively low concentrations of solute such as 1% / 1g
dilute solutions
134
solutions which contain relatively high concentrations of solute, such as 37% / 37g
concentrated solutions
135
component of a solution that is dissolved
solute
136
substance of a solution which does the dissolving
solvent
137
relative to embalming fluids, a synonym for the solvent of water would be called the.....
vehicle
138
amount of solute present in a given amount of solvent at saturation describes _______
saturation point
139
any solution which contains the maximum amount of solute which it is capable of dissolving
saturated
140
any solution which contains less than the maximum amount of solute which it is capable of dissolving.
unsaturated
141
examples of unsaturated
dilute
| concentrated
142
any solution which contains more solute than it is capable of dissolving
supersaturated
143
When formaldehyde gas is dissolved in water the resulting solution is called
formalin
144
concentrations of solutions are quantitatively expressed in what 2 methods?
1. Percentage method
| 2. Ratio method
145
this is an example of what method????
The percent of solution to % of solute.
By weight or volume - formaldehyde: 37% by weight, 40% by volume
percentage method
146
this is an example of what method????
ratio method
147
not sure what this means...confirm
parts per million...cubits of air
148
The number of grams of pure formaldehyde gas in 100 milliliters of solutions defines
index
149
The diffusion of fluids thru semi-permeable membranes or porous partitions describes
osmosis
150
__________ does not need a semi-permeable membrane
diffusion
151
Two solutions of equal concentrations are called
isotonic
152
more or excessive solute
hypertonic solutions
153
less or below - less solute
hypotonic solutions
154
In addition to true solutions, other solution like systems are ___________ and ____________ which differ primarily in particle size.
emulsions
| suspensions
155
Inasmuch as solutions are diffusible, they therefore lend themselves to _________ which is diffusion through membranes.
osmosis
156
A __________ solution is one that contains a lower solute concentration that of the other solution. This type solution may cause cells to_______ which results in _______.
hypotontic
burst
hemolysis
157
Edematous remains would require a more ____________ solution in order to __________________ from body tissues.
hypertonic (plasmoptysis)
| withdraw moisture
158
Consequently, a hypertonic solution is one that contains a higher solute concentration than the opposing solution. This, in turn will cause body cells to _________which is called __________________.
shrink
| crenation (plasmolysis)
159
Dehydrated bodies should be injected with a ______ solution; whereas edematous bodies should be injected with a ____________ solution. Why? ???
hypotonic
hypertonic
You'd want it to plump up
160
______________are yet another type of solution like substance only designated by particle size.
emulsions
161
examples of emulsions...
Blood plasma
Egg white solution
Mayonnaise
Oil & Vinegar
162
are mixtures such as milk of magnesia
suspensions
