Study Guide Flashcards
(232 cards)
0
Q
Law
A
Phenomenon in nature proven to occur when certain conditions meet
1
Q
Hypothesis
A
Propose Possible solutions to a problem or explanations for observation; suggesting such a possibility in scientific language; proposed explanation made on basis of the limited evidence at starting point
2
Q
Theory
A
(Model) is a set of tested hypothesis that gives an overall explanation of some part of nature
3
Q
Model
A
Activity to make something easy to understand
4
Q
Element
A
Substance that can’t be decomposed into simpler substances by chemical or physical means. Example: H ; Na
5
Q
Compound
A
Substance with constant composition that can be broken down into elements by chemical processes. Example: HNa ; PKO
6
Q
Mixture
A
Material of variable composition that contains two or more substances. Example: water + sugar ; the ocean
7
Q
Homogenous mixture
A
Mixture that is the same throughout; a solution. Example: gasoline; sugar water
8
Q
Heterogenous mixture
A
Mixture with different properties in different regions of the mixture. Example: jellybeans; the ocean
9
Q
Physical changes
A
A change in the form of a substance but not in its chemical nature; Chemical bonds are not broken in a physical change
10
Q
Chemical change
A
Change of substances in other substances through a reorganization of atoms; chemical reaction. Example: burning toast
11
Q
Pure substance
A
Substance with constant composition. Example: elements; compounds
12
Q
Calorie
A
Unit of measurement for energy; 1 calorie is the quantity of energy required to heat 1 g of water by 1°C
13
Q
Joule
A
Unit of measurement for energy. Example: 1 cal—> 4.184 joules
14
Q
Sig fig? 69678 g
A
5 sig figs
15
Q
Sig fig? 400607g
A
6 sig figs
16
Q
Sig fig? .00560g
A
5 sig figs
17
Q
Sig fig? 3.56 x 10^23g
A
3 sig figs
18
Q
Sig fig? 5600g
A
2 Sig figs
19
Q
Sig fig? 5600. g
A
4 Sig figs
20
Q
Exponential notation? .000005060 cm
A
5.06 x 10^-6
21
Q
Exponential notation? 5698000000 cm
A
5.698 x 10^9
22
Q
5.67 liters to milliliters
A
5.67L x 1000mL = 5670 mL
23
Q
567 Cm to m
A
567cm x .01m= 5.67 m
24
673 degrees Celsius to kelvin
673+273= 946K
25
37.6 degrees Fahrenheit to Celsius
37.6-32 / 1.80 = 3.1 Degrees Celsius
26
Given 100 g of a metal that has a volume of 63.5 mL, calculate its density. Using GESA and remember to use units
D=m/v D= 100g / 63.5 mL = 2g / mL
27
If the density of iron is .45 g/mL, what is the mass of a sample of metal that occupies 78 mL of volume?
.45= g/78mL ---> 35g
28
Cation
Positive ion; metal forms a cation by losing electrons
29
Anion
Negative ion; nonmetals form anions by gaining electrons
30
Nucleus
Extremely dense; accounts for almost all of the atom's mass; small dense of positive charge in an anion
31
Electron
Negatively charged particle that occupies the space around the nucleus of an atom
32
Proton
Positively charged particle
33
Neutron
Particle in atomic nucleus with a mass approximately equal to that of the proton but without charge
34
Na. What is the name of the element?
Sodium
35
Na. What family is it in?
Group 1A
36
Na. What period is in it?
Period 3
37
Na. What is its atomic number?
11
38
Na. How many protons does it have?
11
39
Na. How many neutrons does it have?
23-11= 12
40
Na. How many electrons does it have?
10
41
Na. With what element is it isoelectronic?
Neon
42
Na. Write a formula for a compound with this element and a halogen.
NaF
43
Na. Write a formula for this element combined with oxygen.
Na2O
44
Hydrogen acetate
HC2H3O2
45
Copper (II) nitrite
Cu(NO2)2
46
Nitrogen dioxide
NO2
47
Phosphorus trichloride
PCl3
48
Sodium phosphate
Na3PO4
49
Potassium carbonate
K2CO3
50
Phosphoric acid
H3PO4
51
Lead (IV) chloride
PbCl4
52
Tin (II) bromide
SnBr2
53
Ammonium hydroxide
NH4OH
54
Periodic acid
H5IO6
55
Iron (II) hydroxide
FeOH2
56
Carbon dioxide
CO2
57
Dinitrogen pentoxide
N2O5
58
Silver oxide
Ag2O
59
Aluminum nitride
AlN
60
Manganese (II) hydroxide
Mn(OH)2
61
Ammonium carbonate
(NH4)2CO3
62
Aluminum oxide
Al2O3
63
Antimony pentasulfide
JbS5
64
Manganese (II) oxide
MnO2
65
Sulfur dioxide
SO2
66
Iron (II) sulfate
FeSO4
67
Hypochlorous acid
HClO
68
Potassium permanganate
KMnO4
69
Silver chloride
AgCl
70
Copper (II) hydroxide
Cu(OH)2
71
Ammonium sulfide
(NH4)2S
72
Nickel (I) bromide
NiBr
73
Iron (II) oxide
FeO
74
Bromic acid
HBr
75
Ammonium Bisulfate
NH4HSO4
76
Mercury (I) sulfate
Hg2SO4
77
Iron (III) oxide
Fe2O3
78
Magnesium phosphate
Mg3(PO4)2
79
Nickel (I) bicarbonate
NiHCO3
80
Zinc hydroxide
ZnOH
81
Hydriodic acid
HI
82
Diphosphorus pentoxide
P2O5
83
Aluminum Phosphate
AlPO4
84
Define and give examples of physical changes
Change in substances through a reorganization of atoms. Example: rust; burning toast
85
Define and give examples of chemical changes
Change in the form of a substance, but not in the chemical nature (composition). Example: boiling; freezing water
86
Define mixtures and give examples
Variable composition of pure substances. Example: water and sugar/ocean
87
Define solution and give examples
Homogeneous mixture. Example: water; sugar water
88
Define pure substance and give examples
Compounds/H2O And Elements/H
89
What is the formula for density? What are the units of density?
D=m/v And g/mL or g/mL3
90
Convert 36 mg to kg?
36,000,000
91
How do you convert kcal to joules? Give an example.
```
Kcal---> joules. 1kcal ---> 4.184 joules.
Convert kcals (4) to joules.
4kcals x 4.184j = 16.736j
```
92
How do you find the volume of a cube with an edge length of .10cm?
*GESA* Length= .10cm
V= lxwxh
V= .1x.1x.1...... Since cube all sides equal
V= .001cm^3
93
What are the metric prefixes for 10^6 to 10^-9?
```
10^6= mega
10^-9= nano
```
94
How do you convert degrees Celsius to Kelvin?
```
T k= C+273
C=21
K= C+273
K= 21+273
K= 294K
```
95
What is the rule of significance for adding/subtracting?
Limiting term is the 1 with the smallest number of decimal places.
Example: 23.445 + 7.830 = 31.275---> corrected ---> 31.28
96
What is the rule of significance when multiplying/diving?
Number of significant figures in result is same as that in measurement with the smallest number of significant figures. Example: 1.342 x 5.5 = 7.381---> 7.4
97
Accuracy
How close you actually come to the location
98
Precision
Consistency in measurement
99
What are the rules for significant figures?
1. Nonzero integers always count as significant figures. Example: 1457 has 4 significant figures
2. Zeros
A. Leading zeros that precede all nonzero digits... NEVER count as significant figures. Example: .048 ---> 2 significant figures
B. Captive zeros that fall between nonzero digits... ALWAYS count as significant figures. Example: 16.07 ---> 4 significant figures
C. Trailing zeros are zeros at the end of the number... significant figure ONLY if contains decimal point. Example: 9.300---> 4 significant figures. Example: 150---> 2 significant figures
3. Exact numbers have UNLIMITED number of significant figures. Example: 1 in. ---> 2.54 cm, exactly. Example: 9 pencils (obtained by counting)
100
Step 1 of Scientific Method
Objective
101
Step 2 of Scientific Method
Research
102
Step 3 of Scientific Method
Hypothesis
103
Step 4 of Scientific Method
Procedure
104
Step 5 of Scientific Method
Data
105
Step 6 of Scientific Method
Analysis
106
Step 7 of Scientific Method
Conclusion
107
Step 8 of Scientific Method
Communicate Results
108
What's chemistry
Chemistry Deals with the materials of the universe and the changes that they undergo
109
What are two types of observations?
Qualitative. E.g: blue water
| Quantitative. E.g: 591 mL
110
Sig figs rule for mult/div.
You're answer can only have the same number of sig figs as your factor with the least
111
Sig figs when add/sub.
Answer has the same number of decimal places as the number with the least
112
Sig figs? 73.000g
5
113
Sig figs? 4.00809 km
6
114
Sig figs? 6.9cg
2
115
Sig figs? .0056m
2
116
Sig figs? 6.00 x 10^3 s
3
117
Sig figs? 301.0m
4
118
Sig figs? .0039km
2
119
How many decimeters in a meter?
10
120
What is the fundamental SI unit of mass in the metric system?
kg
121
How many mg are in 45.6g?
456
122
Mass formula
Density x Volume
123
Volume formula
Mass/density
124
Density formula
Mass/volume
125
What is the most abundant element on earth, including the crust, oceans, and atmosphere?
Oxygen
126
Which particle has the smallest mass?
Electron
127
Which Atomic particle determines the chemical behavior of an atom?
Electron
128
If you have 13 electrons and you lose one there are how many now?
14
129
If u lose an electron...
Add 1
130
If you gain an electron...
Lose 1
131
The mass number of an atom equals...
The number of protons plus the number of neutrons per atom
132
The number of protons in the nucleus of an atom is called...
Atomic number
133
What has approximately the same mass?
A proton and a neutron
134
In what pair does the components have the same charge?
A Neutron and a hydrogen atom
135
Left of staircase is
Metal
136
Right of staircase
Nonmetals
137
Where are metalloids?
In staircase
138
What's the first group of metals?
Alkali metals
139
What is the second group of metals?
Alkaline earth metals
140
Middle groups?
Transition metals
141
Halogens are in what group?
Group 7A
142
What group are the noble gases in?
Group 8A
143
The columns are...
Groups or families
144
The rows are...
Periods
145
The elements outside of the periodic table are called...
Inner transition metals or rare earths
146
The State of matter for an object that has neither definite shape nor definite volume is
Gaseous
147
The state of matter for an object that has a definite volume but not a definite shape is
Liquid
148
The state of matter for an object that has both definite volume and definite shape is
Solid
149
Anything that has mass and volume is called
Matter
150
Cooking an egg
Chemical change
151
Boiling water
Physical change
152
Ironing a shirt
Physical change
153
Burning gasoline
Chemical change
154
Decomposing water
Chemical change
155
Evaporating alcohol
Physical change
156
Sanding a table top
Physical change
157
Grinding grain
Physical change
158
Fermenting fruit juice
Chemical change
159
Dissolving sugar in water
Physical change
160
"Helium is very non reactive." Is an example of what kind of property
Chemical property
161
Driving a car
Chemical change
162
Sugar dissolving in coffee is only a ____ change
Physical
163
A tin can rusting is a ____ change
Chemical
164
Digesting a pizza is a ____ change
Chemical
165
In a chemical change,
Products are different substances from the starting materials
166
If iodine melts at 114*C and boils at 184*C, what is the physical state at 120*C?
Liquid
167
If iodine melts at 114*C and boils at 184*C, what is the physical state at 98*C?
Solid
168
If iodine melts at 114*C and boils at 184*C, what is the physical state at 250*C?
Gas
169
What describes a chemical property of gold
Good is an inert (nonreactive) metal
170
Burning paper is a ____ change
Chemical
171
Air is a ______
Pure compound
172
Homogenous is a ....
Mixture
173
Elements are on the...
Periodic table
174
A _____ always has the same composition
Compound
175
T/F. A compound can consist of one kind of element
False
176
An example of mixture is
The air in this room
177
examples of a pure substance
Elements, compounds, pure water, carbon Dioxide
178
T/F. Heterogenous compound
False. No such thing
179
Homogenous mixture=
A solution
180
Table salt is an example of
A compound
181
Chlorine gas is an example of
An element
182
Sand in water is an example of
Heterogenous mixture
183
Petroleum is an example of
Homogenous mixture
184
Caffeine is an example of
An element
185
Water is an example of
A compound
186
A solution can be distinguished from a compound by its
Variable composition
187
14k Gold
Mixture
188
Pure silver
Element
189
Aluminum
Element
190
Distiller water
Compound
191
Tap water
Mixture
192
Brass
Mixture
193
Tungsten
Element
194
Sodium chloride
Compound
195
Air
Mixture
196
Homogenous mixture?
Vodka
197
Helium is an example of
An element
198
The process of filtering a sand salt water mixture is a _____ process
physical
199
Example of What process requires chemical methods
Breaking a compound into its constituent elements
200
Example of What process is a chemical change
The light on a candle burns until a bell jar is placed over it for a period of time
201
What is an example of a homogeneous mixture
Gasoline
202
Diamond is a ____ state of matter
Solid
203
A ____ change involves a change in one or more physical properties but no change in the fundamental components that make up a substance
Physical
204
A ____ change involves a change in the fundamental components of the substance; a given substance changes into a different substance or substances
Chemical
205
Examples of Pure substances
Water, gold, ammonia
206
Examples of a compound
Water, ammonia
207
Smoke
Hetero
208
Air
Homo
209
Ocean
Hetero
210
River moving rapidly
Hetero
211
Gasoline
Homo
212
Mixture of 2 solids=
Alloy
213
Seeing difference
Hetero
214
Can't see difference
Homo
215
Alloid
Homo
216
Table sugar/salt
Pure substance
217
Mixture = 2+ elements combined (pure substance and physical)
Example: salt and sugar combo
218
Vinegar and milk combo
Hetero
219
Elements are
Atoms and molecules... Vice versus
220
Density
Physical
221
Dissolving water
Physical
222
Acid on blue jeans
Chemical
223
NACL
Compound
224
Paper tearing
Physical
225
Rubies, emeralds
Mixtures
226
A match
Chemical
227
Rocks
Mixture
228
Granite
Hetero
229
Physical property
Phase change, directly observable, bubbling with heat (sometimes)
230
Chemical property
Wasn't there before, behavior, things it'll do, bubbling with out heat, or with (sometimes)
231
Exact # of sig figs
Unlimited # of sig figs
