Chapters 1-4 Flashcards
1
Q
Chemistry
A
the science that deals with the materials of the universe and the changes that these materials undergo.
2
Q
Observation
A
Recognize the problem and state it clearly.
3
Q
Experiment
A
Searching for new information
4
Q
Theory
A
set of tested hypotheses that gives an overall explanation of some part of nature.
5
Q
Scientific Method
A
Process that lies at the center of scientific inquiry; Observe, Hypothesis, Experiment, Theory, Prediction, Law
6
Q
Hypothesis
A
Possible solutions or possible explanations for the observation
7
Q
Law
A
Summary of observed behavior
8
Q
Scientific Notation
A
expresses a number as a product of a number between 1-10 and the appropriate power of ten.
9
Q
Mega
A
M
1,000,000
10^6
10
Q
kilo
A
k
1000
10^3
11
Q
deci
A
d
0.1
10^-1
12
Q
centi
A
c
0.01
10^-2
13
Q
milli
A
m
0.001
10^-3
14
Q
micro
A
u
0.000001
10^-6
15
Q
nano
A
n
0.000000001
10^-9
16
Q
nonzero integers
A
always significant
17
Q
leading zeros
A
never significant
18
Q
captive zeros
A
always significant
19
Q
trailing zeros
A
significant in the presence of a decimal
20
Q
Celsius to Fahrenheit
A
F=1.80(C) +32
21
Q
Fahrenheit to Celcius
A
C=(F-32)/1.80
22
Q
Density
A
mass/volume
23
Q
Matter
A
has mass
occupies space
24
Q
Solid
A
rigid; has a fixed shape and volume
25
Liquid
has a definite volume but takes the shape of its container
26
Gas
has no fixed volume or shape; takes the shape and volume of its container.
27
Physical properties
odor, color, volume, state, density, melting point, and boiling point.
28
Chemical properties
ability to form new substances
29
Physical change
involves a change in one or more physical properties but no change in the fundamental components that make up the substance.
30
Chemical change
involves a change in the fundamental components of the substance; a given substance changes into a different substance or substances.
31
Element
cannot be broken down into other substances by chemical means.
32
Compound
substances that have the same composition no matter where we find them.
33
Mixture
something that has variable composition.
34
Pure substance
always has the same composition.
35
Homogenous Mixture
same throughout; does not vary in composition from one region to another.
36
Heterogenous Mixture
regions that have different properties from those of other regions.
37
Element symbols
abbreviations for the chemical elements
38
Atom
tiny particles that make up elements
39
Chemical Formula
the atoms are indicated by the element symbols, and the number of each type of atom is indicated by a subscript.
40
Electrons
negative particles in atoms
41
Nuclear atom
an atom with a dense center of positive charge around which tiny electrons moved in a space that was otherwise empty.
42
Nucleus
center of the atom
43
Proton
has the same magnitude of charge as the electron but it is positive.
44
Neutron
slightly more massive than a proton but has no charge
45
Isotopes
atoms with the same number of protons but different number of neutrons.
46
Atomic number
the number of protons in a nucleus
47
Mass number
protons + neutrons in nucleus
48
A X
| Z
x=symbol of the element
a= the mass number
z=the atomic number
49
Alkali metals
Group 1
50
Alkaline earth metals
Group 2
51
Halogens
Group 7
52
Noble Gases
Group 8
53
Physical properties of metal
Efficient conduction of heat and energy
Malleability
Ductility
Shiny
54
Diatomic molecules
Molecules made up of two atoms
| Red on periodic table
55
Ion
Charged entity
56
Cation
positive ion, produced when one or more electrons are lost from a neutral atom
57
Anion
negative ion, produced when electrons are gained by a neutral atom
58
Ionic compound
When a metal and nonmetal form a compound
59
Dalton's atomic theory
Elements are made of atoms
All atoms are identical
Atoms are different than atoms of another element
Atoms can combine with atoms of another element to form a compound that always has the same relative numbers and types of atoms.
Atoms are indivisible in chemical properties.
60
Rutherford (1911)
Explained the nuclear atom
Atom has a nucleus-dense center of charge
Electrons travel around nucleus
Proton has same magnitude but different charge
61
Rutherford and Chadwick (1932)
Most nuclei also contain neutron
| Neutron-more massive than proton- no charge
62
Plum pudding model
atom might be thought of as a uniform pudding of positive charge with enough electrons scattered within to counterbalance that positive charge.
William Thomson
63
Law of constant composition
A given compound always has the same composition no matter where it came from
64
NH3
ammonia
65
CH4
methane
66
NaCl
table salt
67
H
Hydrogen
| nonmetal
68
He
Helium
| nonmetal
69
Li
Lithium
| Metal
70
Be
Beryllium
| Metal
71
Na
Sodium
| Metal
72
Mg
Magnesium
| Metal
73
K
Potassium
| Metal
74
Ca
Calcium
| Metal
75
Sc
Scandium
| Metal
76
Ti
Titanium
| Metal
77
V
Vanadium
| Metal
78
Cr
Chromium
| Metal
79
Mn
Manganese
| Metal
80
Fe
Iron
| Metal
81
Co
Cobalt
| Metal
82
Ni
Nickel
| Metal
83
Cu
Copper
| Metal
84
Zn
Zinc
| Metal
85
B
Boron
| Nonmetal
86
C
Carbon
| Nonmetal
87
N
Nitrogen
| Nonmetal
88
O
Oxygen
| Nonmetal
89
F
Fluorine
| Nonmetal
90
Ne
Neon
| Nonmetal
91
Al
Aluminum
| Metal
92
Si
Silicon
| Semimetal
93
P
Phosphorous
| Nonmetal
94
S
Sulfur
| Nonmetal
95
Cl
Chlorine
| Nonmetal
96
Ar
Argon
| Nonmetal
97
Ga
Gallium
| Metal
98
Ge
Germanium
| Semimetal
99
As
Arsenic
| Semimetal
100
Se
Selenium
| Nonmetal
101
Br
Bromine
| Nonmetal
102
Kr
Krypton
| Nonmetal
103
Sr
Strontium
| Metal
104
Ag
Silver
| Metal
105
Cd
Cadmium
| Metal
106
Sn
Tin
| Metal
107
Sb
Antimony
| semimetal
108
I
Iodine
| nonmetal
109
Ba
Barium
| Metal
110
W
Tungsten
| Metal
111
Pt
Platinum
| Metal
112
Au
Gold
| Metal
113
Hg
Mercury
| Metal
114
Pb
Lead
| Metal
115
Bi
Bismuth
| Metal
116
Ra
Radium
| Metal
117
U
Uranium
| Metal
118
1kg
1000g
119
1L
1000mL
120
1m (cm)
100cm
121
1g
1000mg
122
1mL
1cm3
123
1m(mm)
1000mm
124
1 meter (in)
39.4 inches
125
1 km (mi)
.621 miles
126
1 gallon (li)
3.79 liters
