Final Flashcards
1
Q
Define purpose of an experiment
A
A 2-3 sentence summary of what you want to find out by conducting the experiment or the question that the experiment will answer
2
Q
Independent Variable
A
What you change
3
Q
Dependent Variable
A
What you measure, depends on what you change
4
Q
Controlled Variable
A
Constant, what stays the same
5
Q
Conclusion of an experiment
A
Summarize how your results support or contradict your original hypothesis
6
Q
Density formula
A
D=m/v
7
Q
Metric system acronyms
A
King kilo Henry hecta Died deka By base (m, l, g) Drinking deci Chocolate centi Milk milli
8
Q
Convert from celsius to kelvin
A
C+273
9
Q
Convert from celsius to fahrenheit
A
(9/5)(C)+32=F
10
Q
Convert Fahrenheit to celsius
A
(5/9)(F-32)=C
11
Q
Accuracy
A
how close a measurement is to its standard or known value
12
Q
Precision
A
how close two or more measurements are to each other, regardless whether those measurements are accurate or not
13
Q
X axis is independent or dependent variable
A
independent variable
14
Q
Y axis is independent or dependent variable
A
dependent variable
15
Q
Sig fig rules
A
- All digits 1-9 are significant.
- Zeros between 1-9 are significant. Ex: 5007
- Trailing zeros: counted for if decimal
- Zeros only to place decimal point are NOT significant Ex: 0.00025
- Zeros following a decimal sig fig are significant Ex: .470000
16
Q
Chemical properties
A
properties that can be observed only when substances interact with one another
(Did you make something new?)
17
Q
Examples of chemical properties
A
rust
explosion
oxidation reduction
18
Q
Evidence of a chm rxn
A
change of color formation of ppt odor change in temp combustion
19
Q
Physical properties
A
properties that can be observed or measured without changing the composition of matter
20
Q
Examples of physical properties
A
texture mass volume length width height taste odor malleability flexibility viscosity hardness
21
Q
Examples of physical changes
A
melting cut wood phase changes break glass color
22
Q
Physical change
A
a change that effects only physical properties
23
Q
Chemical change
A
a change that produces one or more substances
24
Q
Element
A
cannot be further broken down by ordinary chemical means
25
Compound
combined chemically/ two or more elements chemically combined
26
Mixture
combined physically
27
Heterogeneous mixture
not the same throughout
28
Homogeneous mixture
same throughout
29
What are physical means to separate a mixture?
- evaporation
- chromatography
- distillation
- decantation
- filtration
- centrifuge
- chemical separation
30
% error formula
theo - exp/ (theo)
31
Law of Conservation of Mass
mass cannot be created nor destroyed
32
proton charge, location, amu
+, nucleus, 1
33
neutron charge, location, amu
neutral, nucleus, 1
34
electron charge, location, amu
-, electron cloud, very small
35
parts of an atom?
proton, neutron, electron
36
STUDY SCIENTISTS
okay
37
STUDY DIATOMICS
okay
38
what is the mass number equal to
protons + neutrons
39
isotopes
have same number of electrons, just different # of neutrons/ two of same element w/ diff number of neutrons
40
atomic number
of protons/ identifies number on periodic table
41
of neutrons
mass # - atomic number
42
of electrons
equal to protons if the atom is a neutral atom
43
of protons
atomic number
44
ion
when theres a charge + or -
45
mass number then atomic number when you write the symbol
okay
46
alkali metals
1A
47
alkaline-earth
2A
48
transition metals
3-12
49
halogens
7 valence electrons
50
noble gases
full shell, furthest to the right
51
lathanide
top bottom, 4f
52
actinide
lower bottom, 5f
53
super 7
H2, N2, O2, F2, Cl2, Br2, I2
54
increasing ionization energy
to the right and up
55
increasing atomic radius
to the left and down
56
increasing Ionic radius
to the left and down
57
increasing electron affinity
down: no trend
across: increases
58
increasing metallic characteristic
to the left and down
59
increasing electronegativity
to the right and up
60
order for quantum numbers
n, l, ml, ms
61
for quantum numbers, n is the
coefficient
62
for quantum numbers, l is the
s p d f
| 0 1 2 3
63
for quantum numbers, ml is the
-1, 0, +1
64
for quantum numbers, ms is the
up arrow +1/2
| down arrow -1/2
65
electromagnetic spectrum
```
Radio (red)
Microwave
Infrared
Visible
Ultraviolet
X-ray
Gamma ray ( higher frequency, smallest wavelengths) (purple)
```
66
photon
a tiny packet of energy
67
ground state of atoms
the lowest possible energy state of an atom, closest to the nucleus and most stable
68
excited state
atoms get zapped with energy
69
when the electron jumps back to the ground state, photons are ______
emitted
70
An electron transitioning from a 4s orbital to the ground state gives off yellow light. What color of light might be emitted by an electron transitioning from a 5s orbital to the ground state in the same atom?
green, blue or purple
71
difference between ionic and covalent
ionic metals
| covalent nonmetals
72
identify compounds as ionic or molecular
molecular non metal plus non metal
| ionic ALL metals according to nick
73
metal gives ______ to nonmetal in ionic bonding
electron
74
how are electrons transferred in covalent bonding
they are shared
75
ternary is
polyatomic ions
76
ionic naming
change ending to ide
77
what do transition metals need when naming
roman numerals
78
molecular naming
prefixes
79
HF
hydro _____ ic acid
80
acronym for polyatomic acids
i ate a dic
| ite ous
81
hydrates
name normal then add prefix to hydrate
82
example of hydrate
MnSO4 - 4H2O
| Manganese (ll) Sulfate Tetrahydrate
83
What are the types of reactions in equations
synthesis, double replacement, single replacement, decomposition
84
what is the type of reaction when carbon dioxide and water is formed
combustion
85
When is resonance formed when drawing compounds
when the double bond can go with multiple elements
86
what is the VSEPR theory
model used in chemistry to predict the geometry of individual molecules from the number of electron pairs surrounding their central atoms
87
what are the hybridizations of molecular orbitals
```
sp1
sp2
sp3
sp3d
sp3d2
```
88
polar
not symmetrical
89
nonpolar
symmetrical
90
exceptions to the octet rule
odd # of valence e' ex: NO
incomplete (mostly B or Be) ex: BF3
Expanded: PCl5
91
polar dissolves
polar
92
non polar dissolves
non polar
93
for solids as temperature increases solubility...
increases bitch
94
for gases as temperature increases solubility...
decreases slut
95
for gases as pressure increases solubility...
increases
96
for solids as pressure increases solubility...
stays the same
97
suspension
a temporary mixture; the particles will eventually settle
98
colloid
a mixture that scatters light and particles don't settle out
99
solution
a mixture that is homogeneous at the molecular level
100
emulsion
mixture of two or more liquids that are normally immiscible
101
electrolytes
a compound that conducts an electric current (aqueous sol.)
102
non-electrolytes
dissolve in solution/doesn't dissociate or conduct elect.
103
molarity formula
moles of solute/liters of solvent
104
molality
moles of solute/kg of solvent
105
What is the formula for dilutions
M1V1 = M2V2
106
What is the name for the "i value"
Vant hoff factor
107
How do you find the i value
You see how many ions the substance will disociate into
108
What is the formula for FP depression
K x m x i
K is the constant from the chart, m is for molality, and i is the vant hoff factor
109
What is the formula for BP elevation
K x m x i
K is the constant from the chart, m is for molality, and i is the vant hoff factor
110
chromatography
ink permeates up
111
intensive property
do not depend on the amount of matter
112
extensive property
do depend on the amount of matter
113
% yield
actual/theoretical
114
What is a real gas
Hip lot
High pressure
Low temperature
