TEAS Math and Chemistry Flashcards
1
Q
Properties of matter
A
CHOWS <3 T
color
hardness
odor
weight
shape
(density=Volume/Mass)
texture
2
Q
integer
A
positive, negative, zero
no fractions, no decimals
3
Q
prime factorization
A
break down a number into factors; break the factors down into factors; until everything is prime
4
Q
factors
A
two numbers that get multiplied together
5
Q
multiples
A
take a digit and multiply it by an integer in an series, (0->10+)
8x0
8x1
8x2
8x3
8x4
and so on
6
Q
prime number
A
can only be divided by itself and 1
1/1=1;
3/1=3; 3/3=1
7/1=7; 7/7=1
also includes 2
7
Q
prime factorization
A
break numbers into factors until all you have left is prime numbers
8
Q
GCF
greatest common factor
A
similar to prime factorization but instead of stopping at the prime numbers you choose the factor that is the same between two numbers
if they both share two numbers then multiply them together to get the GCF
9
Q
what are the least common multiples? (of 2 and 5)
A
first give multples of each number.
multiples of 2 are 2,4,6,8,10,12,14,16,18,20
multples of 5 are 5,10,15,20
pick the common multiples which are 10 and 20.
from that, pick the least common multiple, which is 10.
10
Q
x^1=
A
x
11
Q
x^0=
A
1
12
Q
x^-n =
A
1/x^n
13
Q
x^m * x^n=
A
x^m+n
14
Q
x^m / x^n =
A
x^ m-n
15
Q
perfect square numbers
A
1, 4, 9 , 25, 36, 49, 64, 81, 100
16
Q
8!
A
8x7x6…x2x1
integers only positive, not zero
17
Q
quadratic formula
A
x= -b +- sq (b^2 - 4ac) / 2a
18
Q
Mass
A
protons + neutrons on average
19
Q
proton mass
A
1.67 x 10^-27 kg = 1.007 amu
20
Q
weight
A
how much gravity is pulling an object downwards
21
Q
volume
A
how much space does this object take up
22
Q
density
A
mass per volume
23
Q
smallest unit of matter
A
atom
24
Q
atomic weight equals
A
protons + neutrons
average all isotopes
25
atomic mass
protons + neutrons
26
Ions
POS and NEG charged atoms
27
Isotope
atoms have equivalent protons but differing neutron numbers
28
atomic number
number at the top
the number of protons
determines the element
29
atomic energy
atoms want to be at the lowest energy state possible
30
N shell
where electrons are found
-lowest
31
Orbitals
1s
2s2p
3s3p3d
4s4p4d4f
| s holds 2 elect, 1 orb
p holds 6 elect, 3 orb
d holds 10 elect, 5 orb
## Footnote
1, 2, 3, 4 represent the principle energy level
32
electron configuration
arrangement of electrons in its ground state into orbitals around the nucleus
33
which electrons participate in chemical reactions
valence
34
octet rule?
atoms lose, gain, or share electrons to acquire 8 electrons
35
transition metals
thermal & electric conductors
shiny
Have higher melting points
Higher density
can be shaped & stretched
36
Non metals, who are they
C, N, O, P, S
COPS + N (n for non metal)
+ Halides ( F, Cl, Br, I)
37
properties of non metals
form small molecules
strong covalent bonds
weak intermolecular attraction
brittle, powder
form good electrical & thermal INSULATOR
38
Metalloids
Brittle (shiny or dull)
ductile or malleable
used as semiconductors
ex: Si or Ge, As, Sb, Te, Po, B
39
Ionic Bond
Bond between a metal and a nonmetal
40
Bond with the strongest intermolecular force?
hydrogen bonds
41
Covalent bond definition
a bond formed when atoms SHARE electron pair
42
Polar bond
unequal sharing, hydrophillic, dissolve in water
43
# [](http://)
intERmolecular forces
weak attraction between molecules (s, g, l)
44
intRA molecular forces
forces WITHIN molecules
strong
ex: hydrogen bonds
45
BP and FP of water
BP 212 F or 100 C
32 F or 0 C
46
How to get from farenheight to celcius
multply celcius by 9/5 and add 32
or subtract farenheight by 32, then F = 9/5 C
47
Solids properties
Definite shape & volume
no expand
smallest molecular movement
48
Solids properties
Conductor
FP
BP
49
Gas properties
expand
shape of container
lowest density
compressable
homogenous with other gases in a mixture
50
average speed of gas
20c
500 m/s
1100 mph
51
define sublimation
solid to gas
NO LIQUID STAGE
| sub = solid first
52
Deposition
GAS to SOLID
| deposit like into soil which is solid
53
evaporation
liquid to gas
54
condensation
gas to liquid
55
specific heat capacity
energy to raise temp of ONE GRAM of any substance by ONE degree C
| water is 4.18 j/g degree celcius
56
Cell membrane
cell structure which allows h20, 02, and co2 to pass through
57
osmolality
* concentration of solution
* solute particles per kilogram
57
hypertonic solution
conc. greater on outside of cell
water flow to the outside
58
facilitated diffusion
transport of substances across cell membrane using transporters but PASSIVE transport
59
definition of osmotic pressure
pressure that must be applied to prevent osmotic movement across a selectively permeable membrane
60
synthesis reaction
A+B = AB
61
Single replacement reaction
AB+C = A+ BC
62
decomposition
AB => A+B
63
double replacement reaction
AB + CD => AD + CB
64
Redox reaction (ox-red rxn)
oxidation = loss of electrons
reduction = gain of electron (or neg charge)
transfer of electrons
65
ingredients and product of Combustion
Oxygen is always the reactant
Water and CO2 always be the product
66
combustion equation
hydrocarbon + O2 => CO2 + H2O
CH4+ 2O2 => 2H2O + CO2
67
an endothermic reaction is what
absorbs heat. things get colder after its over
the heat it uses from the environment is used as the activation energy to help the reaction go along
68
exothermic reactions favors what kind of reactions
reverse reactions
69
human ph
7.35 to 7.45
70
definition of an acid
electrolytes that dissociate to release hydrogens in water
7 to 0 high H+
71
Base definition
substance that releases ions that combine with hydrogens
7 to 14
lower H+
72
pH level definition
how much H+ a substance contains
between 0 and 14
73
carbs
-recognition molecules
-chemical energy
- CO groups
- OH groups
- aldehyde groups (COHR)
- with long carbon chains
74
Polysaccharides are formed by
dehydration synthesis between two monosaccharides
75
polysaccharides examples
starch, glycogen, cellulose, heparin, peptidoglycan
76
disaccharides
sucrose, lactose, maltose
77
monosaccharides
glucose, fructose, galactose
tri = 3 C
pent = 5 C
hex = 6 C
78
hydroxide
OH
helps dissolve organic compounds
78
ribose has how many carbons
pentose, 5 carbon sugar
| hexose is 6 carbon
79
aldehyde
COHR
80
ketone
COR2
81
definition of starch and cellulose
glucose polymer that has glycosidic bonds
- can't be digested
82
DNA structure
deoxyribose sugar
phosphate
nitrogenous base
83
RNA structure
ribose
phosphate
nitrogen base
84
Mendels law of segregation
Each inherited trait comes from a pair of genes, one from each parent.
85
The law of independent assortment
Genes on different chromosomes are kept separate from each other so that the inheritance of one trait does not depend on the inheritance of another.
86
law of dominance
If a pair of genes is made up of one dominant and one recessive gene, the dominant gene will be expressed.
87
primary pathogen vs opportunitistic
primary will infect someone no matter what their immune system is
opportunitistic is infect only when immune system is weakened
88
capsid
protein coat for viruses that surrounds their DNA OR RNA
89
are viruses living or non living
non living
90
protozoans
eukaryotic animal like
rely on contaminated water or animals to infect humans
91
vector
typically an animal, that spreads disease to humans
mosquitos are animals
92
Protozoan examples
1. entamoeba histolytica
2. plasmodium
93
light microscope
uses two lenses to multiply the magnification
can view organelles
94
electron microscope
uses beam of electrons which are smaller than wavelengths of light.
can view more in smaller detail
95
strength of covalent vs ionic
ionic bond
96
what is a substance in chemistry
It can be made up of pure elements or pure compounds, but not mixtures of elements or mixtures of compounds.
Substances must have a definite chemical composition and distinct chemical properties.
97
If gravity changes, is mass and/or weight affected?
mass is unaffected, but weight it affected. mass is simply the amount of matter an object contains.
98
volume is dependant on:
| 3 things
Volume is dependent on the type of atoms that make up a substance, how those atoms are arranged, and what state of matter the substance is in.
98
Density
how concentrated the mass of a substance is.
99
FP and BP are dependant on
pressure
## Footnote
gas can be compressed into a liquid state, even if it has not cooled to the condensation point.
100
in chemistry, a color change indicates..
that a chemical change has taken place
101
atoms in liquids..
The atoms in a liquid have enough energy to break loose from each other, but not enough to escape completely.
102
gasses
The atoms in gases have enough energy to completely escape from each other and will move far apart. Gases will expand to fill the space they are given. They have very low densities and have no definite shape or volume.
103
plasma..
Plasma is a rare state of matter (on Earth, anyway) and consists of extremely high-energy particles that have become ionized. The electrified gas in a neon lamp is plasma. The matter in the Sun and other stars is in the plasma state.
104
The rate of a reaction can be increased by
temperature, pressure, or concentration and by adding a catalyst.
105
The law of conservation of mass
matter cannot be created or destroyed
106
one mole of an SI unit of measurement
6.022×1023
, or 602
sextillion atoms.
107
Pressure causes matter to become
from gas to liquid
| no l to s
108
the higher the concentration of reactants...
increased rate of reaction
109
is cellular respiration endo or exothermic
an exothermic reaction
combustion
110
solution
homogeneous mixture of two substances
111
molarity
mol/L
112
mole fraction
mole solute/(mol solute+solvent)
113
molality
mol solute/kg solvent
114
mass percentage
mass solute/mass solution
115
a buffer contains
a salt and either an acid or base
116
neutralization reaction
when an acid and base react in a solution. The product is water (made by combining the H from the acid and the OH from the base) and a salt.
117
what is a scientific conclusion
. A true scientific conclusion should be backed up with data and should not contain any inference or conjecture about things not directly measured.
118
what is a hypothesis
A prediction that has not been thoroughly tested yet made off of prior knowledge
119
what is a casual relationship
* A is always followed by B.
* the relationship between A and B can’t happen due to chance
* there are no other variables that can explain the relationship between A and B
120
steps of scientific method
1. identify a probem
2. ask the question
3. hypothesis
4. data collect
5. analyze (for errors)
6. conclude
7. peer review
121
a good scientific trial:
tests one variable at a time, has an adequate number of trials, and large sample size
122
what is the dependent variable
the variable of interest that will be measured during the course of the experiment. If a medication was being tested to increase bone density, the medication would be the independent variable and the bone density of the patients would be the dependent variable.
123
what is on the x and y axis in clinical trial data
X is the independant variable, Y is the dependant variable.
124
