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TEAS > TEAS Math and Chemistry > Flashcards

TEAS Math and Chemistry Flashcards

1
Q

Properties of matter

A

CHOWS <3 T

color
hardness
odor
weight
shape

(density=Volume/Mass)

texture

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2
Q

integer

A

positive, negative, zero
no fractions, no decimals

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3
Q

prime factorization

A

break down a number into factors; break the factors down into factors; until everything is prime

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4
Q

factors

A

two numbers that get multiplied together

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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

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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

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7
Q

prime factorization

A

break numbers into factors until all you have left is prime numbers

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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

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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.

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10
Q

x^1=

A

x

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11
Q

x^0=

A

1

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12
Q

x^-n =

A

1/x^n

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13
Q

x^m * x^n=

A

x^m+n

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14
Q

x^m / x^n =

A

x^ m-n

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15
Q

perfect square numbers

A

1, 4, 9 , 25, 36, 49, 64, 81, 100

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16
Q

8!

A

8x7x6…x2x1

integers only positive, not zero

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17
Q

quadratic formula

A

x= -b +- sq (b^2 - 4ac) / 2a

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18
Q

Mass

A

protons + neutrons on average

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19
Q

proton mass

A

1.67 x 10^-27 kg = 1.007 amu

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20
Q

weight

A

how much gravity is pulling an object downwards

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21
Q

volume

A

how much space does this object take up

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22
Q

density

A

mass per volume

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23
Q

smallest unit of matter

A

atom

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24
Q

atomic weight equals

A

protons + neutrons
average all isotopes

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25
Q

atomic mass

A

protons + neutrons

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26
Q

Ions

A

POS and NEG charged atoms

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27
Q

Isotope

A

atoms have equivalent protons but differing neutron numbers

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28
Q

atomic number

A

number at the top
the number of protons
determines the element

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29
Q

atomic energy

A

atoms want to be at the lowest energy state possible

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30
Q

N shell

A

where electrons are found
-lowest

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31
Q

Orbitals

A

1s
2s2p
3s3p3d
4s4p4d4f

s holds 2 elect, 1 orb
p holds 6 elect, 3 orb
d holds 10 elect, 5 orb

1, 2, 3, 4 represent the principle energy level

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32
Q

electron configuration

A

arrangement of electrons in its ground state into orbitals around the nucleus

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33
Q

which electrons participate in chemical reactions

A

valence

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34
Q

octet rule?

A

atoms lose, gain, or share electrons to acquire 8 electrons

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35
Q

transition metals

A

thermal & electric conductors
shiny
Have higher melting points
Higher density
can be shaped & stretched

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36
Q

Non metals, who are they

A

C, N, O, P, S
COPS + N (n for non metal)
+ Halides ( F, Cl, Br, I)

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37
Q

properties of non metals

A

form small molecules
strong covalent bonds
weak intermolecular attraction
brittle, powder
form good electrical & thermal INSULATOR

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38
Q

Metalloids

A

Brittle (shiny or dull)
ductile or malleable
used as semiconductors

ex: Si or Ge, As, Sb, Te, Po, B

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39
Q

Ionic Bond

A

Bond between a metal and a nonmetal

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40
Q

Bond with the strongest intermolecular force?

A

hydrogen bonds

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41
Q

Covalent bond definition

A

a bond formed when atoms SHARE electron pair

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42
Q

Polar bond

A

unequal sharing, hydrophillic, dissolve in water

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43
Q

intERmolecular forces

A

weak attraction between molecules (s, g, l)

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44
Q

intRA molecular forces

A

forces WITHIN molecules
strong
ex: hydrogen bonds

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45
Q

BP and FP of water

A

BP 212 F or 100 C
32 F or 0 C

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46
Q

How to get from farenheight to celcius

A

multply celcius by 9/5 and add 32

or subtract farenheight by 32, then F = 9/5 C

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47
Q

Solids properties

A

Definite shape & volume
no expand
smallest molecular movement

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48
Q

Solids properties

A

Conductor
FP
BP

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49
Q

Gas properties

A

expand
shape of container
lowest density
compressable
homogenous with other gases in a mixture

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50
Q

average speed of gas

A

20c
500 m/s
1100 mph

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51
Q

define sublimation

A

solid to gas
NO LIQUID STAGE

sub = solid first

52
Q

Deposition

A

GAS to SOLID

deposit like into soil which is solid

53
Q

evaporation

A

liquid to gas

54
Q

condensation

A

gas to liquid

55
Q

specific heat capacity

A

energy to raise temp of ONE GRAM of any substance by ONE degree C

water is 4.18 j/g degree celcius

56
Q

Cell membrane

A

cell structure which allows h20, 02, and co2 to pass through

57
Q

osmolality

A
  • concentration of solution
  • solute particles per kilogram
57
Q

hypertonic solution

A

conc. greater on outside of cell
water flow to the outside

58
Q

facilitated diffusion

A

transport of substances across cell membrane using transporters but PASSIVE transport

59
Q

definition of osmotic pressure

A

pressure that must be applied to prevent osmotic movement across a selectively permeable membrane

60
Q

synthesis reaction

A

A+B = AB

61
Q

Single replacement reaction

A

AB+C = A+ BC

62
Q

decomposition

A

AB => A+B

63
Q

double replacement reaction

A

AB + CD => AD + CB

64
Q

Redox reaction (ox-red rxn)

A

oxidation = loss of electrons
reduction = gain of electron (or neg charge)

transfer of electrons

65
Q

ingredients and product of Combustion

A

Oxygen is always the reactant
Water and CO2 always be the product

66
Q

combustion equation

A

hydrocarbon + O2 => CO2 + H2O

CH4+ 2O2 => 2H2O + CO2

67
Q

an endothermic reaction is what

A

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
Q

exothermic reactions favors what kind of reactions

A

reverse reactions

69
Q

human ph

A

7.35 to 7.45

70
Q

definition of an acid

A

electrolytes that dissociate to release hydrogens in water
7 to 0 high H+

71
Q

Base definition

A

substance that releases ions that combine with hydrogens

7 to 14
lower H+

72
Q

pH level definition

A

how much H+ a substance contains
between 0 and 14

73
Q

carbs

A

-recognition molecules
-chemical energy
- CO groups
- OH groups
- aldehyde groups (COHR)
- with long carbon chains

74
Q

Polysaccharides are formed by

A

dehydration synthesis between two monosaccharides

75
Q

polysaccharides examples

A

starch, glycogen, cellulose, heparin, peptidoglycan

76
Q

disaccharides

A

sucrose, lactose, maltose

77
Q

monosaccharides

A

glucose, fructose, galactose
tri = 3 C
pent = 5 C
hex = 6 C

78
Q

hydroxide

A

OH
helps dissolve organic compounds

78
Q

ribose has how many carbons

A

pentose, 5 carbon sugar

hexose is 6 carbon

79
Q

aldehyde

A

COHR

80
Q

ketone

A

COR2

81
Q

definition of starch and cellulose

A

glucose polymer that has glycosidic bonds
- can’t be digested

82
Q

DNA structure

A

deoxyribose sugar
phosphate
nitrogenous base

83
Q

RNA structure

A

ribose
phosphate
nitrogen base

84
Q

Mendels law of segregation

A

Each inherited trait comes from a pair of genes, one from each parent.

85
Q

The law of independent assortment

A

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
Q

law of dominance

A

If a pair of genes is made up of one dominant and one recessive gene, the dominant gene will be expressed.

87
Q

primary pathogen vs opportunitistic

A

primary will infect someone no matter what their immune system is
opportunitistic is infect only when immune system is weakened

88
Q

capsid

A

protein coat for viruses that surrounds their DNA OR RNA

89
Q

are viruses living or non living

A

non living

90
Q

protozoans

A

eukaryotic animal like
rely on contaminated water or animals to infect humans

91
Q

vector

A

typically an animal, that spreads disease to humans
mosquitos are animals

92
Q

Protozoan examples

A
  1. entamoeba histolytica
  2. plasmodium
93
Q

light microscope

A

uses two lenses to multiply the magnification

can view organelles

94
Q

electron microscope

A

uses beam of electrons which are smaller than wavelengths of light.
can view more in smaller detail

95
Q

strength of covalent vs ionic

A

ionic bond

96
Q

what is a substance in chemistry

A

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
Q

If gravity changes, is mass and/or weight affected?

A

mass is unaffected, but weight it affected. mass is simply the amount of matter an object contains.

98
Q

volume is dependant on:

3 things

A

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
Q

Density

A

how concentrated the mass of a substance is.

99
Q

FP and BP are dependant on

A

pressure

gas can be compressed into a liquid state, even if it has not cooled to the condensation point.

100
Q

in chemistry, a color change indicates..

A

that a chemical change has taken place

101
Q

atoms in liquids..

A

The atoms in a liquid have enough energy to break loose from each other, but not enough to escape completely.

102
Q

gasses

A

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
Q

plasma..

A

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
Q

The rate of a reaction can be increased by

A

temperature, pressure, or concentration and by adding a catalyst.

105
Q

The law of conservation of mass

A

matter cannot be created or destroyed

106
Q

one mole of an SI unit of measurement

A

6.022×1023
, or 602
sextillion atoms.

107
Q

Pressure causes matter to become

A

from gas to liquid

no l to s

108
Q

the higher the concentration of reactants…

A

increased rate of reaction

109
Q

is cellular respiration endo or exothermic

A

an exothermic reaction
combustion

110
Q

solution

A

homogeneous mixture of two substances

111
Q

molarity

A

mol/L

112
Q

mole fraction

A

mole solute/(mol solute+solvent)

113
Q

molality

A

mol solute/kg solvent

114
Q

mass percentage

A

mass solute/mass solution

115
Q

a buffer contains

A

a salt and either an acid or base

116
Q

neutralization reaction

A

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
Q

what is a scientific conclusion

A

. A true scientific conclusion should be backed up with data and should not contain any inference or conjecture about things not directly measured.

118
Q

what is a hypothesis

A

A prediction that has not been thoroughly tested yet made off of prior knowledge

119
Q

what is a casual relationship

A
  • 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
Q

steps of scientific method

A
  1. identify a probem
  2. ask the question
  3. hypothesis
  4. data collect
  5. analyze (for errors)
  6. conclude
  7. peer review
121
Q

a good scientific trial:

A

tests one variable at a time, has an adequate number of trials, and large sample size

122
Q

what is the dependent variable

A

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
Q

what is on the x and y axis in clinical trial data

A

X is the independant variable, Y is the dependant variable.

124
Q
A

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