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chemistry Flashcards

1
Q

definition of precise

A

all the answers are close together

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2
Q

definition of accuracy

A

all the answers are near the targeted answer

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3
Q

kelvin and celsius conversion

A

273.15 + Celsius measurement = Kelvin measurement

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4
Q

adding one oxygen makes the name…

A

per____ate

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5
Q

removing 1 oxygen makes the name…

A

_____ite

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6
Q

removing 2 oxygens makes the name…

A

hypo____ite

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7
Q

hydrogen carbonate

A

HCO3 (-1)

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8
Q

hydrogen phosphate

A

HPO4 (-2)

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9
Q

bisulfite or hydrogen sulfite

A

HSO3(-1)

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10
Q

acetate

A

C2H3O2(-)

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11
Q

chromate

A

CrO4(-2)

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12
Q

peroxide

A

O2(-2)

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13
Q

phosphate

A

PO4(-3)

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14
Q

borate

A

BO3(3-)

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15
Q

carbonate

A

CO3(2-)

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16
Q

nitrate

A

NO3(-1)

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17
Q

arsenate

A

AsO4(-3)

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18
Q

sulfate

A

SO4(-2)

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19
Q

selenate

A

SeO4(-2)

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20
Q

chlorate

A

ClO3(-)

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21
Q

bromate

A

BrO3(-1)

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22
Q

iodate

A

IO3(-1)

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23
Q

difference between the element, mixture, and compound

A

elements: pure substances made from one type of atom, and cannot be broken down by simple chemical means
mixture: 2+ substances that are mixed together, and ARE NOT chemically bonded
compound: 2+ elements that are mixed together and chemically bonded, and CANNOT be separated and when they are created, it makes a new type of matter

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24
Q

difference between heat and temperature

A

heat is total energy of the particles in a substance, but temperature is the actual property that the substance exhibits and measures the energy of the motions of the particles

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25
Q

adding a hydrogen to “-ide” makes…

A

hydro_____ic acid

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26
Q

adding a hydrogen to “-ate” makes…

A

_______ic acid

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27
Q

adding a hydrogen to “-ite” makes…

A

_______ous acid

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28
Q

name/describe the states of matter triangle and their phases

A

solid to liquid = melting
liquid to solid = freezing
solid to gas = sublimation
gas to solid = deposition
liquid to gas = evaporation
gas to liquid = condensation

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29
Q

endothermic

A

absorbing heat

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30
Q

exothermic

A

releasing heat

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31
Q

evidences of chemical change

A

heat, light, color change, smell, bubbles, burning, precipitate (formation of a solid)

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32
Q

intensive property vs extensive property

A

intensive - depends on the identity of the matter (for example, color)
extensive - depends on amount of matter (for example, mass)

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33
Q

physical property

A

observation without changing matter type

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34
Q

chemical property

A

observation when matter changes

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35
Q

what are the fundamental chemical laws?(3)

A
  1. law of conservation of mass - mass of reactants is equal to mass of products
  2. law of definite proportions:
  3. law of multiple proportions:
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36
Q

what is the law of conservation of energy?

A

energy cannot be created or destroyed, only transferred

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37
Q

name the properties of each: solid, liquid and gas

A

solid - volume doesn’t expand, cannot be compressed, retain their shape, particles are held in fixed positions with high IMF

liquid- volume doesn’t change, weaker forces of attraction / IMF, particles can flow and they take the shape of their container, and cannot be compressed

gas - have no IMF at all, their particles move quickly and freely, can be compressed, has a much greater volume than solids and liquids, and it takes the shape and volume of its container

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38
Q

kinetic energy vs potential energy

A

kinetic energy is the motion of particles
potential energy is the potential for particles to move

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39
Q

intermolecular forces vs. intramolecular forces

A

intermolecular -
intramolecular -

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40
Q

3 postulates of kinetic theory?

A

particles are in constant motion, 2 substances at the same temperature will have the same amount of kinetic energy, and the molecules are incompressible

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41
Q

pure substance

A

all particles are identical

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42
Q

what is the molar mass? where can you find it?

A

molar mass is the mass of one mole of the element on the periodic table, and the number is the one below each element

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43
Q

empirical vs. molecular formula

A

molecular can be reduced, empirical cannot.

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44
Q

what is avogadros number? when do you use this?

A

6.022 x 10^23
used when converting mass to moles to formula units/molecules/particles

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45
Q

what are the steps to find percent composition by mass?

A
46
Q

what are the steps to find percent composition to empirical/molecular formula

A
47
Q

what is the orders to convert with moles, particles and mass?

A
48
Q

how to find the molecular formula using given empirical formula and molar mass?

A
49
Q

cations vs anions

A

cations = positive charge
anions = negative charge

50
Q

metals vs. nonmetals (which one gains e- and which loses e-?)

A

metals lose electrons
nonmetals gain electrons

51
Q

what is the octet rule?

A
52
Q

what are the metal physical properties?

A
53
Q

what are isotopes?

A

isotopes are different types of elements, and they have the same atomic # with different molar masses and diff physical properties

54
Q

what does it mean for a substance to be isoelectronic?

A

electron number is the same

55
Q

what is a valence e-

A

of electrons in the highest level in that substance

56
Q

what is electronegativity

A

particle’s ability to attract e- from other atoms

57
Q

what is atomic radius? what is the pattern on the periodic table?

A

atomic radius is the closeness of the electron and neutron

58
Q

what are allotropes

A

different types of isotopes

59
Q

what is ionization energy

A

energy needed to ionize a substance (going across it increases and going down it decreases)

60
Q

what is coulumbic attraction?

A

attraction between oppositely charged particles

61
Q

what Is the difference between mass # and atomic mass

A

mass # = protons + neutrons
atomic mass = # of protons

62
Q

how to read a isotope symbol?

A

the top left is mass # and bottom left is atomic mass

63
Q

what does it mean to be: saturated, unsaturated, and supersaturated?

A

saturated - the maximum amount of solute that can be dissolved has been reached

unsaturated - there is still more solute that is capable of being dissolved

supersaturated - solution has more dissolved solute than required for a saturated solution (imagine reaching the saturated point and then cooling the solution down)

64
Q

what is solubility?

A

the measure of the maximum amount of solute that can dissolve in a given amount of solvent at a specific temperature

65
Q

what is the difference between miscible and immiscible?

A

miscible - fully mixed in all proportions
immiscible - mixing polar and non polar together, doesn’t mix and separate instead

66
Q

definition of dilute and its equation

A

low amount of solute - MV = MV

67
Q

what does it mean to be concentrated

A

large amount of solute

68
Q

diff between colloid and suspension

A

colloid - particles are large enough to be seen
suspension - larger particles that can settle out over time and aren’t fully combined

69
Q

what does “like dissolves like” mean

A

polar dissolves polar, non polar does not dissolve polar. molecules with similar interactions will dissolve best.

70
Q

what is the difference between molality and molarity?

A

molality is moles/kg
molarity is moles/Liters

71
Q

what is the solution equation?

A

solution = solute + solvent (all in grams)

72
Q

what happens to solute when boiling point increases

A

they are directly related, so when boiling point increases, the solute increases

73
Q

what happens to solute when freezing point increases

A

freezing point is inversely related, so the solute decreases

74
Q

what is the difference in dissolved particles in ionic compounds compared to covalent ones?

A

ionic compounds break up the compounds, and covalent ones dont

75
Q

name all the “drill” molecular geometry names and their angles

A

linear (180)
trigonal planar (120)
bent (120)
tetrahedron (109.5)
trigonal pyramid (107)
bent (105)
trigonal bipyramidal (90)
seesaw (90)
T shaped (90)
linear (180)
octahedral (90)
square pyramidal (90)
square planar (90)

76
Q

polar bonds vs non polar bonds

A

polar bonds have partial charges and non polar charges dont

77
Q

what are the different types of bonds (hydrogen bonds, dipole dipole, and dispersion) and describe them

A

hydrogen bonds - strongest bonds, intermolecular force (on the outside of the molecule), uses covalent bonds, only between Hydrogen with O, N or F

dipole dipole interactions - positive and negative charges in dipoles attract each other, only occurs in polar molecules

dispersion forces - all molecules have dispersion forces, the more e- there are, the stronger the dispersion force is.

78
Q

what do the straight lines represent in the graph of temperature’s relationship with time/heat (the graph with the AB CD DE EF stuff and phases)

A

they represent potential energy (BC = fusion) (DE = vaporization)

79
Q

what is the difference between the Arrhenius and Bronsted Lowry acids and bases?

A

Arrhenius = acids have H+ and Oxygen and are all aqueous, and bases have OH

Bronsted Lowry = acids have H+ and bases have OH-

80
Q

what are conjugate acid and base pairs

A

conjugate acids received ion and conjugate bases lose an ion

81
Q

acids react with metals to create…

A

H2 (g) and chloride salt

82
Q

acids react with carbonates/bicarbonates to form…

A

H2O and CO2

83
Q

bases react with metal ion solutions to form…

A

H2 (g)

84
Q

what are spectator ions?

A

spectator ions don’t change across a reaction

85
Q

what are acid base indicators

A

solutions that change colors to indicate the pH of a solution

86
Q

what happens to the substance when they dissolve

A

they break apart

87
Q

describe the types of ions in basic, acidic, and neutral solutions

A

basic = hydroxide
acid = Hydrogen
neutral = equal concentration of both

88
Q

what is Le chatelier’s principle

A

when a stress is placed on a system @ equilibrium, the system will shift in order to minimize stress

89
Q

name the five ways to speed up chemical reactions

A

1) lowering the volume of the vessel
2) speeding up the particles
3) catalysts
4) individual particles instead of groups
5) more particles

90
Q

fill in the blanks: during chemical changes, reactants___________ and products _______

A

decrease, increase

91
Q

name all of the shifts associated with the following: reactants, products, temperature, volume

A

reactants - increase = right
decrease = left
products increase = left
decrease = right
temperature = whichever side its on will be what it acts as
volume = volume increases = pressure decrease = shifts to the side with more moles
volume decrease = pressure increase = shifts to side with less moles

92
Q

what are the steps to write and balance half reactions? what are the steps to write and balance in acidic solutions? In basic solutions?

A
93
Q

what is an antioxidant

A
94
Q

anode vs cathode

A

anodes oxidized, lose e-
cathodes reduce and gain e-

95
Q

how do you tell which element is the better oxidizing and reducing agent on the Ered paper?

A
96
Q

what are the 6 rules of oxidation numbers?

A

Oxygen is

97
Q

name which types of reactions are always, never, and sometimes redox reactions.

A
98
Q

heat of fusion

A
99
Q

surface tension

A

ability of a substance’s surface to resist an outside force

100
Q

viscosity

A

the substance’s resistance to flow

101
Q

boiling point

A

when the atm (atmospheric pressure) is equal to the vapor pressure

102
Q

vapor pressure

A
103
Q

name the type of solids and their characteristics

A
104
Q

what are the rules of polar bonds and non polar bonds

A

no lone pairs - non polar
one lone pair - polar
two lone pair - polar
all diff - polar

105
Q

stoichiometric mixture

A

the mixture is mixed in all proportions (balanced equation)

106
Q

how do you read the activity series?

A
107
Q

what are the difference between metal and nonmetal oxides? which one is basic and which one is acidic?

A

metal oxides are acidic because they result in H+
nonmetal oxides are basic because they result in OH

108
Q

limiting reactant

A

reactant that runs out first

109
Q

name all 7 diatomic elements

A

H, O, F, N,

110
Q

what is precipitation and neutralization in double displacement reactions

A
111
Q

describe how JJ Thompson discovered cathode rays

A

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