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Honors Chemistry > Semester 1 Final > Flashcards

Semester 1 Final Flashcards

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1
Q

Matter has

A

substance, stuff, it is anything that has mass and volume

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2
Q

___is the property of matter that can be measured

A

mass

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3
Q

the amount of space matter takes up is called

A

volume

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4
Q

Mass is measured in

A

milligrams(mg), grams(g)(1000mg), and kilograms(kg)(1000mg)

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5
Q

Volume is measured in

A

milliliters(mL), and liters(L)(1000mL)

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6
Q

calculating the conversion of some units to another unit is

A

information given x conversion factor(s) = information sought

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7
Q

elements

A

building material of all matter, the purest form

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8
Q

compound

A

different elements combined in specific ratios, represented by a chemical formula

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9
Q

ratios of the elements in compounds __ change

A

never

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10
Q

ratio of carbon to oxygen atoms in CO2

A

1:2

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11
Q

molecules

A

multiple atoms of the same element combined, not compounds

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12
Q

Aqueous Phase

A

when a substance forms a mixture with water ex. seawater, vinegar. It is not a liquid

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13
Q

Homogenous Mixture

A

one phase, solution or pure substance ex. sugar + water

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14
Q

Heterogenous mixture

A

2 or more phases, can be separated by filtration or extraction ex. sand + water

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15
Q

Reactivity

A

property describing how easily an element will combine with other substance to form new compounds

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16
Q

the more reactive an element is,

A

the more rapidly it combines with other elements

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17
Q

Atomic Mass

A

mass of an atom, measured in atomic mass units(amu)

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18
Q

Periodic table

A

arranges the 118 chemical elements into rows and columns, based on a set of repeating properties

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19
Q

Vertical columns

A

called groups

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20
Q

horizontal rows

A

called periods

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21
Q

in chemistry, positive ions can be called

A

salts

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22
Q

the elements on the periodic table can be grouped into

A

metals, metalloids, and nonmetals

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23
Q

atom

A

the smallest particle of an element retaining its identity in a chemical reaction; made of subatomic particles

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24
Q

subatomic particles

A

protons, neutrons, and electrons

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25
Q

proton

A

subatomic particle with a positive charge equal to about 1 amu, p+

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26
Q

electron

A

subatomic particle with a negative charge equal to about 0.000055 amu, e-

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27
Q

neutron

A

subatomic particle with no charge equal to about 1 amu, n0

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28
Q

nucleus

A

dense central core of atoms made up of neutrons and protons - makes up most of an atom’s mass

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29
Q

electron cloud

A

electrons surrounding, orbiting, the nucleus - makes up most of an atom’s volume

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30
Q

atomic mass unit(amu)

A

unit used to measure the mass of subatomic particles

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31
Q

atomic number

A

number of protons in an atom, which determines the identity of an element

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32
Q

normal atoms have what charge and why

A

neutral because the number of protons and electrons is the same

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33
Q

Mass number

A

total number of protons and neutrons in an atom

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34
Q

Isotope

A

atom with the same number of protons but a different number of neutrons, therefore, different atomic numbers

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35
Q

to calculate average atomic mass of isotopes of an element

A

create weighted average, so use ratios as percentages that multiply amus and add together
(0.9)(20amu)+(0.09)(22amu)+(0.01)(21amu)= 20.19amu

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36
Q

transmutation

A

conversion of one element into an atom of another element, occurs naturally thru radioactive decay, when nuclei emit particles an rays

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37
Q

Nuclear Stability is controlled by two forces

A

electrostatic repulsion force and the strong nuclear force

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38
Q

electrostatic repulsion force

A

repels positively charged particles, so when protons in an atom increase, the force increases

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39
Q

strong nuclear force

A

short range force on atoms independent of charge, when overall number of subatomic particles in nucleus increases, force increases

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40
Q

the large an atom’s nucleus, the more the __ force overpowers the __ force

A

repulsion, strong

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41
Q

an imbalance in force in an nucleus creates

A

instability

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42
Q

Valley of stability

A

atoms with atomic numbers under 80

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43
Q

alpha decay

A

decay of an element to stabilize nucleus that involves the emission of an alpha particle, or the nucleus of a helium, 2 neutrons and 2 protons

alpha particle(4/2 He) emitted and atom changes

222/88 Ra –> 4/2 He + 218/80 Rn

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44
Q

quirks

A

make up neutrons and protons,
-up quirks
-down quirks
proton have 2 up quirks and 1 down quirk
neutron has 1 up quirk and 2 down quirks

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45
Q

beta decay B- (negative)

A

decay of an element to stabilize nucleus that involves the transformation of a neutron into a proton, creating a high energy electron

90/39Y – B- –> 90/40 Zr

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46
Q

In beta decay, the atomic number __ while the mass number __

A

changes, remains the same

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47
Q

beta decay B+ (positive)

A

decay of an element to stabilize nucleus that involves the transformation of a proton into a neutron, creating a positron(positive electron)
49/25 Mn –> 49/24 Cr + 0/+1 e

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48
Q

light is made up of

A

waves with varying wavelength

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49
Q

the shorter the wavelength of a light

A

the more energy it has

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50
Q

blue light has __ wavelengths while red light has __ wavelengths

A

longer, shorter

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51
Q

when heated, some electrons get “excited”, moving

A

father from the nucleus to the next orbit, but its instability causes it to fall to a lower energy state by emitting a photon of specific energy

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52
Q

an energy input causes electrons to move up to

A

excitation, followed by an energy output, leading to relaxation

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53
Q

electron shells

A

circles, orbits, or electrons around the nucleus

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54
Q

each electron shell represents a discrete

A

(specific) energy level

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55
Q

Atomic Emission Spectrum(AES)

A

pattern formed when light emitted by an element, unique to every element, because an atom in a gas state emits light when energy is absorbed

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56
Q

energy is quantized in energy input and output

A

only discrete, specific, values are allowed, the opposite is continuous values

57
Q

an electron can change energy level to one higher only if

A

it absorbs the difference in energy levels

58
Q

light not only acts like waves, also like

A

particles

59
Q

Quanta

A

particles of energy, in quantum theory, the smallest amounts of energy in nature

60
Q

an energy gap in electron shells gets continuously __ the farther away from nucleus

A

smaller

61
Q

valence shell

A

outermost atomic shell, all the electrons in btwn nucleus and valence shell are called core electrons

62
Q

valence electrons

A

electrons on outermost shell of an atom, which affect a chemical’s reactivity, as chemicals with the same number of valence electrons have similar properties

63
Q

HONC Rule

A

hydrogen makes one bond, every oxygen makes two bonds, every nitrogen makes three bonds, every carbon makes four bonds. These are covalent

64
Q

Isomers

A

molecules with different structural formula but same molecular formula. Have different chemical and physical properties

65
Q

Because of 3D aspect of molecular structure, structural formulas show sequence in which atom is connected to next; can be rotated, as the __ and __ of connections are what matter

A

number, type

66
Q

VSEPR(Valence Shell Electron Pair Repulsion) Theory

A

Tendency for electron pairs to be as far apart from one another as possible

67
Q

Bond Rotation

A

p-orbital overlap in carbon-carbon single bond allows for axel rotation
conformation- structures differing only differing in rotations

68
Q

double p-orbital overlap in a carbon-carbon results in fixed geometry, double bond can __, and single bond can’t

A

rotate

69
Q

presence of double bond(two pairs of electrons shared) enables

A

cis/trans-isomerism
cis-symmetrical sides to atom in terms of non-hydrogen group
trans- non-hydrogen groups are diagonal

70
Q

functional group

A

an atom or group of atoms within a molecule that has similar chemical properties whenever it appears in various compounds. Even if other parts of the molecule are quite different, certain functional groups tend to react in certain ways.

71
Q

Structural (constitutional) isomers have the same molecular formula but ___. Stereoisomers have ___ molecular formulas and arrangements of atoms.

A

have a different bonding arrangement among the atoms
identical

72
Q

where are electronegativity values the highest on the periodic table
where are they lowest

A

bottom right corner,
top left

73
Q

difference in electronegativity in covalently bonded atoms determines

A

polarity, the larger the difference the more polar, because the atom with higher electronegativity will develop a partial negative charge relative to the other in bond, and single bonds with bigger difference lead to greater bond dipoles

74
Q

differences in electronegativity

A

0-0.4 - nonpolar covalent
0.5-1.8 polar covalent
>1.8 Ionic Bond

75
Q

dispersion forces are the result of electrostatic interactions that are merely __ and __, occuring in non-polar molecules

A

temporary and fluctuating

76
Q

dipole dipole interactions

A

stronger than dispersion because molecules more polar

77
Q

hydrogen bonding

A

strongest type of intermolecular interaction because H covalently bonded to N,O, and F and a dipole by electronegative atom(N,O,F) in a different molecule or a different part of the same molecule

78
Q

intramolecular forces of attraction(ionic and covalent) are ____ than intermolecular forces of attraction

A

stronger

79
Q

vapor pressure and boiling point are directly related to the strength of the

A

intermolecular interactions

P.S.
melting points also tend to correlate with interaction strength, but because the interactions are only rearranged, in melting, the relations are more subtle

80
Q

ionic solids have __ vapor pressures, __ melting points, and __ boiling points

A

low, high, high,
they conduct electricity only when ions are mobile, as when the ionic solid is melted or dissolved in water

81
Q

kelvin temperature of a sample of matter is directly proportional to the

A

average kinetic energy of the particles in the sample

82
Q

density of a substance formula

A

p=m/v
density = mass/volume

volume is inversely proportional(when increases, density decreases)
mass is directly proportional(when increases, density increases)

ex. mg/mL, g/L, kg/m^3 = mg,g,kg / mL, L, cm^3, m^3

83
Q

critical point on phase diagram

A

the point in temperature and pressure on a phase diagram where the liquid and gaseous phases of a substance merge together into a single phase. Beyond the temperature of the critical point, the merged single phase is known as a supercritical fluid .

84
Q

triple point on phase diagram

A

3 phases coexist

85
Q

chemical equilibrium

A

dynamic condition where the rate of forward reaction equals the rate of the reverse reaction

86
Q

Kinetic molecular theory of Gasses(keep in mind these are laws in ideal conditions)

A
  1. Gasses are comprised of small molecules far apart from each other
  2. Collisions between gas molecules and the wall of the container are elastic, meaning that the molecules maintain speed and bounce
  3. Gas molecules are in constant random motion
  4. There is minimum/no attractive force between Gas molecules
  5. Temperature is directly proportional to Kinetic energy K.E.=1/2m(mass) x v(velocity)^2
87
Q

gas pressure

A

caused by forces of collisions between molecules of gas and container walls. As the container is shrunk, the pressure and collisions increase.

88
Q

gasses with higher temperature will have

A

faster particles –> more collisions –> higher pressure

opposite for lower temp

89
Q

In Real Gasses there is/is not attractive force when compressed?

A

is, and kinetic energy is insufficient to overcome the attractive force

90
Q

PSI is a unit used to measure __,
given by formula __

A

pressure,
pounds/inch^2

91
Q

how do liquids behave in comparison to gasses

A

particles are in constant random motion just as gasses, however, particles are closer together because of intermolecular forces of attraction. liquid molecules are also less mobile, and there is less void space in between particles
Both liquids and gasses can diffuse

92
Q

unlike gasses, fluids are/are not compressible?

A

are not, because fluid density is about 1000x of gas of same substance

93
Q

liquid property of surface tension

A

liquids decrease surface area to smallest possible size, done by adjacently-pulling force on liquid surface. this property resists penetration

94
Q

capillary action

A

attraction of the surface of a liquid to the surface of a solid

95
Q

vaporization vs evaporation

A

vaporization any conversion from liquid to gas(including boiling or equilibrium), while evaporation does not include the liquid reaching its boiling point yet particles from liquid surface escape to atmosphere

96
Q

Liquids with higher temperatures have a __ proportion of molecules of __ kinetic energy(enough to evaporate) in comparison to liquids with lower temperatures

A

higher
high

97
Q

gas to liquid
gas to solid
liquid to solid
liquid to gas
solid to liquid
solid to gas

A

condensation
deposition
freezing
vaporization
melting
sublimation

98
Q

boiling point

A

temperature at which equilibrium vapor pressure of the liquid equals the atmospheric pressure

99
Q

dynamic gas liquid equilibrium

A

opposing changes occur at equal rates in a closed system, rate of evaporation equals rate of condensation

100
Q

vapor pressure

A

pressure exerted by vapor in dynamic gas-liquid equilibrium with its corresponding liquid at a given temperature
more particles in the vapor phase causes a higher vapor pressure

101
Q

intermolecular forces of attraction relation with vapor pressure

A

stronger IMFA equals lesser vapor pressure

102
Q

volatile liquids

A

evaporate readily because of relatively weak intermolecular forces of attraction

103
Q

altitude’s relationship with pressure

A

higher altitude has lower atmospheric pressure

104
Q

at a substance’s melting point its particles

A

slide past each other

105
Q

aufbau principle

A

electrons are filled into atomic orbitals in the increasing order of orbital energy level.

106
Q

electron configuration notation

A

1s, 2s, 2p, 3s, 3p, 4s, 3d, 4p, 5s, 4d, 5p, 6s, 4f, 5d, 6p, 7s, 5f, 6d, 7p

107
Q

s, p, d, and f sublevels/oribtial in energy level hold _ _ _ _ electrons

A

2, 6, 10, 14

108
Q

formula for electrons is 2n²
sublevel n =

A

principle quantum number

109
Q

Bohr electron model is ___ rather than probablistic, which is the

A

deterministic
electron cloud model

110
Q

Atomic Emission Spectrum

A

an atom in the gas state emits light when energy is absorbed, pattern formed when light emitted by an element, unique to every element

111
Q

noble gas shorthand

A

shorthand including a noble gas as filler for first energy sublevels filled since noble gasses stable with octet, use noble gas preceding element notated

112
Q

polyatomic ion

A

pre-determined ionic compound, treated as an entity, and cannot be destroyed in most chemical reactions

113
Q

what sort of element written first in ionic compound

A

metal

114
Q

in ionic compounds the anion ends with the suffix

A

ide

115
Q

ionic bond

A

extremely stable electrostatic attraction holding oppositely charged ions

116
Q

ionic compound

A

ex. NaCl, Sodium Chloride
ionic bonds form between metal and nonmetal reacting to make electrically neutral compound made of cations and ions that balance charges

117
Q

electrolytes

A

ionic compounds dissolved in water that which makes aqueous solution conductive

118
Q

covalent bonding

A

only in non-metals when atoms share pairs of electrons

119
Q

metallic bonding

A

metals lose electrons to form positive ions and delocalised electrons, bond is strong electrostatic attractions between cations and delocalised electrons from valence shells of metal ions, array of positive metal ions surrounded by sea of electrons

120
Q

molecular solids have low melting point because

A

covalent bonds exist in the molecules but between them there is low imfas,

121
Q

molecular solids don’t conduct electricity because

A

the valence electrons are held tightly between the covalent bonds and the lone pairs of each molecule

122
Q

metallic solids are good conductors of heat and electricity because

A

of delocalised electrons,

123
Q

Avogadro’s Number

A

6.022x10^23, describes the number of particles or formula units in a mol of a pure sample of a substance

124
Q

chemical reaction

A

when a substance is transformed into a new substance, typically with a different composition. In this process heat, light, formation of a gas, formation of a precipitate, and/or a color change indicate that a chemical change has occured.

125
Q

chemical reactions can be categorized into five types

A

synthesis, decomposition, single replacement, double replacement, combustion

126
Q

catalyst

A

substance that increases the rate of a reaction by decreasing the activation energy but does not impact reaction pathway(effect) and total energy change

127
Q

precipitate

A

a solid as a result of two soluble ionic substances, implying also the differing levels of strength in hydration force and ionic bonding force

128
Q

Molar mass shows the __ per mole of a substance, determined by using atomic mass of an element measured in amus

A

of grams(mass),

129
Q

law of conservation of matter

A

matter is neither created nor destroyed

the number of atoms of an element in the Reactant ride equals the number of atoms of that element in the product side

130
Q

endothermic reaction absorbs energy because the energy released is ___ than the activation energy

A

less

131
Q

exothermic reaction absorbs energy because the energy released is ___ than the activation energy

A

more

132
Q

intramolecular forces of attraction

A

ionic and covalent - ionic is stronger

133
Q

intermolecular forces of attraction

A

hydrogen bonding(strongest), dipole-dipole, dispersion force(weakest)

134
Q

synthesis reaction

A

two elements or compounds form one product
ex. Na + Cl –> NaCl

135
Q

decomposition reaction

A

one reactant breaks down into two simpler substances

ex. H2O –> H2 + O

136
Q

Single replacement reaction

A

uncombined atom, ion, or element, replaces another in a compound

ex. Zn + 2HCl -> ZnCl2 + H2

137
Q

Double replacement reaction

A

two elements(positive ions) in reactants exchange places
ex. KBr + AgNO3 –> KNO3 + AgBr

138
Q

combustion reaction

A

carbon containing compound burns in oxygen from air to produce carbon dioxide, water, and heat or flames

CH4 + 2O2+ CO2 + 2H2O

Honors Chemistry (2 decks)

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