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Chem Quiz #1 > Chem Quiz #1 > Flashcards

Chem Quiz #1 Flashcards

1
Q

Define element

A

a type of matter composed of atoms w/ the same atomic # (substance can only correspond to 1 element on periodic table)

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2
Q

Allotrope

A

Diff. STRUCTURAL forms of the same element in the same phase
- diff. forms can have diff. reactivity

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3
Q

Examples of allotropes

A

Carbon: Diamond, graphite, & fullerenes
Oxygen: dioxygen (O2) & Ozone (O3)
Sulfur: orthorhombic, monoclinic, amorphous (30 others)
Phosphorus: red, white, & black

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4
Q

Photocatalytic water splitting

A

Uses sunlight to split H20, butt electrolysis energy doesn’t compensate for energy spent

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5
Q

Compound

A

substance that contains 2 or more elements

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6
Q

Binary compound

A

Contains 2 elements

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7
Q

Binary compound examples

A

H20, H202, CO, & CO2

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8
Q

Ternary compound

A

Contains 3 elements

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9
Q

Ternary compound examples

A

C2H5OH (ethanol)

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10
Q

Quaternary compound

A

Contains 4 elements

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11
Q

Polymorphs

A

Diff. structural forms of the same COMPOUND in the same phase

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12
Q

Polymorph examples

A

TiO2 (Anatase & Kutile)

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13
Q

Organic compound made w/

A

Carbon, Hydrogen, Oxygen, & sometimes Nitrogen

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14
Q

Prussian Blue

A

absorbs thallium & is treatment for radioactive exposure
Fe4[Fe(CN)6]3

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15
Q

Mixtures

A

Combination of 2 or more elements/compounds

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16
Q

Example of a mixture

A

Salt Water (NaCl + H20), Brass (Cu + Zn)

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17
Q

Heterogeneous

A

Can be physically separated (not uniform)

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18
Q

Heterogenous ex.

A

solid mixture of blue Cu(NO3)2 x 6H20 & yellow Cds
or
Cereal

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19
Q

Homogeneous

A

mixed @ molecular level butt NOT chemically bonded
- properties don’t vary through the sample
- can be separated butt not easily

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20
Q

Homogeneous ex.

A

NaCl + Water or air

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21
Q

Pure Substance

A

only an element or compound

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22
Q

Material

A

sample of unknown composition & may be a pure substance/mixture

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23
Q

Greek root of atom

A

atom (not) tomos (cut)

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24
Q

1st evidence for existence of atoms

A

analyzing weights of products & reactants

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25
Q

Law of Conservation of Mass

A

Mass is neither created nor destroyed in a chemical reaction

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26
Q

Law of Definite Proportions

A

In a pure compound, the constituent elements are always present in a set proportion or % by mass

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27
Q

Law of Constant Composition

A

All samples of a given chemical compound have the same elemental composition
- H20 is always 11.1% H & 88.9% no matter the source or method or prep
- lead sulfite is always lead sulfite…adding more just leaves leftover unreacted material

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28
Q

Dalton’s 5 Theories of Matter

A
  1. Elements consist of tiny indivisible particles called atoms (divisible by ionization
  2. All atoms of a given element are identical in mass & other properties
  3. Diff. elements have diff. atom kinds which have diff. masses
  4. Compounds are formed when atoms of unlike elements combine in small whole # ratios
  5. Atoms retain their identities in a chemical process & a chem. reaction just changes the atoms bonding
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29
Q

How are atoms divisible

A

Ionization & nuclear reactions

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30
Q

Law of Multiple Proportions

A

When 2 elements form a series of compounds, the masses of 1 element that combine w/ a fixed mass of the other element are in the ratio of small integers to each other

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31
Q

Law of Combining Gas Volumes

A

When gases (@ same pressure & temp.) react, they do so in a definite integer ration by volume. Volume of either reacting gas is the ratio of simple integers

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32
Q

Avogadro’s Hypothesis

A

Equal volumes of diff. gases @ same temp. & pressure contain equal # of particles. THe distances between the particles are very large, compared w/ the size of the particles

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33
Q

Avogadro’s Hypothesis ex.

A

1 L of hydrogen gas has the same # of particles as 1 L of oxygen gas or 1 : of nitrogen gas or 1 L of hydrogen chloride

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34
Q

Explain Avogadro vs Dalton beliefs

A

Dalton: believed particles of an elemental gas consisted of atoms
Avo: believed of an element gas could be atoms, diatomic, or polyatomic & could explain law of combining volumes

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35
Q

Cannizzaro findings

A

Calculated molecular mass of gaseous compounds & obtained a self-consistent set of relative atomic & molecular masses (accepted that these are diatomic molecules)
ex. if H2 is assigned a mass of 2, O2 is assigned a mass of 32 w/ a 16:1 Oxygen to Hydrogen ratio

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36
Q

Cannizzaro beliefs

A
  1. Molecules contain whole #’s of atoms
  2. Avogadro’s hypothesis is correct & equal volumes of gases under the same condition contain the same # of molecules (masses of equal volumes of gasses are proportional to the relative masses of the particles (atoms/molecules)
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37
Q

Relative molecular mass using Avo.’s hypothesis ex.

A

ratio of masses of equal volumes of oxygen & hydrogen is 16:1

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38
Q

Cannizzaro accepted

A
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39
Q

How to determine relative molecular masses of elements that aren’t gasses

A

study gaseous compounds of those elements

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40
Q

Physical structure of atoms

A

composed of + charged nucleus (protons & neutrons) and - electrons

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41
Q

facts abt protons

A

charge of P+ & e- are exactly the same
proton mass = neutron mass
proton mass = 1836 x electron

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42
Q

Evidence for electrons

A

Cathode/Beta rays

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43
Q

Cathode/Beta Rays

A

stream of electrons that could be deflected by magnetic & electric fields

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44
Q

OG name for electrons

A

corpuscles

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45
Q

charge to mass ratio of an electron

A

e/Me = -1.76x10^8 C/g

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46
Q

Millikan’s Oil Drop Project

A

observed (-) charged oil drops could be kept from falling by charging electric plates and using an instrument that measures the charge of the drop

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47
Q

e- charge

A

1.59x10^-19 C

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48
Q

e- mass

A

Me = 9.11 x 10^-31 kg

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49
Q

Plum Pudding Model

A

thot (+) charge spread thru entire atom & expected heavy alpha particles would pass through the thin gold foil

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50
Q

Plum Pudding Debunked!?

A

Most alpha particles passed straight through, but some deflected at a large angle…rutherford concluded most of the mass was concentrated in a very small & dense (+) charged particles

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51
Q

Rutherford Model

A

nucleus posses net charge of +Ze, w/ Z electrons surrounding the nucleus

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52
Q

Particles w/ thier mass & charge
e-
p+
N

A

Charge & Mass:
e- = (1-) = 9.11 x 10^-31 kg
p+ = (1+) = 1.67 x 10^-27 kg
N = (None) = 1.67x10-27 kg

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53
Q

Atom structure

A

tiny nucleus surrounded by electron cloud (without neutrons, protons wouldn’t stick together)

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54
Q

baseball size nucleus = _____ diameter
pea size nucleus weighs _______ tons

A

4 km
250 million tons

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55
Q

Harold Clayton Ureg discovery, where, & how?

A

deutrium & won noble prize for it, found in HAVEMEYER, 5L liquid hydrogen distilled to 1mL using distillation apparatus (went from 1st to 2nd floor) then let evaporated liquid condense at room temp. then measured spectrum of light emitted by passing a high xxx
- also lead isotope separation studies

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56
Q

Nuclide characterized by

A

p+ (Z) or atomic #
# neutrons (N)
mass # (Z + N = A) or (# prontons + # neutrons)

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57
Q

Isotopes

A

Nuclides of same elements w/ diff. mass #’s (A)
- also means “same place”
- introduced by F. Soddy to explain observations on radioactivity

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58
Q

Isotopes of Hydrogen

A

protium: 1 p+ & 0 neutrons (99.985%)
deuterium: 1 p+ & 1 neutron (0.015%)
tritium: 1 p+ & 2 neutrons (radioactive w/ 1/2 life of 12.3 years)

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59
Q

Isotopes of Carbon

A

C12: 6 p+ & 6 neutrons (98.89%)
C13: 6 p+ & 7 neutrons (1.11%)
C14: 6 p+ & 8 neutrons (radioactive w/ half-life of 5,730 years)

60
Q

Meaning of subscripts in a chemical formula

A

relative number of atoms present

61
Q

Chemical Bonds

A

how atoms are connected together (very from compound to compound)

62
Q

Covalent Bonding

A

sharing of elements to hold atoms in molecules together

63
Q

“flat drawing”

A

indicates connectivity

64
Q

in a perspective drawing
solid line =
dashed line =
wedged line =

A

solid line = bonds in the plane
dashed line = atom connected to central atom behind the plane
wedged line = atom connected to central atom is in front of the plane

65
Q

Ionic Bonding

A

electrons are completely transferred from one atom to another, resulting in formation of charged atoms (ions)

66
Q

How does Ionic bonding work?

A

attraction between cations (+ ions) & anions (- ions)

67
Q

Isotropic

A

finds anything around them that isn’t oppositely charged

68
Q

Non-directional bonds

A

Ionic…allows ionic solids (salts)

69
Q

Periodic table

A

links together families of elements that have similar chemical or physical properties
- chemical & physical properties of the elements are periodic functions of the atomic # (# p+ = # e- in the neutral atoms…the later determines the chemistry)

70
Q

Q: Why does carbon combine w/ 4 atoms of hydrogen to form CH4, wheras oxygen combines w/ only 2 atoms of hydrogen to form H20?
Q: Why does helium exist as atoms (He), wheras hydrogen exists as diatomic molecules?

A

A: concerned w/ electronic structures of the individual atoms & these are dictated by the positions of the elements in the periodic table

71
Q

8 groups of main group elements

A
  1. Alkali metals: (H). Li, Na, K, Rb, Cs
  2. Alkaline earth metals: Be, Mg, Ca, Sr, Ba, Ra
  3. Boron family (teriels): B, Al, Ga, In, Tl
  4. Carbon family (tetrels): C, Si, Ge, Sn, Pb
  5. Nitrogen group (pnictogens): N, P, As, Sb, Bi
  6. Chaliogens: O, S, Se, Te, Po
  7. Halogens: F, Cl, Br, I, At
  8. Noble gasses: He, Ne, Ar, Kr, Xe, Rn
72
Q

Alkali Metals

A

H, Li, Na, K, Rb, Cs

73
Q

Alkaline Earth Metals

A

Be, Mg, Ca, Sr, Ba, Ra

74
Q

Boron family (teriels)

A

B, Al, Ga, In, Tl

75
Q

Carbon family (tetrels)

A

C, Si, Ge, Sn, Pb

76
Q

Nitrogen group (pnictogens)

A

N, P, As, Sb, Bi

77
Q

Chaliogens

A

O, S, Se, Te, Po

78
Q

Halogens

A

F, Cl, Br, I, At

79
Q

Tin & lead are metals butt react similar too ___________

A

Silicn

80
Q

Mendeleev Periodic Table organization

A

Chemical & physical properties of the elements are periodic functions of their atomic masses

81
Q

Bottom rows of elements

A

Lanthanides & Actinides

82
Q

Do actinides occur naturally or artificially?

A

Mostly artificially, butt thorium & uranium have a reasonable natural occurrence

83
Q

1-18 numbers on periodic table

A

1-9 indicate # of valence electrons and once in double digits, the 2nd number indicates the # of valence electrons

84
Q

Core e-

A

aren’t normally available for bond forming
- exception is group 11 (Cu, Ag, & Au which may have valence of 1, 2, or 3)

85
Q

Characteristics of Metals

A
  • Metallic luster (shine)
  • Good conductor of heat & electricity
  • Malleable (hammered into sheets)
  • Ductile (drawn into wire)
86
Q

Characteristics of Non-metals

A
  • dull color
  • poor conductor of heat & electricity
  • brittle
87
Q

Semimetals/metalloids

A

have characteristics that resemble metals in some regards & nonmetals in others (form a zigzag line of division)

88
Q

metalic or nonmetalic
left side periodic table =
right of periodic table =

A

left = metalic
right = non metalic

89
Q

lighter element examples =
heavier elements examples =

A

N2, O2, Fe
Bi, Te, I2

90
Q

Most abundant element in the universe

A

Hydrogen

91
Q

Lightest element

A

Hydrogen

92
Q

2nd lightest element that doesn’t burn

A

Helium

93
Q

2nd most abundant element in the universe

A

Helium

94
Q

Element used in cryogenics & MRI

A

Helium

95
Q

Combine w/ water to give alkaline solutions

A

Alkali Metals (G1)

96
Q

Soft metals that can be cut w/ a knife

A

Alkali Metals (G1)

97
Q

Malleable & ductile metal (ex. sodium wire)

A

Alkali Metals (G1)

98
Q

Highly reactive metals towards water liberating H2 that ignites of explodes

A

Alkali Metals (G1)

99
Q

Alkali metal compounds

A

form compounds w/ M+ ions (ex. NaCl)
- Na burns in Cl2

100
Q

Meaning of “Earth” in Alkali Earth Metals

A

substances that are insoluble in water & stable to heat (originally referred to oxides of these elements)

101
Q

Harder than Alkali metals

A

Alkali earth metals

102
Q

Alkaline Earth Metal Info

A
  • less reactive than alkali metals
  • usually forms compounds that features M2+ ions + 2e-
103
Q

Organic Chemistry

A

Chemistry of carbon (will bond w/ all sorts of elements & structure)

104
Q

Meaning of carbon existing allotropy

A

existence of 2+ structural forms of an elements in the same states
ex. diamond, graphite, fullereness

105
Q

Group that transition from non-metalic (C) to semimetalic (Si, Ge) to metalic (Sn, Pb) character

A

Carbon group

106
Q

Fullerenes

A

C60 is a soccer ball made of hexagons & pentagons

107
Q

Diamond info

A
  • hardest known naturally occurring substance
  • only made under high temp. & pressure where its thermodynamilly more stable
108
Q

Is diamond or graphite more stable @ room temp & pressure?

A

Diamond is thermodynamically unstable w/ respect to graphite, but is kinetically stable

109
Q

Carbon Nanotubule

A

Different roles influence electric conductivity

110
Q

Graphite

A

flakes easily but more stable then diamond

111
Q

Endohedral Fullerenes

A

Most expensive material in the wrld $167,000,000/g

112
Q

Silicon for Electric Industry

A

Singte, pure, silicon crystals (cut into wafers & used in computers)

113
Q

Carbon Group Compounds

A

Form tetravalent compounds of composition MX4, but tin & lead also form divalent 1:2 compounds (the inert pair effect)

114
Q

2 coordinate divalent

A

stable for tin & lead butt highly reactive speicies for carbon

115
Q

Petroleum Fuels

A

hydrocarbon
ex. octane

116
Q

Carbon Dioxide

A
  • formed when something burns or we breathe
  • responsible for “greenhouse effect”
  • increasing levels makes rivers, lakes, & oceans acidic & kill certain plants & animals
117
Q

Dry Ice

A

goes from solid to gas (sublimation)(made of CO2)

118
Q

Nitrogen

A
  • main component of air (80%) & oxygen is (20%)
  • gas but becomes a liquid @ very low temperatures
  • used in MRIs & coding
119
Q

Nitrogen compounds

A
  • ammonia & nitric acid are 2 of the most nitrogen compounds made on a massive scale
  • nitric acid used for dyes, drugs, fertilizers, & explosives
120
Q

Phosphorus

A
  • matches are a mix of red phosphorus & potassium chloride
  • lots of allotropes
120
Q

Bismuth

A

true structure isn’t known & is in pepto bismol

121
Q

Chalcogen meaning

A

ore former (ex. metal oxides & sulfides)

122
Q

Chalcogens

A
  • transition from nonmetallic (O, S, Se) to semimetallic (Te, Po)
  • Po is reactive and little studied
123
Q

Combustion of metals in O2

A
  • metlass react w/ O2 to form oxides
  • iron reacts slowly w/ O2 in the presence of water @ room temp. to give rust & oxide-hydroxides
  • iron burns readily in O2 to give ultimately Fe2O3
124
Q

Water

A
  • burn hydrogen & oxygen
  • in one molecule of water, 3 atoms are bonded together
125
Q

H2O & H2O2 is an example of

A

Law of Multiple Proportions

126
Q

Hydrogen Peroxide

A
  • 2 atoms of hydrogen & 2 atoms of oxygen
  • unstable & decomposses to water & oxygen
  • often used as bleach
127
Q

Halogens Greek

A

Halos = salt
Genes = forming

128
Q

Group that only exists as diatomic molecules & are nonmetals

A

Halogens (F, Cl, Br, I, At)

129
Q

Melting point on periodic table

A

Increases further right you go

130
Q

Inert/Noble Gasses

A

He, Ne, Ar, Kr, Xe, Rn

131
Q

Group where compounds exist in a monoatomic form relative to a certian degree

A

Inter/Noble Gases

132
Q

1st noble gas compound

A

Xe + PtF6

133
Q

Mass Spectrometer

A

measures atomic & molecular mass

134
Q

How Spectrometer works?

A
  1. Ionizing sample w/ e- bombardment (removing or adding e-)
  2. Accelerating ions thru a magnetic field
  3. Measuring amount of deflation (depends on mass/charge ratio)
    - smallest ions on top & biggest on bottom of detector plate
135
Q

Atomic Masses

A

mass of individual atom or deflected more
- reported relative to mass of C12 being defined as 12 atomic mass units

136
Q

C12 weight

A

12.01 amu

137
Q

How does carbon naturally exist?

A

mixture of isotopes C12 & C13

138
Q

Ratios of Reactants

A

2 bread slices + 1 cheese = cheese sandwich
soooo 2H2 + O2 –> 2H2O (2 molecules of H2 react w/ 1 molecules of O2 to give 2 molecules of H20)
- use atomic mass to calc. ratio

139
Q

Avagadro’s Number

A

of atoms in 12g of C12
6.022x10^23
universal constant

140
Q

Mole

A

unit that corresponds to Avogadro’s # of particles

141
Q

Na x volume of 1 molecule =

A

volume occupied by molecular mass in grams

142
Q

How is volume of 1 molecule determined?

A

X-Ray

143
Q

How is molecular mass in grams determined?

A

Density

144
Q

mass (g) of any element is numerically equal to

A

relative atomic mass of that element

145
Q
A

Chem Quiz #1 (5 decks)

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