Chemistry Semester Exam Review I Name______
1) ______is any substance that has mass, volume (takes up space) and measurable properties.
2) Differentiate between solids, liquids, and gases: / solid / liquid / gasshape (yes/no)
fixed volume (yes/no)
flows (yes/no)
compressible (yes/no)
arrangement (orderly/random)
molecular proximity (closest, close, far apart)
molecular motion (slow, faster, fastest)
average kinetic energy (slow, faster, fastest)
intermolecular attraction (almost none, greater, greatest)
3) A substance in the plasma state has [less/ more] energy and is [slower/faster] than in the gas state.
4) Temperature is the measure of a substance’s average [kinetic/potential] energy that increases as its temperature [increases/decreases].
5) Physical property: ______
6) Chemical property: ______
7) Classify as physical (p) or chemical(c) property of a substance: melting point __, rusts __, color __,
reacts w/ acid __, boiling point __, density __, decomposes __, texture __, oxidizes __
8) Physical change: ______
9) Chemical change/chemical reaction: ______
10) ______- substances used up in the reaction; ______- substances made in the reaction
11) For the reaction: 2H2 + O2 à 2H2O, identify the reactant/s ______; product/s ______.
12) 6 signs a chemical change:______, ______, ______, ______,______, ______
13) Classify as physical (p) or chemical (c) change: burning __, dissolving __, rusting __, melting __, evaporating __, bleaching __, subliming __, baking __, decomposing __, boiling __, rotting __, cutting __
14) Indicate the state changes: solidàliquid ______; liquidàgas ______; solidàgas ______
gasàliquid ______; liquidàsolid ______; gasàsolid ______
15) The state changes that result from an increase in energy are ______,______,______
16) The state changes that result from a decrease in energy are ______,______,______
17) While a substance changes states its temperature [decreases/stays the same/increases].
18) Atomic Theory states that ______
19) What 2 principles of Dalton’s Atomic Theory changed? How?
i. ______
ii. ______
20) ______discovered electrons w/ the ______experiment. His ______model stated negatively charged e-s are embedded in positively charged matter/atom.
21) ______discovered the nucleus w/ the ______experiment. In his model, negatively charged e-s are scattered around the small, dense, positively charged ______that contains most of an atom’s mass.
22) ______’s Model- electrons can be only certain distances (energy levels) from the nucleus. *ladder rungs
23) ______Theory takes into account both particle and wave properties of electrons.
24) A/n ______(also ______) is a region where there is a high probability of finding electrons.
25) The number of protons and neutrons in the nucleus is ______number; ______number is the number of protons which identifies the element.
26) The modern periodic table is based on atomic ______. Mendeleev’s PT was based on atomic ______.
27) ______are atoms of the same element with different numbers of neutrons and different mass #s.
28) List the subatomic particles (p+, n0, e-) in order of increasing mass.____, _____, _____
29) A quantum is a discrete packet of ______; A photon is a packet of electromagnetic energy, or ____.
30) Complete subatomic particle structure charts: name______
subatomic particle / charge / Mass # / Mass / Location in the atom (nucleus, outside the nucleus)electron
proton
neutron
Hyphen notation / isotopic symbol / Mass# (p++n0) / Atomic # (p+) / p+ / n0 / e-
Copper-66
157N3-
20 / 22 / 18
31) ______:all frequencies(ν) or wavelengths(λ) of electromagnetic radiation.
32) Frequency(ν) + wavelength(λ) are ______related; if frequency(ν) increases, wavelength(λ) ______.
33) Show substitution and rearranged equation solving for the unknown variable.
c = νλ, c = 3.00x108m/s, c = speed of light in a vacuum, 1 hertz (Hz) = 1s or 1s-1
ex) Calculate wavelength(λ) of microwaves used to cook food with a frequency(ν) of 3.44x109Hz.
3.00x108m/s=(3.44x109Hz)λ à λ=(3.00x108m/s)÷(3.44x109Hz)= 8.72x10-2m
a) What’s the wavelength of violet light with frequency of 7.26x1014 Hz? ______=4.13x10-7m
b) What’s the frequency of light reflected from a green leaf with a wavelength of 4.90x10-7m?
______=6.12x1014Hz
34) Determine energy (in joules) of a photon w/ frequency of 3.55x1017Hz. Show substitution.
E=hν, E=energy, h(Planck’s constant) =6.626x10-34J·s
______=2.35x10-16J
35) Photoelectric effect: ______
36) Ground state: ______
37) ______: when an electron gained energy and has a higher potential energy than ground state.
38) Energy is not continuous, but exists in discrete amounts. Electrons must absorb/emit a specific quantum of energy to go from a lower energy state (more stable) to a higher one (less stable).
39) In dropping from a higher energy state to a lower energy state, an electron emits ______as ______.
40) ______: specific frequencies of light (spectrum of a few colors) emitted from elements (each element is unique) resulting when light passes through a prism and separates.
41) List the 4 quantum numbers, what they mean, and fill in the chart.
a) P______: ______
b) A______: ______
c) M______: ______
d) S______: ______
sublevel / shape / # orbitals or orientations about the nucleus / Max #e-s in sublevels
p
d
f
42) Pauli exclusion principle: ______
43) Aufbau principle:______
a) The energy levels in increasing order: 1s2, ___ , ___ , ___ , ___ , ___ , ___ , ___ , ___ , ___ , ___ , 6s2
44) Hund’s rule: ______
45) Electron configuration (superscripts) for Ni: ______
a) How many electrons are in Nickel’s electron configuration? ___
46) Orbital (¯) notation for O: ______a) # of electrons in O configuration? __
47) Which element has an electron configuration that ends with 3p2? ___; ends with 5s2? ___; 4d9?____
Chemistry Semester Exam Review II Name______
48) What element has a noble gas configuration of [Kr]5s24d105p1? ___; [Xe]6s2?___; [Ar]4s23d7?___
49) Noble gas configuration of exceptions *[Ar]4s13d10? ___; *[Ar]4s13d5?____
50) How many electrons are required to fill the 1st energy level (period)? __; 2ndenergy level?__;4th?___
51) ______ electrons are electrons in the s and p orbitals of the outermost energy level.
52) When an atom has a full outer energy level of 8 electrons it is [less/more] stable than when it doesn’t.
53) Elements in the same ______, column, have the same number of valence electrons w similar physical and chemical properties and therefore, ______similarly.
54) Elements in the same ______, row, have the same principle quantum number, thus have the same number of occupied ______.
55) How many unfilled orbitals are in the following atoms: N______; O______; K______; F______
56) Most elements on the periodic table are [solid/liquid/gas/plasma].
57) What element is in period 4, group 2? __; group 15, period 3? __; P 2, G 18?__; G4 P5? __
58) Identify each group of the Periodic Table and give 1 characteristics of each:
A) ______;______
B) ______;______
C) ______;______
D) ______;______
E) ______;______
F) ______;______
G) ______;______
H) ______;______
I) ______;______
J) ______;______
59) Underline + state how many significant figures: (leading zeroes aren’t significant, trailing are w decimal)
a) 10000 / b) 1.000 / c) 0.0100 / d) 0.0110 / e) 1.000x104 / f) 1x10-6g) 1.0000 / h) 0.0001 / i) 10.100 / j) 110 / k) 1.0x1023 / l) 1.00x105
60) Sig figs Show unrounded answer and rounded answer to correct # of sig figs.
(Adding and subtracting): Round answer to least precise place in given numbers.
ie) 5.4m-2.13m=3.27mà3.3m; 100g+1g=101gà100g
a) 1.1+5.437+9.95=______=______
b) 4.78+3.218+5.82=______=______
c) 9.99-6.6=______=______
d) 100-11=______=______
(Multiplying and dividing): Round answer to least significant digits in given numbers.
ie) 2.4(15.8)=37.92à38; 16.8/5.8=2.896à2.9; 102.4/51.2=2à2.00
a) 6.2 x 13.0=______=______
b) 15.00/3.00=______=______
c) 38,736/478=______=______
d) 55x100=______=______
Multi-step. Show intermediate step, unrounded answer, and final answer rounded to correct # of sig figs.
ie) (2.35g+15.6g)/0.03591mL=17.95g/0.03591mL=499.86...g/mLà500.g/mL
a) (3.5x21.3)-71.5=______=______=______
b) 23.91/(43.6+14.15)= ______=______=______
c) (35.65-117.8)8.494=______=______=______
d) 26(15.00-14.90)= ______=______=______
61) ºC↔K (ºC+273=K) Show work. Round answer to least precise place in given numbers.
a) 34.0ºC+273=307K / b) 273.0ºC / c) 22.5ºCd) 546K-273=273ºC / e) 0.0 K / f) 1277.3K
62) Round ↓ to 1 sig figs Round ↓ to 2 sig fig Round ↓ to 3 sig figs Round ↓ to 4 sig figs
a) 0.03425à0.03 / b) 0.03452à0.035 / c) 34.567à34.6 / d) 912678à912700e) 678912à / f) 1.0234à / g) 678912à / h) 1099.9à
i) 9.29x105à / j) 354.673à / k) 0.09595à / l) 1.02345à
Name______
63) scientific notation↔standard notation ex)1000↔1x103; 0.001↔1x10-3
a) 0.000765= / b) 6190.00 = / c) 9000=d) 6.0x10-2= / e) 3.98x10-3= / f) 2.500x10-4=
64) Molar conversions: Show all work, unit and substance on every number, sigfigs.
1 mole=6.022x1023atoms; 1 mole = atomic mass (g) from PT rounded to 2 places after decimal.
a) 17.0mol of xenonà atoms 1.02x1025b) 4.020x1025formula units CuSO4à moles 66.76
c) 1.002mol of chlorineàgrams 35.52
d) 0.039g of carbonà moles 0.0032
e) 4.22g sulfur dioxide, SO2àmolecules 3.97x1022
f) 8.22 x 1023 atoms of cesium àgrams 181
65) Density (D=m/v): Show substitution, work, intermediate answer, final answer to correct # of sig figs.
a) What is the mass of 100.0cm3 of gold if the density is 19.32 g/cm3? 1932b) What is the volume of mercury with a density of 13.55g/mL and a mass of 120.0g?8.856
c) What substance has a mass of 55g and occupies 6.14cm3? Fe=7.87g/cm3, Cu=8.96g/cm3, Pb=11.36g/cm3
66) In an experiment, a/n ______variable (cause) is a variable that is varied or manipulated, a/n ______variable (effect) is the response that is measured, and a/n ______is a constant variable.
67) In an experiment designed to test “How does concentration effect reaction rates?“ independent variable ______dependent variable ______control ______.
68) Metric conversions: List from shortest (1) to longest (6), (*convert all to m)
Show work; use dimensional analysis, units, sig figs.
1000m=1km / 100m=1hm / 10m=1dam / 1m=10dm / 1m=100cm / 1m=1000mm / 1m=1x106µma) 0.100km x ______=
( ) / b) 10mm x ______=
( )
c) 1x107µm x ______=
( ) / d) 0.010hm x ______=
( )
e) 10cm x ______=
( ) / f) 0.010dm x ______=
( )
Chemistry Semester Exam Review III Name______
69) Ion formed (symbol+charge):barium____;aluminum____;iodine___;nitrogen___;cesium____;sulfur___
70) Name transition metal ion:Fe3+______Co2+______;Sn4+_____;Cu1+______Cr3+______
71) Name transition metal ion:V2O7______;MnO______;AuPO4______;PbI2______
72) Determine the number of valence electrons for: Kr=__; Mg=__; P=__; B=__; K=__; I=_; C=_; S=_; He=_
73) Identify each compound as Ionic (I), Covalent(C), or Acid(A) and give the name or formula:
Type / Formula / Name / Type / Formula / Namea) / I / CaCO3 / b) / nitrogen triiodide
c) / H2SO4 / d) / aluminum chloride
e) / P4H7 / f) / hydrobromic acid
g) / Na2S / h) / vanadium (V) oxide
i) / Cr2(SO4)3 / j) / strontium phosphide
k) / S2F5 / l) / manganese (II) phosphate
m) / HCl / n) / hexacarbon decahydride
o) / SnS2 / p) / phosphorous acid
74) A/n ______bond forms between two nonmetals; a/n ______bond forms between a metal and a nonmetal.
75) Circle the pair most likely to form an ionic bond: C-N, O-F, Na-Cl, S-I
76) Circle the pair most likely to form a covalent bond: Ca-Br, S-O, Li-N, Cu-O
77) What type of bond do the following have in common: AlF3, MgO, KCl, FeSO4? [Ionic/ covalent] bond.
78) What type of bond do the following have in common: CCl4, H2O, N2O2, P2Cl4? [Ionic/ covalent] bond.
79) How do atoms form a bond? Covalent bonds-2 nuclei mutually attract and ______electrons. Ionic bonds ______electrons to produce ions and electrostatic opposites ______one another.
80) All compounds are [positively charged/negatively charged/neutral].
81) Atoms bond to obtain a stable ______, full (8 e-s) outer energy level.
82) The ions Br- and Sr+2 both formed a ______octet like __’s outer electron configuration.
83) When an atom has a full valence shell it is stable like the ______.
84) ______rule-tendency for atoms to lose, gain, or share e-s to have a full outer shell of 8 valence e-s. *Exceptions: H can bond to have only _ electrons in its outer energy level; B can bond to only have _ e-s.
85) Draw Lewis Dot structure, indicate shape and polarity [Polar or NP(nonpolar)] for following:
CH4tetrahedral/NP / BCl3 / NH3 / H2O / Cl2
86) Intermolecular forces are ______.
87) As a substance changes state, the temperature [increases/stays the same/decrease], b/c added energy is used to overcome ______as opposed to increasing average kinetic energy.
88) As temperature increases, average kinetic energy ______.
89) The greater the attraction between molecules the [lower/higher] the melting and boiling points.
90) Strength of intermolecular forces [increase/decrease] when molecules are farther apart.
91) ______-______forces- interactions b/t polar molecules. Positive end of 1 molecule is attracted to negative end of another molecule
92) ______- special dipole-dipole force between small H bonded to a highly electronegative atom
93) Hydrogen bonding occurs between Hydrogen and ______, ______, or ______.
94) ______forces are weak dipole forces resulting from temporary uneven e- distribution.
95) London Dispersion (also van der Waals) forces are [stronger/weaker] between more massive molecules. This is why Br2 is a [liquid/solid] at room temperature while I2 is a [liquid/solid] @ room T.
96) Number#(1-5) the following in order of increasing strength (weakest to strongest):
__ Covalent bond; __Dipole-dipole; __ Hydrogen bonding; __ Ionic; __ London Dispersion;
97) Which intermolecular force is responsible for water’s unique properties? ______
98) ______- liquid’s attraction to solid surfaces; ______- liquid’s attraction to other liquid particles.
99) The combination of adhesion and cohesion forces acting together to allow water to flow up a thin tube without an external force is ______. ______is the tendency of liquids to decrease surface area to smallest size possible forming droplets.
100) On the surface of a liquid, particles with the highest ______will evaporate first.
101) A(n) ______is a pure substance that is made of only one kind of atom. The symbol for a(n) ______is always one or two letters. When the symbol contains two letters, the first letter is always ______, and the second letter is always ______.
102) A(n) ______is a pure substance containing two or more elements that are ______combined. A(n) ______is represented by a chemical ______. The elements in a(n) ______always combine in ______proportions.
103) A(n) ______is made of two or more substances that are ______combined. A(n) ______that is uniformly mixed is called ______. A special name for this is a(n) ______. A(n) ______that is not uniformly mixed is called ______. A special type of mixture that is a solid ______of two or more metals is called a(n) ______.