exam 1(1-3)
Nb
41 atomic #, Niobium, 92.9064 atomic mass, group 5 Transition Metal
Which of the following are chemical properties of matter?
Flammability
What element has the symbol F?
Flourine
4.16x10^3+2.58x102/5.377x104
0.0822
How many neutrons are in a ⁴He atom?
2
convert 2.30 hours to second
2.30 hr x 60.min/1hrx60.0s/1min=8280s
Which quantum state (n,ℓ,mℓ) is NOT possible?
3,0,1
The halogens are found in Group ___
7A (17)
The following picture would be best described as
A liquid compound
Which of the following is a physical change
An apple is cut into quarters
The element symbol for arsenic is
As
Which of the following is an ionic compound?
CaO
What element is designated by the orbital diagram below?
F
All of the following pairs of ions are isoelectronic except which one?
Fe²⁺ and Mn³⁺
Because electron energy levels are quantized, which of the following is true? I) Atomic emission spectra are a series of discrete lines. II) Atomic emission spectra are continuous. III) Electrons may only occupy a discrete set of energy levels. IV) Electrons may occupy a continuous range of energy levels.
I) Atomic emission spectra are a series of discrete lines III) Electrons may only occupy a discrete set of energy levels.
What type of bonding is present in SrCl2
Ionic bonds only
The element symbol for potassium is _____
K
What is the noble gas core in the electron configuration for Ru?
Kr
Which of the following is an extensive physical property of matter?
Length
Which of the following states of matter is pictured below?
Liquid
You have a 100 gram sample of each of the following metals. Which sample has the largest volume?
Magnesium, d= 1.74 g/cm3 (FEEDBACK: 100gx 1cm3/1.74g=57.5cm3
The law of conservation of mass is best described as which of the following statements?
Matter can neither be created nor destroyed.
Which of the following groups of elements tend to form cations?
Metals
Which of the following is most likely to form a +2 ion?
Mg
Which of the following is best classified as a covalent compound?
N2O5
Which of the following series of isoelectronic ions (Mg²⁺, N³⁻, F⁻, Si⁴⁺) has the ionic radii in order of largest to smallest?
N³⁻ > F⁻ > Mg²⁺ > Si⁴⁺
Which of the following states that no two electrons can have the same set of four quantum numbers?
Pauli exclusion principle
Which of the following is NOT a metalloid?
Pb
Rank the following atoms in order of increasing first ionization energies (i.e., lowest to highest): Rb, F, Mg, B, N.
Rb < Mg < B < N < F
Rank the following atoms in order of decreasing size (i.e., largest to smallest): Rb, F, Mg, B, N.
Rb > Mg > B > N > F
What element with a mass number of 100 has 56 neutrons in its nucleus?
Ruthenium (RU) (FEEDBACK: step1 100=x+56 step 2 44=x
What is the empirical formula of a molecule containing four sulfur atoms and four fluorine atoms?
SF
The element symbol for tin is _____
Sn
A homogeneous mixture is also called a ____________.
Solution
Which of the following elements would be chemically similar to calcium (Ca)?
Sr
Which of the following metals would be expected to have the smallest atomic radius?
Tantalum (Ta)
If a hydrogen (H) atom and a helium (He) atom travel at the same speed, which of the following is true about the de Broglie wavelengths of the atoms?
The H atom is about 4 times longer than the He atom.
The Millikan oil drop experiment determined
The charge of the electron
The cathode ray tube experiment determined:
The existence of electrons
In the photoelectric effect, if the intensity of light shone on a metal increases, what will happen?
There will be more electrons ejected
Ignoring the sign, which has a greater magnitude of charge?
They have equal charges
Which of these statements is true concerning the following reaction? Na(g) → Na⁺(g) + e⁻.
This is an ionization process.
Which element is classified as a transition metal?
Zirconium (Zr)
Which of the following is best classified as an ionic compound?
ZnS
If light has a lot of energy, it will have:
a small wavelength
Based on the positions of the following elements on the periodic table, which of them would you expect to form a 3+ cation?
both A scandium and B aluminum
The symbol Cr represents the element ____
chromium
What happens to the energy of a photon if the wavelength is doubled?
energy is reduced by one-half
What type of light on the electromagnetic spectrum has the highest energy per photon?
gramma waves
Which of the following is NOT a rare earth (lanthanide) element?
protactinium
Kelvin is the SI unit for which physical quantity?
temperature (FEEDBACK: c=K-273.15)
What does the mass number of an atom represent?
the total number of protons and neutrons in the atom
True or false: two electrons can simultaneously occupy the same (n,ℓ,mℓ) orbital.
true
Which of the following would be an isotope of ¹⁴N?
¹⁶N
An unknown element X has the following isotopes: ²⁵X (80.50% abundant, mass = 25.03 amu) and ²⁷X (19.50% abundant, mass = 26.98 amu). What is the average atomic mass of X in amu?
(0.8050 x25.03) + (0.1950 x 26.98) step2: (20.15)+(5.261)=25.41amu
An unknown element X has the following isotopes: ⁵²X (89.00% abundant), ⁴⁹X (8.00% abundant), ⁵⁰X (3.00% abundant). What is the average atomic mass in amu of X?
(0.8900 x52) + (0.0800 x49) + (0.0300 x50) = 51.7 52amu
Determine the molar mass of C₂H₇N. Provide an answer to two decimal places.
(2x12.01g) + (7x1.01g) + 14.01g=45.10g
Determine the molar mass of Ca(OH)₂. Provide an answer to two decimal places.
(40.08g/mol) + (6;00g/mol x2) (1.01g/molx2) = 74.1 g/mol
You measured the mass of a dry powder on a balance to be 23.76 g. What would you report as the uncertainty of this measurement?
+-0.01
A race car has maximum speed of 0.104 km/s what is this speed in miles per hour
0.104 km/sx60s/1minx60min/1hrx0.6214mi/1km=233mi/hr
A chemist encounters an unknown metal. They drop the metal into a graduated cylinder containing water, and find the volume change is 4.1 mL. If the metal weighs 3.5 g, what is the density of the metal in g/mL?
0.85 g/mL (FEEDBACK: d=3.5g/4.1mL)
If n = 2, what is the maximum allowed value for ℓ?
1
What is the maximum number of electrons that can have the following set of quantum numbers? n = 4, ℓ = 3, mℓ = 3, ms = -½
1
H
1 atomic #, Hydrogen, 1.008 atomic mass, group 1 Alkali metal
Atoms formula
1 mole = 6.022x1023
A solution is made by dissolving 8 grams of a salt in 100 cm³ of water (density = 1 g/cm³). Assuming the volume does not change, what is the density of the solution?
1.08 g/cm3 (FEEDBACK: 8g+100g/100cm3)
How many atoms of vanadium are in 1.28 grams of vanadium
1.28gVx 1molV/50.94gV x6.022x1023 atoms V/1 molV= 1.51x1022 atoms V
determine the mass in grams of 1.6x10-3 mol glucose C6H12O6
1.6x10-3 mol C6H12O6x 180.18 gC6H12O6/1C6H12O6= 0.29g C6H12O6
How many electrons can be assigned to orbitals designated by the quantum numbers n = 3, ℓ = 2?
10
In a ground state atom of Kr how many electrons total will have the quantum number ℓ = 2?
10
Ne
10 atomic #, neon, 20.1797 atomic mass, group 18 noble gases
You were given a dose of 500 mg rather than 500 μg of a drug. How much more of the drug did you receive?
1000 time more (FEEDBACK: 500mg x 1000ug/1mg=500000ug/ 500ug=1,000 times)
Rf
104 atomic #, Rutherfordium, 261 atomic mass, group 4 Transition Metal
Db
105 atomic #, Dubnium, 262 atomic mass, group 5 Transition Metal
Sg
106 atomic #, Seaborgium, 266 atomic mass, group 6 Transition Metal
Bh
107 atomic #, Bohrium, 264 atomic mass, group 7 Transition Metal
Hs
108 atomic #, Hassium, 277 atomic mass group 8 Transition Metal
Mt
109 atomic #, Meeitnerium, 268 atomic mass, group 8 Transition Metal
Na
11 atomic #, Sodium, 22.9898 atomic mass, group 1 Alkali metal
Ds
110 atomic #, Darmstadtium, 281 atomic mass, group 10 Transition Metal
Rg
111 atomic #, Roentgenium, 272 atomic mass, group 11 Transition Metal
Cn
112 atomic #, Copernicium atomic mass, group 12 Transition Metal
What is the atomic symbol and mass number for an atom containing 50 protons and 64 neutrons?
114Sn (FEEDBACK:50 +64=114)
Mg
12 atomic #, Magnesium, 24.3050 atomic mass, group 2 Alkaline earth metals
What is the mass number of tin-120?
120
Al
13 atomic #, Aluminum, 26.9815 atomic mass, group 13 Transition Metal
What is the mass number for an atom of barium containing 56 protons and 82 neutrons?
138 (FEEDBACK: 56=82=138
Si
14 atomic #, Silicon, 28.0855 atomic mass, group 14 Transition Metal
A popular car has a gas tank that holds a maximum of 14.5 gallons of fuel. what is the size of the tank in liters
14.5gal x 3.785L/1gal=54.9L
How many neutrons are in an atom of uranium-235?
143 ( FEEDBACK: has a mass of 235 uranium has 92 protons therefore has 143 neutrons)
An unknown element is a mixture of isotopes ¹⁵¹X (atomic mass = 150.99 amu) and ¹⁵³X (atomic mass = 153.03 amu). The average atomic mass of X is 151.69 amu. What is the percent abundance of ¹⁵³X?
153.03(x) amu+150.99(1-x) amu=151.69amu (153.03-150.99)x=151.69-150.99 x=151.69-150.99=0.70/153.03-150.99=2.04=0.343 0.343x100% 34.5%
p
15atomic #, Phosphorus, 30.9736 atomic mass, group 15 pnictogens
S
16 atomic #, Sulfur, 32.065 atomic mass, group 16 chalcogens
Cl
17 atomic #, Chlorine, 35.453 atomic mass, group 17 halogens
Ar
18 atomic #,Argon, 39.948 atomic mass, group 18 noble gases
K
19 atomic #, Potassium, #9.0983 atomic mass, group 1 Alkali metal
Which of the following contains the most moles of atoms?
1g of helium
The ground state electron configuration of an Al atom is
1s²2s²2p⁶3s²3p¹
What is the electron configuration of K⁺
1s²2s²2p⁶3s²3p⁶
What is the electron configuration of Co²⁺?
1s²2s²2p⁶3s²3p⁶3d⁷
The ground state electron configuration of a Se atom is
1s²2s²2p⁶3s²3p⁶4s²3d¹⁰4p⁴
Which of the following is the electron configuration of a neutral Fe atom?
1s²2s²2p⁶3s²3p⁶4s²3d⁶
When an electron in excited energy level drops to a lower energy level, a photon is emitted. If the electron is dropping to n=1, which transition will emit the longest wavelength? n=______ to n=1.
2
He
2 atomic #, Helium, 4.0026 atomic mass, group 18 noble gases
A patient is prescribed 100.0mg/day of antibiotic for 2 weeks. the antibiotic is available in vails that contain 20.0 mg/vial of the drug. how many vials are necessary for the entire treatment?
2 weeks x7 days/1wkx100.0 mg/1daysx1 vials/20.0mg=70.0 vials
what is the mass in grams of 2.50 gal of water? the density of water is 1.00 g/ml
2.50galx3.785L/1galx1000mL/1Lx1mL/1g=9.46g/mL
Ca
20 atomic#, Calcium, 40.078 atomic mass, group 2 Alkaline earth metals
Sc
21 atomic #, Scandium, 44.9559 atomic mass, group 3 Transition Metal
Ti
22 atomic #, Titanium, 47.867 atomic mass, group 4 Transition Metal
The answer to the calculation below with the correct number of significant figures is 3.42+ 45.96/0.21
220 ( FEEDBACK: 222.2771429 sig fig 2)
V
23 atomic #, Vanadium, 50.9415 atomic mass, group 5 Transition Metal
Cr
24 atomic #, Chromium, 51.9961 atomic mass, group 6 Transition Metal
Mn
25 atomic #, Manganese, 54.9380 atomic mass, group 7 Transition Metal
how many moles of propylene (C3H6) are in 25.0g of the substance
25.0 gC3H6 x 1 mol C3H6/42.09gC3H6= 0.594 molC3h6
A chemist has a block of gold metal (density is 19.3 g/mL). They drop the metal into a graduated cylinder containing water, and find the volume change is 1.30 mL. What is the mass of the block, in grams?
25.1g (FEEDBACK:19.3xg/1.30mL)
Fe
26 atomic #, Iron, 55.845 atomic mass, group 8 Transition Metal
Co
27 atomic #, Cobalt, 58.9332 atomic mass group 9 Transition Metal
How many hydrogen atoms are in 27 molecules of diborane, B₂H₆?
27x6=162
Ni
28 atomic #, Nickel, 58.6934 atomic mass, group 10 Transition Metal
Cu
29 atomic #, Copper, 63.546 atomic mass, group 11 Transition Metal
How many chlorine atoms are in 29 molecules of chloroform, CHCl₃?
29x3= 87
How many significant figures does the number 67,200 have?
3
Li
3 atomic #, Lithium, 6.941 atomic mass, group 1 Alkali metal
A cooking recipe lists adding 3.0 qt of water as a step. How many mL of water is this?
3.0 qtx 1L/1.0567qtx1000mL/1L=2800mL
A liquid in the lab has a density of 1.17g/c3 what is the volume in liters of 3.02 kg of the liquid?
3.02kgx102g/1kgc1cm3/1.17gx0.001L/1cm3 =2.58L
The number 3780000 written in scientific notation would be
3.78x10^6
Zn
30 atomic #, Zinc, 65.409 atomic mass, group 12 Transition Metal
Ga
31 atomic #, Gallium, 69.723 atomic mass, group 13 Transition Metal
Ge
32 atomic #, Germanium, 72.64 atomic mass, group 14 Transition Metal
convert 32.1 in to centimeters
32.1 in x 2.54cm/1in = 81.5 cm
As
33 atomic #, Arsenic, 74.9216 group 15 pnictogens
Se
34 atomic #, Selenium, 78.96 atomic mass, group 16 chalcogens
Br
35 atomic #, Bromine, 79.904 atomic mass, group 17 halogens
Kr
36 atomic #, Krypton, 83.798 atomic mass, group 18 noble gases
Cs
37 atomic #, Cesium, 132.9055 atomic mass, group 1 Alkali metal
Rb
37 atomic #, Rubidium, 85.4678 atomic mass, group1 Alkali metal
How many protons are in an atom of strontium-90?
38
Sr
38 atmoic #, Strontium, 87.62 atomic mass, group 2 Alkaline earth metals
Y
39 atomic #, Yttrium, 88.9059 atomic mass, group 3 Transition Metal
Which of the following orbitals cannot exist?
3f
For which atomic orbital does n = 3 and ℓ = 1?
3p
Be
4 atomic #, Beryllium, 9.0122 atomic mass, group 2 Alkaline earth metals
determine the number of mole in 4.21x1023 molecules of CaCl2
4.21x1023 molecules of CaCl2 x 1 molCaCl2/6.022x1023 molecules CaCl2= 0.699 molCaCl2
Zr
40 atomic # ,Zirconium, 91.224 atomic mass, group 4 Transition Metal
Mo
42 atomic #, Molybdenum, 95.94 atomic mass, group 6 Transition Metal
Tc
43 atomic #, Technetium, 98 atomic mass, group 7 Transition Metal
A popular car has an engine that is reported to have a volume of 4320 cm3. what is the size in cubic inches
4320 cm3x 1in3/16.387cm3=264in3
Ru
44 atomic #, Ruthenium, 101.07 atomic mass, group 8 Transition Metal
Rh
45 atomic #, Rhodium, 102.9055 atomic mass, group 9 Transition Metal
The answer to the calculation below with the correct number of significant figures is 67.2(45.67-44.98)
46 (FEEDBACK: 67.2(45.67-44.98)= step 1 (45.67-44.98) step 2 6.72x0.69=)
Pd
46 atomic #, Palladium, 106.42 atomic mass, group 10 Transition Metal
Ag
47 atomic #, silver, 107.8682 atomic mass, group 11 Transition Metal
Cd
48 atomic #, Cadmium, 112.411 atomic mass, group 12 Transition Metal
In
49 atomic #, Indium, 114.818 atomic mass, group 13 Transition Metal
In a multi-electron atom, which orbital will have the highest energy
4f
How many significant figures does the number 0.054901 have?
5
How many significant figures does the number 48.050 have?
5
B
5 atomic #, Boron, 10.811 atomic mass, group 13 Transition Metal
A large stone weights 53.0 kg how many pounds does it weight
5.30kg x 2.205lb/1kg=117lb
Sn
50 atomic #, Tin, 118.710 atomic mass, group 14 Transition Metal
Sb
51 atomic #, Antimony, 121.760 atomic mass, group 15 pnictogens
Te
52 atomic #, Tellurium, 127.60 atomic mass, group 16 chalcogens
I
53 atomic #, Iodine, 126.9045 atomic mass, group 17 halogens
Xe
54 atomic #, Xenon, 131.293 atomic mass , group 18 noble gases
An atom of the isotope ¹³³Cs contains how many protons (p), neutrons (n), and electrons (e)?
55p,78n,55e (FEEDBACK: step 1: 133=55+x step 2: 78=x)
Ba
56 atomic #, Barium, 137.327 atomic mass, group 2 Alkaline earth metals
What is the atomic number for an element whose mass number is 138, which contains 81 neutrons per atom?
57 (FEEDBAK: 138-81+57)
How many electrons can be assigned to orbitals designated by the quantum numbers n = 2, ℓ = 1?
6
C
6 atomic #, carbon, 12.0107 atomic mass, group 14 Transition Metal
The bay of Fundy in Nova scotia, Canada is reported to have the largest tides in the world with high tide and low tide occurring two times per day. the tides can measure over approximately 50.0 ft in height at the Hopewell rocks at Hopewell cape, on a specific day height increase was recorded as a rate of 6.08 ft per hour what is the rate in meter per second
6.08 ft/hr x 1 hr/60 minx 1in/60sx0.3048m/60 min=5.15x10-4m/s
The number 0.00000620 written in scientific notation would be
6.20 x10^-6
Which of the following atoms has the same number of neutrons as ⁵⁹Ni?
60Cu ( FEEDBACK: Step1: 59 mass =28protons+x Step2: 31neutron=x 59Ni step1: 60mass=29+x step2: 31neutrons =x)
What is the mass number for an atom of nickel containing 28 protons and 33 neutrons?
61 (FEEDBACK: 28+33=61
N
7 atomic #, Nitrogen,14.0087 atomic #, group 15 pnictogens
What is the wavelength (in nm) of a photon if the energy is 7.26 × 10⁻¹⁹ J? (h = 6.626 × 10⁻³⁴ J • s)
7.26x10-19j=6.626x10-34jxs)(3.00x108m/s)/λ λ= 2.74x10-7 m step2: 2.74x10-7 mx 1x109nm/1m=274nm
an atom of a particular element has a volume of 7.8x10-31 m3 what is this volume in cubic nanometers
7.8x10-31 m3x (108)3 nm3/1m3=7.8x10-4nm3
Hf
72 atomic #, Hafnium, 178.49 atmoic mass, group 4 Transition Metal
Ta
73 atomic #, Tantalum, 180.9479 atomic mass, group 5 Transition Metal
W
74 atomic #, Tungsten, 183.84 atomic mass, group 6 Transition Metal
Re
75 atomic mass, Rhenium, 186.207 atomic mass, group 7 Transition Metal
a human hair is 75.0 um across how many inches is this
75.0 um x 0.001/2.54 um=0.00300 in
Os
76 atomic #, Osmium, 190.23 atomic mass, group 8 Transition Metal
Ir
77 atomic #, Iridium, 192.217 atomic mass Group 9 Transition Metal
Pt
78 atomic #, Platinum, 195.078 atomic mass, group 10 Transition Metal
Au
79 atomic #, Gold, 196.96666 atomic mass, group 11 Transition Metal
O
8 atomic #, Oxygen, 15.9994 atomic mass, group 16 chalcogens
The number 875000 written in scientific notation would be
8.75x10^5
Hg
80 atomic #, Mercury 200.59 atomic mass, group 12 Transition Metal
Tl
81 atomic #, Thallium, 204.3833 atomic mass, group 13 Transition Metal
Pb
82 atomic #, Lead, 207.2 atomic mass, group 14 Transition Metal
Bi
83 atomic #, Bismuth, 208.9804 atomic mass, group 15 pnictogens
Po
84 atomic #, Polonium, 209 atomic mass, group 16 chalcogens
Rn
86 atomic #, Radon, 222 atomic mass, group 18 noble gases
Fr
87 atomic #, Francium, 233 atomic mass, group 1 Alkali metal
Ra
88 atomic #, Radium, 226 atomic mass, group2 Alkaline earth metals
F
9 atomic #, Fluorine, 18.9984 atomic mass, group 17 halogens
Calculate the wavelength in meters of electromagnetic radiation that has a frequency of 980.0 kHz. (c = 3.00 X 10⁸ m/s)
980.0khzx1000hz/1khz=9.800x105hz=9.800x105s-1 λ=c/v=3.00x108m/s/9.800x105s-1=306.1m
How many hydrogen atoms are in three formula units of ammonium benzoate, C₆H₅COONH₄?
9x3=27
How would you determine the formula weight of NaCl?
Add the mass of sodium (22.99 amu) plus the mass of chlorine together (35.45 amu).
What is the formula of a compound containing Al³⁺ and S²⁻ ions?
Al2S3
Which of the following contains the highest number of atoms?
All contain an equal number of atoms
Which color (frequency) of light travels the fastest in a vacuum
All have the same speed
If you go mini-golfing, in which of these scenarios are you precise but not accurate?
All of your shots are off, but they all go to the same place.
Which of the following pairs of ions represent isoelectronic species?
Al³⁺ and O²⁻
Predict the chemical formula for the ionic compound formed by Au³⁺ and HSO₃⁻
Au(HSO₃)₃
What is the formula for an ionic compound containing Ba²⁺ ions and Cl⁻ ions?
BaCl2
Which of the following is an alkaline earth metal?
Beryllium
Which of the following is a main group element?
Bismuth
Polystyrene is made up of a series of styrene (C₈H₈) monomer units. What is the empirical formula for styrene?
CH
Predict the chemical formula for the ionic compound formed by Ca²⁺ and ClO₃⁻
Ca(ClO₃)2
The density of water is approximately 1 g/cm³. Which of these objects will float on water?
Cedar wood block, d=0.380 g/cm3 (FEEDBACK: 1x g/cm3=)
Which of the following is a pure substance that cannot be broken down into simpler substances by chemical means?
Chemical Element
Which of the following is a pure substance that can be broken down into simpler substances by chemical means?
Compound
Which of the following is a chemical change?
Cooking an egg
The element symbol for copper is
Cu
Predict the chemical formula for the ionic compound formed by Cu²⁺ and P³⁻
Cu₃P2
Density fomula
D=mass(g)/volume(mL)
Which of the following are physical properties of matter?
Density
What is the energy of a mole of photons that have a wavelength of 705 nm?
E(6.626x10-34jxs)(3.00x108m/s)/7.05x10-7m =2.81957x10-19j step2: 2.81957x10-19j /1 photon x 6.02x23 photon / 1 mol =1.70x105j
A photon has a frequency of 8.6 × 10⁸ Hz. What is the energy of this photon?
E=(6.626x10-34j.s)(8.6x108 1/s) =5.7x10-25j
Determine the energy of a photon with a wavelength of 364 nm.
E=(6.626x10-34jxs)(3.00x108 m/s)/3.64x10-7m=5.46x10-19j
Einstein's work on the photoelectric effect validated and made extensive use of which of the following equations?
E=hv
Which of the following is true concerning successive ionizations of an atom and its ions?
Each successive ionization requires increasing amounts of energy.
The energy released in the reaction F(g) + e⁻ → F⁻(g) is known as the
Electron affinity
Cathode rays are composed of what fundamental particle?
Electrons
Bohr formula
En = -2.18 x 10 ^ -18 J / n^2
photon formula
Ephoton = hv
What group (G) and period (P) does the element molybdenum (Mo) belong to?
G = 6, P =5
Which of the following states of matter is pictured below?
Gas
alkali metals
Group 1 (Li,Na,K,Rb,Cs,Fr)
Halogens
Group 17 (F,Cl,Br,I,At,Ts)
The accepted value for the density of iron is 7.9 g/mL. Which of the following sets of experimental data for the density of iron is the most accurate?
Group 1: 7.98 g/mL, 7.85 g/mL
alkaline earth metals
Group 2 (Be,Mg,Ca,Sr,Ba,Ra)
The accepted value for the density of iron is 7.9 g/mL. Which of the following sets of experimental data for the density of iron is the most precise?
Group 2: 7.65 g/mL, 7.64 g/mL
Columns on the periodic table are known as
Groups
Which of the following compounds does not contain a polyatomic ion?
H2S
The atomic radii of zirconium (Zr) and hafnium (Hf) are nearly the same despite the fact that hafnium has 32 more protons and electrons. Which of the following bests explains this phenomenon?
Hafnium contains electrons in the 4f orbitals. These 4f electrons do not effectively shield the higher nuclear charge and thus Zeff is higher than might be otherwise expected.
Italian dressing contains olive oil and vinegar, which will separate out from each other if left to sit. This makes the dressing a:
Heterogeneous Mixture
What quantum mechanics principle states that electrons are added to atomic orbitals with the same energy so that each orbital is singularly occupied with electrons having the same spin?
Hund's rule
Which of the following statements about subatomic particles are false? I. Neutrons reside inside of the nucleus. II. The atomic number is equal to the number of neutrons in the nucleus of an atom. III. Electrons are more massive than protons.
II. The atomic number is equal to the number of neutrons in the nucleus of an atom. III. Electrons are more massive than protons.
Consider these electron transitions in a hydrogen atom: I. n = 2 → n = 1 II. n = 3 → n = 1 III. n= 1 → n = 4 Which of the electron transitions would release the most energy?
II. n = 3 → n = 1
Excited hydrogen atoms emit radiation in which region(s) of the electromagnetic spectrum?
IR, visible, and UV
Which periodic trend quantifies the amount of energy required to remove an electron from a neutral, gaseous atom?
Ionization Energy
Which of the following electron configurations is incorrect?
Mn [Ar]4s²4d⁵
Considering periodic trends, valence electrons in which of the following atoms experience the greatest effective nuclear charge (Zeff)?
Ne
Which element is classified as a noble gas?
Neon (ne)
Which subatomic particle is found in the nucleus and has no charge?
Neutron
If a kicker kicks a 38-yard field goal to win the championship game. You are asked to convert the distance to meters. Consider how yards and meters compare in size to each other. Indicate how you would expect the number of yards to the field goal to compare to the number of meters.
Number of yards > Number of meters
Similar properties recur periodically when elements are arranged according to increasing atomic number is the statement of the ______.
Periodic Law
Of the following compounds, which contains a metalloid?
SiF4
Which is not one of Dalton's hypotheses of atomic theory?
The atoms of one element are the same as atoms of another element.
In which direction in a given period of the periodic table does melting point tend to increase?
The closer an atom is to having a half-full valence shell, the higher the melting point (high in the 'middle' of the period and low at the ends).
Which of the following laws explains the following statement? Acetylene gas, regardless of its method of preparation, always has the same carbon to hydrogen ratio.
The law of definite proportions
In two chemical reactions, 4.0 grams of oxygen combine with 3.0 grams of carbon to form one compound, and 8.0 grams of oxygen combine with 3 grams of carbon to form another. This can be explained by:
The law of multiple proportions
The atomic mass of germanium (Ge) on the periodic table is 72.630 amu. Which of the following best explains why the atomic mass is a fraction between 72 and 73?
The presence of different isotopes
What is the atomic symbol for the element in Group 4B (4) and the fourth period?
Ti
A student is determining the density of an unknown metal with a mass of 32.56 g. The student partially fills a graduated cylinder with water and measures the volume of the water by itself as 14.78 mL. The student then adds the metal to the water and measures the new volume as 20.44 mL. What is the identity of the metal?
Tin, d = 5.75 g/mL(FEEDBACK: 20.44mL-14.78mL=5.66mL d=32.56g/ 5.66mL=)
Which electron configuration violates Hund's rule?
[He]2s²2px²2py²
Which of the following is the electron configuration for Ba
[Xe]6s²
A white powder mixture is placed into water. Some of the powder sinks to the bottom of the container, some rises to the top. The separation of the powder mixture is an example of
a physical change
An atom has nine protons and ten electrons. This makes it:
an ion
Which of the following is an intensive physical property of a lump of coal?
color
What type of bonding is present in C₁₂H₂₂O₁₁?
covalent bond only
Energy of a photon is ______ proportional to frequency, and _______ proportional to wavelength.
directly and inversely
Density is defined as mass _____________ volume.
divided by
In which direction on the periodic table does metallic character increase?
down and to the left
The trend towards smaller atomic radii as one moves to the right in a period is _____.
due to the effective nuclear charge increasing.
The net charge on an atom of a given element changes as ______ are added or removed.
electrons
In the Bohr model of the hydrogen atom, the energy required to excite an electron from n = 2 to n = 3 is _______________ the energy required to excite an electron from n = 3 to n = 4?
greater than
Nobel Gas
group 18 (He,Ne,Ar,Kr,Xe,Rn)
transition metal
group 3 -12 (Sc;Y,Ti;Zr;Hf;Rf,V;Nb;Ta;Db,Cr;Mo;W;Sg,Mn;Tc;Re;Bh,Fe;Ru;Os;Hs,Co;Rh;Ir;Mt,Ni;Pd;Pt;Ds,Cu;Ag;Au;Rg,Zn;Cd;Hg;Cn)
Elements that are most similar in their properties are found
in the same group.
What is observed when a noble gas is heated and the emitted light shone through a prism?
individual lines of varying colors
Classify the following compounds as ionic or covalent: BaO, Fe₂O₃, ZnO.
ionic,ionic,ionic
Which of the following metric prefixes corresponds to 10³?
kilo
Red light has a _____ frequency and a _____ wavelength than ultraviolet rays.
lower , longer
Which of the following metric prefixes corresponds to 10⁻³
milli
Carbon dioxide is a _____ compound composed two types of _____ atoms.
molecular; nonmetal
Rutherford's gold foil experiment determined that
most of the space in an atom is empty except for a concentrated area called the nucleus.
Which of the following sets of quantum numbers can describe a 3p electron?
n = 3, ℓ = 1, mℓ = 1
A ground state atom of As could not have any electrons with which of the following configurations?
n = 4, ℓ = 2, mℓ = 0, ms = +½
If ℓ = 0, which of the following may be true?
n=6
Which two particles of the atom have nearly identical masses?
proton and neutron
The nucleus of an atom contains
protons and neutrons
Which particle(s) may be found in the nucleus of an atom?
protons and neutrons
Which type of electromagnetic radiation has the largest wavelength?
radio waves
Which of the following is a transition metal?
silver
Which of the following states of matter is pictured below?
solid
Light wave A has a greater frequency than light wave B. Which has a greater wavelength?
wave B
What is the energy, in J, of light that must be absorbed by a hydrogen atom to transition an electron from n = 3 to n = 6? Submit an answer to three signficant figures.
ΔEi→f= ΔE3→6=2.18x10-18j(1/6^2-1/3^2)=-1.82x10-19j
For a hydrogen atom, calculate the wavelength of light (in m) that would be emitted for the orbital transition of n(initial) = 2 to n(final) = 1. Submit an answer to four significant figures. The Rydberg constant is 1.09678 x 10⁷ m⁻¹.
λ- 1/1.09678x10^7(1-1/2^2)=1.216x10-7m
the de broglie equation
λ=h/mv
