Test 1 Quiz Questions Flashcards by Morgan Harrison

Match the appropriate classification to the substance
Cu-
NaCl-
Whipped cream-
Apple Pie

Options:
Compound
Homogeneous mixture
Element
Heterogeneous mixture

Cu- Element
NaCl- Compound
Whipped cream- Homogeneous mixture
Apple Pie- Heterogeneous mixture

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Which is the substances listed below is a pure compound? Choose all that apply
1)Oxygen
2) Carbon Monoxide
3) Air
4) S8
5) CaCO3

Carbon Monoxide
CaCO3

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Which of the substances below is a pure element? Choose all that apply
1)Oxygen
2) Carbon Monoxide
3) Air
4) S8
5) CaCO3

Oxygen
S8

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Match the appropriate classification to the substance
Air-
O2-
CO2-
Salad Dressing-

Options:
Compound
Pure substances
Heterogeneous mixture
Homogenous mixture

Air- Homogenous mixture
O2- Pure substance
CO2- Compound
Salad Dressing- Heterogeneous mixture

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Determine if each of the following is a physical or chemical change
1) Sugar dissolving in water
2) Human growth
3) Tarnishing of silver
4) Evaporation of water

1) Physical change
2) Chemical change
3) Chemical change
4) Physical change

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Classify each of the following as a physical or chemical change
1) Iron rusting
2) Wood burning
3) Photosynthesis
4) A gas expanding as it is heated

1) Chemical change
2) Chemical change
3) Chemical change
4) Physical change

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Classify each of the following as a physical or chemical property
1) Hydrogen will burn in air
2) Using electricity, liquid water can be converted to hydrogen and oxygen gases
3) Gold is a solid at room temperature
4) Gold melts at 1064 degrees Celsius

1) Chemical property
2) Chemical property
3) Physical property
4) Physical property

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Complete the relationships wit the appropriate value
1) 1 x _________ kg = 1g
2) 1 x _________ m = 1 um
3) 1 x _________ mmole = 1 mol
4) 1 x _________ ns = 1 s

Options:
10E2
10E-6
10E3
10E-9
10E-3
10E9
10E-2

1) 10E-3
2) 10E-6
3) 10E3
4) 10E9

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Match the prefix to the appropriate situation
1) 1 x 10E9 m = 1 ____ m
2) 1 x 10E-6 s = 1 _____ s
3) 1 x 10E6 byte = 1 _____ byte
4)1 x 10E-2 gram = 1 ___ gram

Options:
nano
giga
kilo
micro
milli
mega
deci
centi

1) giga
2) micro
3) mega
4)centi

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Math Question:

To evaluate precision one looks at the average deviation of the values. What is the average deviation of the following densities: 4.17, 4.77, 4.64?

.24

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Math Question:

To evaluate precision one looks at the average deviation of the values. What is the average deviation of the following densities: 4.23, 4.78, 4.62?

.21

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Math Question:

What is the answer with the correct significant digits

0.732 x 23.85

17.5

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Math Question:

What is the answer with the correct significant digits?
5.24 / 143

0.0366

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Math Question:

What is the answer with the correct significant digits
0.196 + 4.4

4.6

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Math Question:

What is the answer with the correct significant digits
38.7 - 7.3

31.4

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Math Question:

What is the answer with the correct significant digits

5.01(0.032 + 5.53)

27.9

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Math Question:

What is the answer with the correct significant digits
(16.1 - 11.4)/6.22

0.76

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Math Question:

Convert 6.06 km2/hr to mm2/min.

101,000,000,000

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Math Question:

Convert 3.14 N/mm2 to kN/km2.

3,140,000,000

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Convert 4.81 x 10 6 nm3 to __________ mm3

Choose from the options below
1) 4.81
2) 4.81e18
3) 4.81e-18
4) 4.81e3
5) 4.81e-12

5) 4.81e-12

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Math Question:

A block has a surface area of 0.15 cm^2. What is its surface area in mm^2?

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Math Question:

A 20.87 g piece of metal is dropped into a graduated cylinder with 108.4 mL of water. If the density of the metal is 4.18 g/cm3, what is the total volume in the graduated cylinder in mL with the correct number of significant digits?

113.4

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Math Question:

A block has a mass of 16.97 g and sides of length: 13.1 mm, 19.6 mm, 13.9 mm. What is its density in g/cm^3?

4.75

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Math Question:

13.1 g of a solid is dissolved in 102.5 mL of water with a density of 1.01 g/mL. If the total volume of the solution is 107.4 mL, what is the density of the solution in g/mL with the correct number of significant digits

1.09

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Math Question: A 48.94 g piece of metal is dropped into a graduated cylinder with 100.8 mL of water. If the total volume in the cylinder is 116.9, what is the density (in g/mL) of the metal with the correct number of significant digits?

3.04

An atom with 12 protons, 13 neutrons, and 10 electrons will have an atomic number of________, a mass number of_________, and a charge of_________.

12 25 +2

There are ______ protons, ________ electrons, and ________ neutrons in a nitride ion, 13^N^3- (look up google for better look of this)

7 10 6

An atom with 82 protons, 125 neutrons, and 78 electrons will have a mass number of ________, an atomic number of ________, and a charge of ________.

207 82 +4

A particular atom has 27 protons and 33 neutrons. What is the atomic number, mass number, and periodic table symbol of this isotope? Atomic Numer: Mass Number: Periodic Table Symbol:

Atomic Number: 27 Mass Number: 60 Periodic Table Symbol: Co

A particular atom has 58 protons and 82 neutrons. What are the atomic number, mass number, and periodic table symbol of this isotope? Atomic Number: Mass Number: Periodic Table Symbol:

Atomic Number: 58 Mass Number: 140 Periodic Table Symbol: Ce

How many protons, neutrons and electrons are in the neutral atom Radon - 220? Radon = Rn Protons: Neutrons: Electrons:

Protons: 86 Neutrons: 134 Electrons: 86

What is always the difference between two isotopes on an element? Options: 1) Number of neutrons 2) Number of protons 3) Number of electrons

1) Number of neutrons

Math Question: A fictitious element that has two isotopes has an average atomic mass of 159.7. If 73.21% of the atoms of the element have an atomic mass of 161.3, what is the atomic mass of the other isotope?

155.3

Math Question: A ficticious element has three isotopes. What is its average atomic mass? Isotope 1. Mass = 98.91 amu Abundance = 33.38 % Isotope 2. Mass = 96.76 amu Abundance = 55.83 % Isotope 3. Mass = 94.66 amu Abundance = 10.79 %

97.25

Math Question: How many moles of CH4 is equivalent to 21.2 g of CH4 (MW= 16.04 g/mol)

1.32

Math Question: How many moles of Pb(SO4)2 are equivalent to 167.5g of Pb(SO4)2 (MW= 399.34 g/mol)

0.4194

Math Question: What is the mass of 0.066 moles of zinc phosphate: Zn3(PO4)2 (MW= 386.17 g/mol)

25.5

How many molecules of hydrofluoric acid (HF) are in 224 g of HF (MW= 20.01 g/mol)

6.74e24

Math Question: What is the mass of 5.74 x 10^21 formula units of sodium hydroxide NAOH (MW= 40.00 g/mol)

0.381

Math Question: How many moles of hydroxide ion are in 6.26 moles of aluminum hydroxide: Al(OH)3 (Mw= 78.00 g/mol)

18.78

Math Question: What mass of oxygen is 62.2 g of magnesium nitrate: Mg(NO3)2 (Mw= 148.33 g/mol)

40.3

Math Question: How many atoms of oxygen are in 6.94 moles of H2O2 (Mw= 34.02 g/mol)

8.36e24

Math Question: How many moles of oxygen atoms are in 5.49 moles of magnesium phosphate: Mg3(PO4)2 (Mw= 262.87 g/mol)

43.9

Math Question: How many carbon atoms are in 1.15 g of dextrose: C6H12O6 (Mw= 180.16 g/mol)

2.31e22

How many H atoms are in 259 g of C12H21O9? (Molar mass of C12H21O9 = 309.29 g/mol) Options: 1) 4.54 x10^24 2) 1.06 x 10^25 3) 6.05 x 10^24 4) 5.40 x 10^23 5) 1.80 x 10^24

2) 1.06 x 10^25

How many O atoms are in 259 g of C12H21O9? (Molar mass of C12H21O9 = 309.29 g/mol) Options: 1) 4.54 x10^24 2) 1.06 x 10^25 3) 6.05 x 10^24 4) 5.40 x 10^23 5) 1.80 x 10^24

1) 4.54 x 10^24

Math Question: What is the frequency in hertz of a photon of light with an energy of 4.12 x 10-21J?

6,220,000,000,000

What is the energy (in Joules) of a photon with a wavelength of 400. nm? Options: 1) None of them 2) 4.97e-21 3) 8.83e-49 4) 4.97e-17 5) 4.97e-19 6) 8.83e-47

5) 4.97e-19

Light with a wavelength of 300nm has__________ frequency and __________ energy per photon compared to a light with a wavelength of 800nm Options: 1) Higher, More 2) Lower, More 3) Lower, Less 4) Higher, Less

1) Higher, More

Sort the following from the greatest (1) energy to smallest energy (6) of a photon Options: Radio Waves Visible Light X-Rays Microwave Radiation Ultraviolet Radiation Infrared Radiation

1) X-Rays 2) Ultraviolet Radiation 3) Visible Light 4) Infrared Radiation 5) Microwave Radiation 6) Radio Waves

Which of the following transitions for an electron in a hydrogen atom emits light with the largest frequency? Options: 1) n=6 --> n=5 2) n=4 --> n=7 3) n=3 --> n=5 4) n=7 --> n=5 5) n=3 --> n=1 6) n=1 --> n=2 7) n=1 --> n=4 8) n=2 --> n=1

5) n=3 --> n=1

Which of the following ideas related to the Bohr Model of the atom do we no longer like? Options: 1) Electrons orbit the nucleus at specific distances 2) Electrons occupy specific energy states within an atom 3) Electrons can transition between energy states by absorbing or releasing energy

1) Electrons orbit the nucleus at specific distances

Using de Broglie's equation, what is the wavelength of an electron (mass = 9.109 x 10^-31 kg) moving at 4.00 x 10^7 m/s Options: 1) 1.82e-11 2) 1.82e-3 3) None of these answers 4) 1.82e4 5) 1.82e-8

1) 1.82e-11

What are the possible quantum numbers for potassium's electron in the 4s energy level n=_____ I=______ ml=______

4 0 0

What is a possible set of quantum numbers for one of silver's electrons in the 4d energy sublevel n=______ I=_______ ml=_______

4 2 0

What is a single set of possible quantum numbers for one of iron's electrons in the 3d energy sublevel n=_____ I=______ ml=______

3 2 0

What is a possible set of quantum numbers for one of tin's electrons in the 5p energy sublevel n=_____ I=______ ml=______

5 1 0

What is a possible set of quantum numbers for one of uranium's electrons in the 5f energy sublevel n=_____ I=______ ml=______

5 3 0

Which set of quantum numbers below is incorrect (rows go by n, I, ml, ms or s) 1) 3, 1, 0, -1/2 2) 1, 0, 0, -1/2 3) 3, 2, 2, +1/2 4) 1, 0, -1, +1/2 5) 2, 1, -1, -1/2

4) 1, 0, -1, +1/2

Which set of quantum numbers below is incorrect (rows go by n, I, ml, ms or s) 1) 3, 1, -1, -1/2 2) 1, 0, 0, -1/2 3) 1, 1, 0, +1/2 4) 2, 1, -1, -1/2 5) 3, 2, 0, +1/2

3) 1, 1, 0, +1/2

Match the energy sublevel to the maximum number of electrons that can be held in the sublevel 5s= 3p= 5d= 6f= Options: 4 20 2 18 6 10 12 14

5s= 2 3p= 6 5d= 10 6f= 14

Match the energy sublevel to the number of orbitals in the sublevel 7s= 3d= 2p= 4f= Options: 4 1 8 5 3 6 7

7s= 1 3d= 5 2p= 3 4f= 7

Which of the following is not an allowed value for the quantum number I (ell) is quantum number n=3 Options: 1) 3 2) 0 3) 1 4) 2

1) 3

What are the values of n and I for the electrons in the 4f sublevel n= I=

n= 4 I= 3

What is the electron configuration of As

1s2 2s2 2p6 3s2 3p6 4s2 3d10 4p3

What is the electron configuration of Kr

1s2 2s2 2s6 3s2 3p6 4s2 3d10 4p6

What is the electron configuration of Ge

1s2 2s2 2s6 3s2 3p6 4s2 3d10 4p2

What is the electron configuration of Ga

1s2 2s2 2s6 3s2 3p6 4s2 3d10 4p1

How many electrons does the vanadium 4+ (V^4+) ion have in each sublevel 1s= 2s= 2p= 3s= 3p= 4s= 3d=

1s=2 2s=2 2p=6 3s=2 3p=6 4s=0 3d=1

What is the electron configuration of S^-2 Options: 1) [Ne] 3p4 2) [Ne] 3s23p2 3) [Ne] 3s43pp4 4) [Ne] 3s23p6

4) [Ne] 3s23p6

Draw the orbital filling diagrams for bromine. Enter a number for the electrons that are paired or unpaired in each sub levels 4s Paired= Unpaired= 3d Paired= Unpaired= 4p Paired= Unpaired=

4s Paired= 2 Unpaired= 0 3d Paired= 10 Unpaired= 0 4p Paired= 4 Unpaired= 1

Draw the orbital filling diagrams for silicon. Enter a number for the electrons that are paired or unpaired in each of the sublevels. 1s Paired= Unpaired= 2s Paired= Unpaired= 2p Paired= Unpaired 3s Paired= Unpaired= 3p Paired= Unpaired=

1s Paired= 2 Unpaired= 0 2s Paired= 2 Unpaired= 0 2p Paired= 6 Unpaired= 0 3s Paired= 2 Unpaired= 0 3p Paired= 0 Unpaired= 2

Germanium has an electron configuration 1s22s22p63s23p64s23d104p2. Which electrons are considered valence electrons? Options: 1) 3d104p2 2) 4s23d104p2 3)1s22s22p63s23p64s23d104p2 4) 4p2 5) 4s24p2

5) 4s24p2

Manganese has an electron configuration 1s22s22p63s23p64s23d5. Which electrons are considered valence electrons Options: 1) 4s2 2) 1s22s22p63s23p64s23d5 3) 4s23d5 4) 3s23p63d5 5) 3d5

3) 4s23d5

Cobalt has an electron configuration 1s22s22p63s23p64s23d7. Which electrons are considered valence electrons Options: 1) 1s22s22p63s23p64s23d7 2) 3d7 3) 4s2 4) 3s23p63d7 5) 4s23d7

5) 4s23d7

Vanadium has an electron configuration 1s22s22p63s23p64s23d3. Which electrons are considered valence electrons Options: 1) 1s22s22p63s23p64s23d3 2) 3d3 3) 3s23p63d3 4) 4s23d3 5) 4s2

4) 4s23d3

What is the approximate effective nuclear charge felt by the valence electrons in Kr? Options: 1) 7+ 2) 3+ 3) 1+ 4) 6+ 5) 5+ 6) 8+ 7) 4+

6) 8+

What is the approximate effective nuclear charge felt by the valence electrons in P Options: 1) 4+ 2) 7+ 3) 5+ 4) 6+ 5) 1+ 6) 2+ 7) 8+

3) 5+

True or False K has a larger radius than Ca

True

True or False Ca has a larger radius than Be

True

Why does K have a larger atomic radius than Na? Options: 1) The valence electrons in K feel a stronger effective nuclear charge than those in Na 2) The valence electrons in Na and K feel a similar Zeff. Those in K are in a higher energy level 3) The valence electrons in Na feel a stronger effective nuclear charge than those in K 4) The valence electrons in Na and K feel a similar Zeff. Those in Na are in a higher energy level 5) K is lower down the group than Na

2) The valence electrons in Na and K feel a similar Zeff. Those in K are in a higher energy level

Why does Ne have a smaller radius than F Options: 1) Ne has more mass than F making it larger 2) Ne is further to the left on the periodic table than F 3) The valence electrons in Ne feel a greater Zeff than those in F 4) Ne has its valence electrons in a higher energy level than F 5) F has more protons in its nucleus than Ne

3) The valence electrons in Ne feel a greater Zeff than those in F

For each pair of ions, choose the one that has the larger radius. O2- or Al3+ Na+ or K+ Options: 1) O2- and Na+ 2) O2- and K+ 3) Al3+ and Na+ 4) Al3 and K+

2) O2- and K+

For each pair of ions, choose the one that has the smaller radius. Na+ or Mg2+ Cl- or K+ Options: 1) Na+ and K+ 2) Mg2+ and Cl- 3) Na+ and Cl- 4) Mg2+ and K+

4) Mg2+ and K+

Which of the following corresponds to the electron affinity of aluminum atoms Options: 1) Al --> Al+ + e- 2) Al+ +e- --> Al 3) Al --> Al3+ +3e- 4) Al + e- --> Al-

4) Al + e- --> Al-

Which of the following is the reaction associated with the electron affinity of zinc Options: 1) Zn(g) → Zn2+(g) + 2e- 2) Zn(g) + e- → Zn-(g) 3) Zn(g) → Zn+(g) + e- 4) Zn(g) → Zn-(g) + e- 5) Zn(g) + 2e- → Zn2-(g)

2) Zn(g) + e- → Zn-(g)

Which of the following is the reaction associated with the first ionization energy of sulfur? Options: 1) S(g) → S-(g) + e- 2) Cl2(g) + 2e- → 2Cl- 3) S(g) → S+(g) + e- 4) S(g) + 2e- → S2-(g) 5) S(g) → S2+(g) + 2e-

3) S(g) → S+(g) + e-

Which of the following is the reaction associated with the first ionization energy of nitrogen? Options: 1) N(g) → N- + e- 2) N(g) + e- → N- 3) N(g) → N+ + e- 4) N(g) + 3e- → N3- 5) N(g) → N3+ + 3e-

3) N(g) → N+ + e-

True or False F has a larger first ionization energy than Cl

True

True or False K has a larger first ionization energy than Mg

False

Which equation is associated with the third ionization energy of aluminum? Options: 1) Al2+(g) → Al3+(g) + e- 2) Al(g) → Al3+(g) + 3e- 3) Al(g) + 3e- → Al3-(g) 4) Al3+(g) → Al(g) + 3e-

1) Al2+(g) → Al3+(g) + e-

Which equation is associated with the fourth ionization energy of carbon? Options: 1) C(g) → C4+(g) + 4e- 2) C3-(g) + e- → C4-(g) 3) C3+(g) → C4+(g) + e- 4) C(g) + 4e- → C4-(g)

3) C3+(g) → C4+(g) + e-

Select the correct answer for the questions below 1) Metallic character_______ going from left to right going across a period 2) Going down a group, metallic character________ 3) Metallic oxides tend to react with acids because they are _______ 4) Metals tend to ________ electrons when they form ions Options: Increase Decrease Acidic Basic Gain Lose

1) Decreases 2) Increases 3) Basic 4) Lose

Select the correct answer for the questions below (1 is used more than once) 1) In general nonmetallic character _______ going from left to right across a period 2) In general, metallic character ________ going down a group 3) Nonmetal oxides tend to be ________ 4) In general, nonmetals tend to form _________ ions (except when bonded with O or F) Options: Increases Decreases Basic Negative Positive Acidic

1) Increases 2) Increases 3) Acidic 4) Negative