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Sem 1- 6 week (2) Flashcards

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1
Q

What was the most important finding in Rutherford’s gold foil experiment?
Electrons orbit the nucleus at specific energy levels.
Protons and neutrons are found in the nucleus of the atom.
Atoms are mostly empty space but not completely empty.
Electrons have a negative charge and protons have a positive charge.

A

Atoms are mostly empty space but not completely empty.

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2
Q

Based on our current understanding of the atom, electrons orbit the nucleus of the atom at specific energy levels.
True
False

A

False

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3
Q 
Which of the following scientists was the first to make observations that showed that atoms existed?
  Democritus 
  Rutherford 
  Thomson 
  Dalton
A

Dalton

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4
Q

Where are the electrons found within the atom?

A

Electrons are found outside of the nucleus.

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5
Q

Where are the protons found within the atom?

A

Protons are found in the nucleus.

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6
Q 
When Thomson performed his cathode ray tube experiment, he found that the beam of gas was attracted to the positively charged plate. If he had found that the beam of gas was attracted to the negatively charged plate, which particle would he have found?
  The proton. 
  The neutron. 
  The electron. 
  The nucleus.
A

The proton.

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7
Q

How many protons does chlorine, Cl, have?

A

17

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8
Q 
What is the mass number of an atom that has 15 protons and 16 neutrons?
  15 
  16 
  31 
  30.97
A

31

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9
Q

Write the isotope notation for an atom that has 7 protons and 9 neutrons.

A

Nitrogen-16

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10
Q

If 15% of the atoms of a certain element have a mass of 14.00 amu and 85% of the atoms have a mass of 15.00 amu, then the average atomic mass is 14.50 amu.
True
False

A

False

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11
Q

Which of the following would the average atomic mass be closest to given the following information?

Isotope Mass (amu) Isotope Abundance (%)

  1. 00 65.74
  2. 00 34.26
  3. 00
  4. 00
  5. 00
  6. 00
A

18.00

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12
Q

An element has three isotopes. The first isotope (4.00 amu) has an abundance of 87.46 %, the second isotope (5.00 amu) has an abundance of 11.57 %, and the third isotope (6.00 amu) makes up the remainder of the abundance. What is the average atomic mass of the element?

  1. 66 amu
  2. 08 amu
  3. 14 amu
  4. 00 amu
A

4.14 amu

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13
Q

In a sample of 200 atoms, 195 are atoms (97.50 % of the total atoms) with a mass of 14.00 amu and 5 atoms (2.50 % of the total atoms) with a mass of 15.00 amu. What is the average atomic mass of this sample? (Be sure to show your work!)

A

14.03 amu

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14
Q

One of nitrogen’s isotopes has a mass number of 15. How many neutrons are in the nucleus of this isotope?

A

Nitrogen- 15

Protons- 7

15-7= 8 Neutrons

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15
Q

(460-370 BCE) A Greek philosopher who theorized that all matter could be reduced to particles that could not be divided, which he described as “atomos.”

A

Democritus

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16
Q
  • everything is made up of atoms
  • atoms are invisible and smallest part of matter
  • all atoms have same element mass and shape
  • atoms can’t be created or destroyed
  • atoms can be combined to make compounds
A

John Dalton

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17
Q
  • did an experiment on how atoms are made up of other components
  • used cathode ray
  • discovered the electron
A

JJ Thomson

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18
Q
  • used gold and alpha, the alpha bounced back b/c of nucleus

- discovered nucleus

A

Ernest Rutherford

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19
Q
  • energy levels

- electrons have energy which keeps them in orbit but they are still attracted to (+)

A

Bohr

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20
Q
  • electron cloud model

- used BOHR MODEL & math to calculate the probabiltity of finding electrons

A

Erwin Schrodinger

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21
Q 
An isotope with 7 protons and 8 neutrons would have which of the following isotope notations?
  P - 15 
  N - 7 
  N - 15 
  O - 15
A

N - 15

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22
Q

Use the following information below to calculate the average atomic mass. Be sure to show your work.

Isotopic Mass Number Relative Abundance
28 66.28%
29 26.34%
30 7.38%

A

28.41 amu

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23
Q

Which of the following was not a conclusion from Rutherford’s experiments with gold foil?

  • The atom is mostly empty space with a small, solid center.
  • Electrons are outside the nucleus at very specific energy levels.
  • The protons are in the nucleus of the atom and electrons are outside the nucleus.
  • There is a tiny nucleus within the atom.
A

Electrons are outside the nucleus at very specific energy levels.

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24
Q

Which element has the following electron configuration?

1s22s22p63s1

Lithium, Li
Magnesium, Mg
Sodium, Na
Neon, Ne

A

Sodium, Na

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25
Q 
How many electrons are in the third energy level for Zirconium, Zr?
  2 
  8 
  10 
  18
A

18

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26
Q

Which of the following is the electron configuration for Cesium, Cs?

A. 1s22s22p63s23p64s23d104p65s25d105p66s1

B. 1s22s22p63s23p64s23d104p65s24d105p66s1

C. 1s22s22p63s23p64s24d104p65s25d105p66s1

D. 1s21p62s22p63s23p64s23d104p65s24d105p66s1

Choice A
Choice B
Choice C
Choice D

A

Choice B

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27
Q 
To write the shorthand configuration for Oxygen, O, which element would you put in brackets?
  Helium, He 
  Oxygen, O 
  Neon, Ne 
  Lithium, Li
A

Helium, He

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28
Q 
The following shorthand configuration belongs to which element? [Kr]5s24d105p5
  Bromine, Br 
  Iodine, I 
  Chlorine, Cl 
  Krypton, Kr
A

Iodine, I

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29
Q

1s22s22p63s23p64s1 is the electron configuration for which element?

A

Potassium

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30
Q

When writing the shorthand notation for sulfur, S, which element would you put in brackets?

A

Neon [Ne]

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31
Q

How many valence electrons does indium, In, have?

A

3

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32
Q

1s22s22p63s23p64s23d1 is the electron configuration for which element?

A

Scandium

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33
Q 
Which of the following is NOT shown in an electron configuration?
  The number of electrons. 
  The spin of the electrons. 
  The energy levels. 
  The sublevels.
A

The spin of the electrons.

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34
Q

Write Selenium’s electron configuration and use it to determine how many valence electrons it has.

A

1s^2^2s2^2p^63s^23p^64s^23d^104p^4

The outermost level is the 4th energy level, and there are 2 electrons in the s orbital and 4 electrons in the p orbital for a total of 6 Valence electrons

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35
Q

Write the electron configuration for Arsenic.

A

1s^22s^22p^63s^23p^64s^23d^104p^3

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36
Q

Write the electron configuration for silver.

A

1s^22s^22p^63s^23p^64s^23d^104p^65s^24d^9

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37
Q 
Which of the following elements would have three valence electrons?
  Calcium, Ca 
  Copper, Cu 
  Gallium, Ga 
  Sulfur, S
A

Gallium, Ga

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38
Q 
Which of the following is not considered electromagnetic radiation?
  Visible light 
  Gamma rays 
  Sound waves 
  Infrared waves
A

Sound waves

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39
Q 
When the energy increases, which of the following decreases?
  Frequency 
  Speed of light 
  Wavelength 
  Planck's constant
A

Wavelength

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40
Q 
The height of a wave is referred to as the \_\_\_\_\_.
  wavelength 
  amplitude 
  trough 
  frequency
A

amplitude

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41
Q

If a t-shirt looks in green in color, which of the following is correct?

  • The atoms in the dye that the t-shirt is made out of gives off green light.
  • The t-shirt absorbs only green light and emits only red light.
  • The t-shirt absorbs only red light and emits only green light.
  • The t-shirt absorbs every color of light except for green light.
A

The t-shirt absorbs every color of light except for green light.

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42
Q

The more waves that pass a point in a given amount of time means they have a longer wavelength.
True
False

A

False

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43
Q

How much energy does a wave with a frequency of 3.78 x 1010 Hz have?

A

2.51 x 10^-23 J

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44
Q 
In a vacuum, all light waves \_\_\_\_\_\_.
  have the same wavelength. 
  have the same energy. 
  have the same speed. 
  have the same frequency.
A

have the same speed.

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45
Q

The energy of a photon is 2.39 x 10-15 J. Calculate the wavelength.

A. 1.20 · 1010 m

B. 8.32 · 10-11 m

C. 3.60 · 1018 m

D. 2.77 · 10-19 m

Choice A
Choice B
Choice C
Choice D

A

Choice B

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46
Q

When an electron absorbs heat and then produces light, what happened to it?

  • The electron vibrates a little within the same energy level.
  • The electron drops an energy level.
  • The electron drops down an energy level and then back up an energy level.
  • The electron jumps up an energy level and then drops down an energy level.
A

The electron jumps up an energy level and then drops down an energy level.

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47
Q

The reason that electrons can absorb light energy is because light not only moves in waves, but also acts like matter that are called photons.
True
False

A

True

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48
Q

Knowing the relationship between energy and frequency and the equation that relates the two, what is the relationship between x and y in the following equation?

x = (28)y

Inverse
Direct
x = y
There is no correlation between x and y

A

Direct

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49
Q

A wave of green light has a wavelength of 505 nm. How much energy does this wave have? Be sure to show your work! (Remember that 1 nm = 1⋅10^-9 m.)

A

3.94 x 10^-19 J

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50
Q

Photon A has a frequency of 5 waves per second and photon B has a frequency of 1 wave per second. Which photon will have the greatest wavelength? Explain how you know.

A

Photon B has a longer wavelength. Light with a longer wavelength has a lower frequency.

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51
Q

The frequency of a wave is 4.28 · 1020 Hz. How much energy does this wave have? Be sure to show your work!

A

2.84 · 10^-13 J

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52
Q 
The amount of energy that an electron has normally is best referred to as its \_\_\_\_\_\_.
  frequency 
  wavelength 
  excited state 
  ground state
A

ground state

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53
Q

The energy of a photon is 6.43 · 10-14 J. What is the wavelength? Be sure to show your work!

A

3.09 · 10^-12 m

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54
Q

The scientist that created the Periodic Table is ________________.

A

Mendeleev first created the Periodic Table.

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55
Q

Mendeleev organized the elements on the Periodic Table by increasing __________________.

A

atomic mass or weight

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56
Q

The modern Periodic Table has elements arranged in order of increasing atomic mass.
True
False

A

False

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57
Q 
Sodium is a metal that reacts violently when exposed to water.  Which other element do you expect to react violently when exposed to water?
  Magnesium 
  Aluminum 
  Cesium 
  Chlorine
A

Cesium

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58
Q

Phosphorous is located in period 3 and group 15.
True
False

A

True

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59
Q 
Mendeleev organized elements in the Periodic Table by \_\_\_\_\_\_\_\_\_\_\_\_\_\_\_\_\_\_\_\_\_\_\_ while Mosley used \_\_\_\_\_\_\_\_\_\_\_\_\_\_\_\_\_\_\_\_\_\_\_\_\_\_\_.
  Atomic mass, atomic number 
  Atomic mass, atomic radius 
  Atomic number, atomic mass 
  Atomic number, atomic radius
A

Atomic mass, atomic number

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60
Q 
How are elements in a period on the modern Periodic Table arranged?
  By chemical properties 
  By physical properties 
  By increasing number of protons 
  By number of valence electrons
A

By increasing number of protons

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61
Q 
What element is in Period 4 Group 17?
  Chlorine 
  Iodine 
  Actinium 
  Bromine
A

Bromine

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62
Q 
Nitrogen can be found in Period \_\_\_\_\_\_\_\_ and Group \_\_\_\_\_\_\_\_?
  15, 2 
  2, 15 
  2, 7 
  7, 2
A

2, 15

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63
Q 
Groups \_\_\_\_\_\_\_\_ and \_\_\_\_\_\_\_contain elements whose valence electrons are only found in the s block?
  17, 18 
  13, 14 
  1, 2 
  7, 8
A

1, 2

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64
Q 
The properties of elements reoccur periodically, demonstrating periodic trends when the elements are arranged in order of increasing
  reactivity 
  atomic radius 
  atomic mass 
  atomic number
A

atomic number

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65
Q

Even though elements like Na, Li, K, and Ca, Mg, Ba share some similarities, why are they grouped into different families on the Periodic Table?
They have different numbers of protons.
They have different chemical properties
They have different masses.
They were discovered at different times.

A

They have different chemical properties

66
Q 
Argon is a gas at room temperature and has a very stable electron configuration.  Which of the following elements would you expect to be gaseous and stable at room temperature?
  Chlorine 
  Nitrogen 
  Oxygen 
  Neon
A

Neon

67
Q 
What do all members of a group have in common?
  Atomic mass 
  Atomic number 
  Atomic radius 
  Valence electrons
A

Valence electrons

68
Q 
The halogen in Period 5 is \_\_\_\_\_\_\_\_.
  Fluorine 
  Iodine 
  Strontium 
  Xenon
A

Iodine

69
Q 
Which element is the most reactive alkali metal?
  Magnesium 
  Calcium 
  Sodium 
  Potassium
A

Potassium

70
Q 
Which element would be the worst conductor of electricity?
  Boron 
  Aluminum 
  Silicon 
  Phosphorous
A

Phosphorous

71
Q

Nonmetals tend to gain electrons to form negative ions.
True
False

A

True

72
Q 
Which family is most likely to form ions with a +1 charge?
  Alkali metals 
  Alkaline earth metals 
  Halogens 
  Noble gases
A

Alkali metals

73
Q

Why do elements in the same group share the same chemical properties?
They have the same number of protons
The valance electrons are in the same energy level
They have the same number of valence electrons.
They share the same physical properties

A

They have the same number of valence electrons.

74
Q 
Name the alkaline earth metal in period 7.
  Radium 
  Francium 
  Barium 
  Radon
A

Radium

75
Q

Why are noble gases unreactive?
Because of the number of protons in the nucleus.
Because they have a full valence shell of electrons.
Because they are colorless and odorless gases.
Because they need too many valence electrons to have a full shell.

A

Because they have a full valence shell of electrons.

76
Q 
Metals tend to \_\_\_\_\_\_\_\_ electrons to form a \_\_\_\_\_\_\_\_ ion.
  Gain, positive 
  Gain, negative 
  Lose, positive 
  Lose, negative
A

Lose, positive

77
Q 
What are the most reactive metals on the periodic table?
  Transition metals 
  Alkaline earth metals 
  Rare earth metals 
  Alkali metals
A

Alkali metals

78
Q 
What family contains the most chemically active non-metals?
  The oxygen family 
  The carbon family 
  The halogens 
  The Noble gases
A

The halogens

79
Q

Properties

Element J

Color
Gray

Reactivity
Medium-low

Phase of matter at room temperature
Solid

To which family might the element described above belong?

Alkali metals
Transition metals
Halogens
Noble gases

A

Transition metals

80
Q 
Alkali metals tend to form ions with what charge?
  \+1 
  \+2 
  -1 
  -2
A

+1

81
Q 
Nonmetals tend to \_\_\_\_\_\_\_\_\_ electrons and form \_\_\_\_\_\_\_ ions.
  Gain, positive 
  Gain, negative 
  Lose, positive 
  Lose, negative
A

Gain, negative

82
Q 
Halogens tend to form ions with what charge?
  \+1 
  \+2 
  -1 
  -2
A

-1

83
Q

Which atom has a larger radius?
Ca
Se

A

Ca

84
Q

Which atom has a larger radius?
Oxygen
Sulfur

A

Sulfur

85
Q

Put the following elements in order of increasing atomic radius: Li, N, P, Cl

Use commas to separate the elements.

A

Cl, N, P, Li

86
Q

Why does Br have a smaller radius than K even though it has more protons and electrons?
Because Br has fewer electron shells than K.
Because Br has more electron shells than K.
Because Br has a stronger nuclear charge than K
Because Br has a weaker nuclear charge than K.

A

Because Br has a stronger nuclear charge than K

87
Q

Why does electron shielding have very little effect on the size of the radius as you move across a period?
Because the increase in the effective nuclear charge cancels out the effect of shielding.
Because across a period, electrons are in the same shell so they experience very little shielding.

A

Because across a period, electrons are in the same shell so they experience very little shielding.

88
Q

Which group of elements, metals or nonmetals, will tend to form ions that are larger than their parent atom?
Metals
Nonmetals

A

Nonmetals

89
Q

Thinking about the size of the parent atom, which ion do you predict will be larger: Na1+ or K1+?
K1+
Na1+

A

K1+

90
Q 
Which of the following atoms will form an ion that is smaller than its neutral atom?
  S 
  O 
  Li 
  Ne
A

Li

91
Q 
Choose the atom below that will form an ion that is larger than its neutral atom.
  Iron 
  Copper 
  Strontium 
  Phosphorous
A

Phosphorous

92
Q

List the following ions in order of increasing size: Ca2+, Na1+, S2-, Cl1-

Use the names of the elements and commas to complete your answer.

A

Na1+, Ca2+, Cl1-, S2-

93
Q

List the following atoms in order of decreasing electronegativity: Sr, Mg, Ca, Be, Ba

Use the symbol with a comma in between each element to record your answer.

A

Be, Mg, Ca, Sr, Ba

94
Q

Oxygen has a lower electronegativity than nitrogen.
True
False

A

False

95
Q 
Which atom is most likely to attract electrons in a bond?
  Al 
  Si 
  P 
  S
A

S

96
Q

Why is the electronegativity of a noble gas listed as zero?

  • The nuclear charge in the noble gases is so strong they do not attract electrons in a bond.
  • The nuclear charge in the noble gases is so weak they do not attract electrons in a bond.
  • Because noble gases do not typically participate in chemical bonds, they do not attract electrons when bonding.
  • Because noble gases will only attract electrons during a bond with other noble gases.
A

Because noble gases do not typically participate in chemical bonds, they do not attract electrons when bonding.

97
Q

Using a drawing, compare the atomic radius of the following elements. Be sure your drawing ranks them from smallest radius to largest radius.

Potassium

Sodium

Sulfur

Selenium

A

Drawing should show the ranking from smallest to largest:

Sulfur, selenium, sodium, potassium

98
Q

What is the most important factor in determining a trend from left to right across a period?
The strength of the nuclear charge
The number of valence electrons
The strength of the electron shielding
The number of energy levels in the atom

A

The strength of the nuclear charge

99
Q

___________ have low ionization energies because ____________.

  • Alkali metals; they have the weakest effective nuclear charge in a period.
  • Alkaline earth metals; they have highest electronegativities in the period.
  • Halogens; they have the weakest effective nuclear charge in a period.
  • Noble gases; they have the highest electronegativities in the period.
A

Alkali metals; they have the weakest effective nuclear charge in a period.

100
Q

Consider atoms of oxygen and fluorine. Which atom will be the least likely to lose an electron to form an ion and why?

A

Fluorine because it has the stronger nuclear charge.

101
Q

What is the most important factor in determining a trend from top to bottom in a group?
The number of valence electrons
The distance between the valence electrons and the nucleus
The number of neutrons in the nucleus
Whether the group consists of metals or nonmetals

A

The distance between the valence electrons and the nucleus

102
Q

Explain the relationship between the size of an atoms’ radius and its ionization energy as you down a group from Na to Fr. (Hint: use the words increases and/or decreases.)

A

As the radius increases, the ionization energy decreases.

103
Q 
Which atom is most likely to attract electrons in a bond?
  K 
  Na 
  S 
  Se
A

S

104
Q 
Which of the following atoms will form an ion with a radius larger than that of its neutral atom?
  Ca 
  Mg 
  Al 
  O
A

O

105
Q

Explain why cations tend to form ions with radii smaller than their neutral atom.

A

When they lose valence electrons, it increases the effective nuclear charge.

106
Q

In any given period, which family will experience the strongest effective nuclear charge and why?

  • Alkali metals because they have the fewest number of protons.
  • Alkali metals because they have the most number of protons.
  • Halogens because they have the fewest number of protons.
  • Halogens because they have the most number of protons.
A

Halogens because they have the most number of protons.

107
Q 
What is the oxidation number of calcium?
  1+ 
  2+ 
  3+ 
  4+
A

2+

108
Q 
An ion found in some compounds contains 12 protons and 10 electrons. What is its symbol?
  Ne 
  Ne2- 
  Mg2+ 
  Mg+
A

Mg2+

109
Q 
What type of compound is CHCl3, the anesthetic chloroform?
  Ionic 
  Covalent 
  Metallic 
  Basic
A

Covalent

110
Q

Which of the following substances would not conduct electricity in any state?
One in which electrons are delocalised and shared among positive nuclei
One in which electrons are transferred between ions
One in which electrons are shared
One in which electrons are kept and no ions are formed

A

One in which electrons are shared

111
Q 
What type of compound is Fe2O3, and what is its name?
  Covalent, diiron trioxide 
  Acid, ferrous acid 
  Base, iron hydroxide 
  Ionic, iron(III) oxide
A

Ionic, iron(III) oxide

112
Q 
What is the name of the following compound, which contains a polyatomic ion: BeCrO₄?
  Beryllium chromate 
  Beryllium chromium tetraoxide 
  Beryllium oxide 
  Beryllium dichromate
A

Beryllium chromate

113
Q 
What type of compound is CO2?
  Ionic 
  Acid 
  Base 
  Covalent
A

Covalent

114
Q 
What is the name of the following compound, which contains a metal that can exhibit more than one ionic charge: PbCl2?
  Lead(II) Chloride 
  Lead Chloride 
  Lead(I) Chloride 
  Lead Chloride(II)
A

Lead(II) Chloride

115
Q 
What is the name of the following compound, which contains a polyatomic ion: MgSO4?
  Magnesium sulfur oxide 
  Magnesium sulfur tetraoxide 
  Magnesium sulfate 
  Magnesium oxide
A

Magnesium sulfate

116
Q 
What is the name of the following compound: XeF4?
  Monoxenon quadrafluorine 
  Xenon tetrafluorine 
  Monoxenon fluoride 
  Xenon tetrafluoride
A

Xenon tetrafluoride

117
Q 
What is the name of the following compound: HCl?
  Hydrochloric acid 
  Hydrogen chloride 
  Monohydrogen monochloride 
  Hydrogen(I) chloride
A

Hydrochloric acid

118
Q 
What is the name for the following compound: RbOH?
  Monorubidium hydroxide 
  Monorubidium oxygen hydride 
  Rubidium hydroxide 
  Rubidium oxygen hydride
A

Rubidium hydroxide

119
Q 
What type of compound is TiCl4 and what is its name?
  Ionic, titanium(IV) chloride 
  Covalent, titanium tetrachloride 
  Acid, titanium chloric acid 
  Base, titanium chloroxide
A

Ionic, titanium(IV) chloride

120
Q 
How many oxygen atoms are in the correct formula the ionic compound formed by the lithium cation, Li+, and the oxygen anion, O2−?
  1 
  2 
  3 
  4
A

1

121
Q 
How many nitrogen atoms are in the correct formula for the ionic compound calcium nitride?
  1 
  2 
  3 
  4
A

2

122
Q 
How many sodium atoms are in the correct formula for the ionic compound sodium chlorate?
  4 
  3 
  2 
  1
A

1

123
Q 
How many copper atoms are in the correct formula for the compound copper(I) oxide?
  4 
  3 
  2 
  1
A

2

124
Q 
How many hydrogen atoms are in the correct formula for hydrobromic acid?
  4 
  3 
  2 
  1
A

1

125
Q 
How many hydrogen atoms are in the correct formula for carbonic acid?
  1 
  2 
  3 
  4
A

2

126
Q 
How many oxygen atoms are in the correct formula for barium nitrate?
  2 
  3 
  5 
  6
A

6

127
Q 
How many oxygen atoms are in the correct formula for the covalent compound xenon trioxide?
  1 
  2 
  3 
  4
A

3

128
Q 
How many arsenic atoms are in the correct formula for the compound diarsenic pentoxide?
  1 
  2 
  3 
  4
A

2

129
Q 
How many sulfur atoms are in the correct formula for the compound tetraphosphorus heptasulfide?
  4 
  5 
  6 
  7
A

7

130
Q 
How many bromine atoms are in the correct formula for the compound lead(IV) bromide?
  4 
  3 
  2 
  1
A

4

131
Q 
How many hydroxide ions are in the correct formula for the compound calcium hydroxide?
  1 
  2 
  3 
  4
A

2

132
Q 
How many calcium atoms are in the correct formula for calcium phosphide?
  1 
  2 
  3 
  4
A

3

133
Q 
How many calcium atoms are in the correct formula for calcium chloride?
  1 
  2 
  3 
  4
A

1

134
Q 
How many fluorine atoms are in the correct formula for hydrofluoric acid?
  4 
  3 
  2 
  1
A

1

135
Q

Write the formula and determine how many sodium ions are in the correct formula for sodium chlorate.

A

NaClO3

1 sodium ion

136
Q

Write the formula and determine how many oxygen atoms are in the correct formula for iron(II) chlorite.

A

Fe(ClO2)2

4 Oxygen atoms

137
Q 
What is the name of the following compound: K3N?
  Tripotassium nitrogen 
  Potassium nitrate 
  Tripotassium mononitride 
  Potassium nitride
A

Potassium nitride

138
Q 
What is the name of the following compound: Cr(NO3)3?
  Chromium(III) nitrate 
  Chromium trinitrate 
  Chromic acid 
  Chromium nitrate
A

Chromium(III) nitrate

139
Q

What is the name of the following compound: N2O3?

A

Dinitrogen trioxide

140
Q

What is the name of the following compound: Al(OH)3?

A

Aluminum hydroxide

141
Q

What is the name of the following compound: CaCO3?

A

Calcium carbonate

142
Q 
How many electrons are transferred in the following compound: BaO?
  1 
  2 
  3 
  4
A

2

143
Q 
How many electrons are transferred in the following compound: AlCl3?
  1 
  2 
  3 
  4
A

3

144
Q 
How many electrons are transferred in the following compound: Al2S3?
  6 
  5 
  4 
  3
A

6

145
Q 
Which of the following compounds share electrons?
  NaCl 
  CO 
  CsF 
  KBr
A

CO

146
Q 
In the compound CO2, how many lone pairs are on the central atom?
  0 
  1 
  2 
  3
A

0

147
Q 
How many bonded pairs of electrons are there in the molecule NOCl?
  2 
  3 
  4 
  5
A

3

148
Q 
How many bonded pairs of electrons are there in the molecule O2?
  4 
  3 
  2 
  1
A

2

149
Q 
What charge does an arsenic ion exhibit?
  1- 
  2- 
  3- 
  4-
A

3-

150
Q 
What charge does a beryllium ion exhibit?
  1+ 
  2+ 
  3+ 
  4+
A

2+

151
Q 
How many bonded pairs of electrons are there in the molecule HCCH?
  5 
  4 
  3 
  2
A

5

152
Q

How are electrons arranged in metallic bonds?
They are transferred between ions.
They are shared between nonmetals.
They are delocalized and free-floating.
They are held tightly by their nuclei.

A

They are delocalized and free-floating.

153
Q 
Which is not a property of metals?
  Brittle 
  Malleable 
  Ductile 
  Conductive
A

Brittle

154
Q

Why do metals bend and not break?
They are made from positive and negative ions.
They share electrons in discrete bonds.
They have metallic luster.

A

They share electrons in discrete bonds.

155
Q

True or False: Metals are good conductors of heat and electricity.
True
False

A

True

156
Q

True or False: Most metals are found to occur naturally in their uncombined states.
True
False

A

False

157
Q

The ability to be stretched into long wires is a property of metals known as __________________.

A

Ductility

158
Q

True or False: All metals have high melting points.
True
False

A

False

159
Q 
An elemental metal contains how many types of atoms?
  1 
  2 
  3 
  4
A

1

160
Q

What is the shape of the OF2 molecule?

A

Bent

161
Q

Which of the following molecules is paired incorrectly with its shape?
Xenon difluoride – Linear
Methane (carbon tetrahydride) – Tetrahedral
Beryllium chloride – Bent
Boron trifluoride – Trigonal planar

A

Beryllium chloride – Bent

Chemistry (5 decks)

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