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chem final Flashcards

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1
Q

True/ False: Atomic mass and mass number are the same.

A

False: Atomic mass and mass are not the same.

Mass number is the sum of the protons and neutrons for a specific isotope of an element and is represented by a whole number since protons and neutrons are counted. The mass number is obtained for an element by rounding off the atomic mass to the nearest whole number. Atomic mass is the weighted average of the isotopes for all the isotopes of an element based on their relative abundance and is most often represented by a decimal number.

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2
Q

True/ False: H2O is really called dihydrogen monoxide.

A

True.

This is true because the prefixes used such as di- added to hydrogen means there are 2 hydrogen atoms and mono- added to oxide means there is 1 atom.

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3
Q

True/ False: When naming ionic compounds, you never change the spelling of the anion if it is a nonmetal.

A

False: When naming ionic compounds, you change the spelling of the anion if it is a nonmetal.

You always change the end of a nonmetal when naming an ionic compound; some examples are -ide, -ite, and -ate.

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4
Q

True/ False: When naming covalent compounds, the spelling of metals are never changed.

A

True: The spelling of metals is not changed.

The metals or the cation always stay the same name + ion added to the end, for example, potassium ion.

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5
Q

True/ False: The electron configuration of a selenide ion is 1s² 2s² 2p⁶ 3s² 3p⁶.

A

False: The electron configuration of a selenide ion is 1s² 2s² 2p⁶ 3s² 3p⁶ 3d¹⁰ 4p⁶.

Selenide is located in the 4th period meaning if the end of the electron configuration were 4p⁶ it would end up in the third period.

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6
Q

True/ False: Sodium and lithium can combine to form a covalent compound.

A

False: Sodium and lithium cannot combine to form a covalent compound.

This is false because two metals cannot form to create an ionic compound.

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7
Q

True/ False: Ionic bonding is the result of an electrostatic attraction between a positive and negative ion.

A

True.

This is true because the positive and negative ions create a strong bond forming the ionic bond.

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8
Q

True/ False: Covalent compounds share electrons to fulfill the octet rule.

A

True.

This is true because unlike ionic compounds that give the electrons to fulfill the octet rule, covalent compounds share the electrons within each other to fulfill the rule.

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9
Q

What do covalent compounds do to fulfill the octet rule?

A

Covalent compounds share electrons

Unlike ionic compounds that transfer electrons, covalent compounds share electrons within each other.

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10
Q

True or False: Ionic compounds are usually crystals.

A

True

Ionic compounds have high melting points, an example being salt which melts at 1474 degrees.

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11
Q

True or False: In contrast to ionic compounds, covalent compounds usually have a lower melting point.

A

True

Covalent compounds have weaker attractions and often exist as fluids compared to the stronger attractions in ionic compounds.

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12
Q

What are valence electrons?

A

Electrons in the outer s and p sublevels that are available for bonding

These sublevels typically involve electrons that are most commonly used in bonding.

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13
Q

True or False: Nitrogen will obtain 3 electrons to obey the octet rule.

A

True

Nitrogen is in group 5A and requires 3 electrons to complete its octet.

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14
Q

True or False: Helium has 8 valence electrons just like the other noble gases.

A

False

Helium has only 2 valence electrons because it contains one outer energy level.

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15
Q

What charge does a calcium ion have?

A

Charge of +2

Calcium is a metal that gives away two valence electrons to fulfill the octet rule.

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16
Q

True or False: The halogens have 6 valence electrons.

A

False

Halogens contain 7 valence electrons as they are in group 7A.

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17
Q

True or False: The transition metals often are capable of forming two or more ions with differing charges.

A

True

Transition metals can form both positive and negative ions.

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18
Q

What is the name of the compound represented by the formula NP?

A

Nitrogen phosphide

If the formula were N2P4, it would be named di-nitrogen tetra-phosphide.

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19
Q

What is Fe(NO3)3 commonly called?

A

Iron (III) nitrate

Iron has more than one oxidation number, which is why it is specified as (III) in the name.

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20
Q

True/False: AIC is called aluminum chlorite.

A

False

AIC should be called aluminum chloride, as the correct suffix is chloride and not chlorite.

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21
Q

True/False: Elements in group 6A form -2 ions.

A

True

Nonmetals in group 6A gain 2 electrons to obey the octet rule.

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22
Q

True/False: Any halide ion has an electron configuration ending in …s2p5.

A

true

Halide ions are nonmetals that gain electrons, resulting in an electron configuration ending in …s2p5.

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23
Q

True/False: Almost all the mass of an atom is contained within the electron cloud.

A

False

The nucleus contains most of the mass of an atom, significantly outweighing the electron cloud.

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24
Q

True/False: The nucleus has a positive charge.

A

True

The positive charge of the nucleus balances the negative charge of the electron cloud.

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25
Q

True/False: Ionization energy increases as you go up the periodic table because shielding decreases in that direction.

A

False

Shielding does not affect ionization energy when moving up the periodic table.

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26
Q

True/False: Atomic radius increases as you go down the periodic table and as you move to the left.

A

True

Atomic radius increases due to the increase in electron shells as you move down and to the left.

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27
Q

True/False: Ionization energy increases as you move to the right on the periodic table because of shielding or an increase in energy levels.

A

False

Ionization energy increases due to the increase in nuclear charge as you move to the right.

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28
Q

True or False: Ionization energy increases as you move to the right on the periodic table.

A

True

Ionization energy increases due to the increase in nuclear charge, which causes the outermost electron to be more strongly bonded to the nucleus.

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29
Q

True or False: All the noble gases have 2 electrons in their outer s orbital and 6 electrons in the outer p orbital.

A

True

This configuration allows noble gases to obey the octet rule with a total of 8 electrons.

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30
Q

True or False: Atomic mass is a weighted average of the known isotopes for an element.

A

True

Each isotope has a different mass, and the atomic mass reflects the weighted average of these isotopes.

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31
Q

True or False: The mass of an electron is about equal to the mass of a proton or neutron.

A

False

The mass of an electron is about 1/2000 the mass of a proton or neutron.

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32
Q

True or False: Metals form cations and nonmetals form anions.

A

True

Metals lose electrons to form cations, while nonmetals gain electrons to form anions.

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33
Q

True or False: Nitrogen forms a nitride ion with a 3- charge.

A

True

Nitrogen gains 3 extra electrons, resulting in an overall negative charge.

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34
Q

True or False: The alpha decay of uranium-234 is written as 234 U - 232 Rn + * He.

A

False

The correct notation for alpha decay of uranium-234 is 231 U - 230 Rn + 4 He.

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35
Q

True or False: The beta decay of carbon-14 is written as C6 → 14N7 + e.

A

True

In beta decay, the mass number remains the same while the atomic number increases by one.

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36
Q

True or False: Alpha decay results in the atomic number decreasing by four and the mass number decreasing by 2.

A

False

Alpha decay results in the atomic number decreasing by 2 and the mass number decreasing by 4.

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37
Q

True or False: A nucleus goes through decay to become more stable if the neutron/proton ratio exceeds a value of 1.

A

True

A neutron/proton ratio greater than 1 indicates instability, prompting decay to achieve stability.

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38
Q

Of the four types of nuclear radiation, _______ decay is the most harmful.

A

gamma

This is because gamma decay can harm the human body while beta decay does not harm the human body.

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39
Q

The mass number for oxygen is _______.

A

16

Oxygen has 8 protons and 8 neutrons, adding up to the mass number of 16.

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40
Q

The atomic mass of oxygen is _______.

A

16

Oxygen has 8 protons and 8 neutrons, adding up to the atomic mass of 16.

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41
Q

There are _______ significant figures in the following data: 1.05050000 kilometers.

A

8

The significant figures of 1.05050000 kilometers include all digits except the leading zero after the decimal.

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42
Q

The formula for lead IV oxide is _______.

A

PbO2

There is one lead atom connected to two oxygen atoms.

43
Q

Magnesium acetate is written as _______.

A

Mg(C2H302)2

Acetate has 2 carbon, 3 hydrogen, and 2 oxygen.

44
Q

The most common isotope of hydrogen has _______ neutron.

A

0

protium

0 nuetrons

45
Q

Carbon-12 is _______.

A

not radioactive

Carbon-12 is stable with a neutron-to-proton ratio of 1:1.

46
Q

Neptunium has _______ neutrons.

A

144

Neutrons are calculated by subtracting the atomic number from the atomic mass: 237 - 93 = 144.

47
Q

True/False: The most common isotope of hydrogen has 1 neutron.

A

False

The most common isotope of hydrogen has no neutrons.

48
Q

True/False: Carbon-12 is very radioactive.

A

False

Carbon-12 is stable and not radioactive due to its 1:1 neutron to proton ratio.

49
Q

True/False: Neptunium has 145 neutrons.

A

False

Neptunium has 144 neutrons, calculated by subtracting its atomic number from its mass number (237 - 93 = 144).

50
Q

True/False: Emitted gamma radiation does not affect the mass of the nucleus if it is given off during nuclear decay.

A

True

Gamma radiation does not change the mass of the nucleus when emitted.

51
Q

True/False: Calcium has a greater ionization energy and a greater atomic radius than potassium, rubidium, and strontium.

A

False

Potassium, rubidium, and strontium have larger atomic radii than calcium, although calcium has a greater ionization energy.

52
Q

What are the 15 polyatomic ions you need to memorize for the final?

A

List of polyatomic ions

ammonium, nitrate, nitrite, cyanide, permanganate, hydroxide, carbonate, sulfate, sulfite, phosphate, phosphite, acetate, chlorate, chlorite, hydrogen carbonate.

53
Q

Differentiate between atomic mass and _______.

A

mass number

Atomic mass is the weighted average of isotopes, while mass number is the total number of protons and neutrons.

54
Q

Explain the differences between ______, beta, and gamma radiation.

A

alpha radiation

Alpha particles consist of 2 protons and 2 neutrons, beta particles are high-energy electrons or positrons, and gamma radiation is electromagnetic radiation.

55
Q

Differentiate between electron configurations of atoms versus ______.

A

ions

Ions have different electron configurations due to the loss or gain of electrons.

56
Q

What is required for nomenclature regarding ionic and ______ compounds?

A

covalent

ionic compounds require a metal and nonmetal while covalent compounds require two nonmetals.

57
Q

Recite the following without the aid of music or notes: ______.

A

https://www.youtube.com/watch?v=U2cfju6GTNs

This link presumably leads to a relevant educational resource.

58
Q

Complete the phrase: Don’t be like water and choose the path of ______.

A

least resistance

This phrase encourages taking on challenges rather than avoiding them.

59
Q

What is a polyatomic ion?

A

A polyatomic ion is a charged species composed of two or more atoms covalently bonded together.

60
Q

Which of the following is a common polyatomic ion? (a) Na+, (b) SO4^2-, (c) Cl-

A

b) SO4^2-

Sulfate

61
Q

True or False: All polyatomic ions carry a negative charge.

A

False

62
Q

What is the charge of the ammonium ion (NH4+)?

A

+1

63
Q

Name the polyatomic ion with the formula CO3^2-.

A

Carbonate

64
Q

What is the formula for the sulfate ion?

A

SO4^2-

65
Q

Fill in the blank: The polyatomic ion _______ has the formula NO3-.

A

Nitrate

66
Q

Which polyatomic ion contains phosphorus?

A

Phosphate (PO4^3-)

67
Q

True or False: The hydroxide ion (OH-) is a polyatomic ion.

A

True

68
Q

What is the relationship between atomic structure and the periodic table?

A

Atomic structure determines the arrangement of elements in the periodic table based on their atomic number and properties.

69
Q

Which trend in the periodic table generally increases from left to right?

A

Electronegativity

70
Q

What is the charge of the phosphate ion (PO4^3-)?

A

-3

71
Q

Name a polyatomic ion that contains chlorine.

A

Chlorate (ClO3-)

72
Q

Fill in the blank: The polyatomic ion _______ is known as bicarbonate.

A

Hydrogen carbonate

73
Q

How does atomic radius change across a period in the periodic table?

A

Atomic radius decreases from left to right.

74
Q

True or False: The nitrate ion (NO3-) has a single negative charge.

A

True

75
Q

What is the formula for the acetate ion?

A

C2H3O2-

76
Q

Which polyatomic ion has a formula that includes a sulfur atom and has a charge of -2?

A

Sulfate (SO4^2-)

77
Q

What determines the chemical behavior of an atom?

A

The arrangement of electrons in its atomic structure.

78
Q

Fill in the blank: The polyatomic ion _______ is used in fertilizers and has the formula NH4+.

A

Ammonium

79
Q

What is the effect of increasing atomic number on ionization energy?

A

Ionization energy generally increases with increasing atomic number.

80
Q

True or False: The carbonate ion (CO3^2-) is a monatomic ion.

A

False

81
Q

What is the charge of the permanganate ion (MnO4-)?

A

-1

82
Q

Name the polyatomic ion with the formula ClO4-.

A

Perchlorate

83
Q

Which trend in the periodic table generally decreases as you move down a group?

A

Ionization energy

84
Q

What is the formula for the nitrite ion?

A

NO2-

85
Q

True or False: (CrO4^2-) is known as chromate.

A

true

86
Q

True or False: Elements in the same group of the periodic table have similar chemical properties.

A

True

87
Q

What is the charge of the thiosulfate ion (S2O3^2-)?

A

-2

88
Q

What do you call the horizontal rows in the periodic table?

A

Periods

89
Q

Fill in the blank: The polyatomic ion _______ has a formula of C2O4^2-.

A

Oxalate

90
Q

What is the primary factor that influences the trends in the periodic table?

A

Atomic structure and electron configuration.

91
Q

Which polyatomic ion is represented by the formula HPO4^2-?

A

Hydrogen phosphate

92
Q

What is the formula for the dichromate ion?

A

Cr2O7^2-

93
Q

True or False: Polyatomic ions can be formed from metals only.

A

False

94
Q

How does electronegativity generally change down a group in the periodic table?

A

Electronegativity decreases.

95
Q

What is the charge of the cyanide ion (CN-)?

A

-1

96
Q

Name the polyatomic ion with the formula PO3^3-.

A

Phosphite

97
Q

True or False: (CLO-) is known as hypochlorite.

A

True

98
Q

What is the charge of the borate ion (BO3^3-)?

A

-3

99
Q

True or False: The formula for the sulfate ion is SO3^2-.

A

False

SO4^2-

100
Q

What is the formula for the selenate ion?

A

SeO4^2-

101
Q

Which polyatomic ion has a formula of ClO3-?

A

Chlorate

102
Q

Fill in the blank: The _______ ion (C2H3CO-) is commonly found in vinegar.

A

Acetate

103
Q

What is the charge of the oxalate ion (C2O4^2-)?

A

-2

chemistry final (1 decks)

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