chem final

Question 1

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

Answer 1

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.

Question 2

True/ False: H2O is really called dihydrogen monoxide.

Answer 2

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.

Question 3

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

Answer 3

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.

Question 4

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

Answer 4

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.

Question 5

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

Answer 5

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.

Question 6

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

Answer 6

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

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

Question 7

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

Answer 7

True.

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

Question 8

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

Answer 8

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.

Question 9

What do covalent compounds do to fulfill the octet rule?

Answer 9

Covalent compounds share electrons

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

Question 10

True or False: Ionic compounds are usually crystals.

Answer 10

True

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

Question 11

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

Answer 11

True

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

Question 12

What are valence electrons?

Answer 12

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.

Question 13

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

Answer 13

True

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

Question 14

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

Answer 14

False

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

Question 15

What charge does a calcium ion have?

Answer 15

Charge of +2

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

Question 16

True or False: The halogens have 6 valence electrons.

Answer 16

False

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

Question 17

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

Answer 17

True

Transition metals can form both positive and negative ions.

Question 18

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

Answer 18

Nitrogen phosphide

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

Question 19

What is Fe(NO3)3 commonly called?

Answer 19

Iron (III) nitrate

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

Question 20

True/False: AIC is called aluminum chlorite.

Answer 20

False

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

Question 21

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

Answer 21

True

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

Question 22

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

Answer 22

true

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

Question 23

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

Answer 23

False

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

Question 24

True/False: The nucleus has a positive charge.

Answer 24

True

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

Question 25

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

Answer 25

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

Question 26

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

Answer 26

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

Question 27

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

Answer 27

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

Question 28

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

Answer 28

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

Question 29

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

Answer 29

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

Question 30

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

Answer 30

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

Question 31

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

Answer 31

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

Question 32

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

Answer 32

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

Question 33

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

Answer 33

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

Question 34

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

Answer 34

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

Question 35

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

Answer 35

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

Question 36

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

Answer 36

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

Question 37

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

Answer 37

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

Question 38

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

Answer 38

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

Question 39

The mass number for oxygen is _______.

Answer 39

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

Question 40

The atomic mass of oxygen is _______.

Answer 40

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

Question 41

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

Answer 41

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

Question 42

The formula for lead IV oxide is _______.

Answer 42

PbO2 ## Footnote There is one lead atom connected to two oxygen atoms.

Question 43

Magnesium acetate is written as _______.

Answer 43

Mg(C2H302)2 ## Footnote Acetate has 2 carbon, 3 hydrogen, and 2 oxygen.

Question 44

The most common isotope of hydrogen has _______ neutron.

Answer 44

0 | protium ## Footnote 0 nuetrons

Question 45

Carbon-12 is _______.

Answer 45

not radioactive ## Footnote Carbon-12 is stable with a neutron-to-proton ratio of 1:1.

Question 46

Neptunium has _______ neutrons.

Answer 46

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

Question 47

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

Answer 47

False ## Footnote The most common isotope of hydrogen has no neutrons.

Question 48

True/False: Carbon-12 is very radioactive.

Answer 48

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

Question 49

True/False: Neptunium has 145 neutrons.

Answer 49

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

Question 50

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

Answer 50

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

Question 51

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

Answer 51

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

Question 52

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

Answer 52

List of polyatomic ions ## Footnote ammonium, nitrate, nitrite, cyanide, permanganate, hydroxide, carbonate, sulfate, sulfite, phosphate, phosphite, acetate, chlorate, chlorite, hydrogen carbonate.

Question 53

Differentiate between atomic mass and _______.

Answer 53

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

Question 54

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

Answer 54

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

Question 55

Differentiate between electron configurations of atoms versus ______.

Answer 55

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

Question 56

What is required for nomenclature regarding ionic and ______ compounds?

Answer 56

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

Question 57

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

Answer 57

https://www.youtube.com/watch?v=U2cfju6GTNs ## Footnote This link presumably leads to a relevant educational resource.

Question 58

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

Answer 58

least resistance ## Footnote This phrase encourages taking on challenges rather than avoiding them.

Question 59

What is a polyatomic ion?

Answer 59

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

Question 60

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

Answer 60

b) SO4^2- ## Footnote Sulfate

Question 61

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

Answer 61

False

Question 62

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

Answer 62

+1

Question 63

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

Answer 63

Carbonate

Question 64

What is the formula for the sulfate ion?

Answer 64

SO4^2-

Question 65

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

Answer 65

Nitrate

Question 66

Which polyatomic ion contains phosphorus?

Answer 66

Phosphate (PO4^3-)

Question 67

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

Answer 67

True

Question 68

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

Answer 68

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

Question 69

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

Answer 69

Electronegativity

Question 70

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

Answer 70

-3

Question 71

Name a polyatomic ion that contains chlorine.

Answer 71

Chlorate (ClO3-)

Question 72

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

Answer 72

Hydrogen carbonate

Question 73

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

Answer 73

Atomic radius decreases from left to right.

Question 74

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

Answer 74

True

Question 75

What is the formula for the acetate ion?

Answer 75

C2H3O2-

Question 76

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

Answer 76

Sulfate (SO4^2-)

Question 77

What determines the chemical behavior of an atom?

Answer 77

The arrangement of electrons in its atomic structure.

Question 78

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

Answer 78

Ammonium

Question 79

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

Answer 79

Ionization energy generally increases with increasing atomic number.

Question 80

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

Answer 80

False

Question 81

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

Answer 81

-1

Question 82

Name the polyatomic ion with the formula ClO4-.

Answer 82

Perchlorate

Question 83

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

Answer 83

Ionization energy

Question 84

What is the formula for the nitrite ion?

Answer 84

NO2-

Question 85

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

Answer 85

true

Question 86

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

Answer 86

True

Question 87

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

Answer 87

-2

Question 88

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

Answer 88

Periods

Question 89

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

Answer 89

Oxalate

Question 90

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

Answer 90

Atomic structure and electron configuration.

Question 91

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

Answer 91

Hydrogen phosphate

Question 92

What is the formula for the dichromate ion?

Answer 92

Cr2O7^2-

Question 93

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

Answer 93

False

Question 94

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

Answer 94

Electronegativity decreases.

Question 95

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

Answer 95

-1

Question 96

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

Answer 96

Phosphite

Question 97

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

Answer 97

True

Question 98

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

Answer 98

-3

Question 99

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

Answer 99

False ## Footnote SO4^2-

Question 100

What is the formula for the selenate ion?

Answer 100

SeO4^2-

Question 101

Which polyatomic ion has a formula of ClO3-?

Answer 101

Chlorate

Question 102

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

Answer 102

Acetate

Question 103

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

Answer 103

-2