Deck 15: How Atoms Bond and Molecules Attract

Question 1

What is the valence shell?

A)It is the outermost shell of electrons in an atom.
B)It is the shell of electrons in an atom that is the least reactive.
C)It is the last partially filled orbital in an atom.
D)It is the shell of electrons in element V (atomic no. = 23)
E)It is the same as the orbital configuration.

Answer 1

A

Question 2

How many valence electrons does gallium (Ga, atomic no. = 31)have?

A)1
B)6
C)3
D)31
E)70

Answer 2

C

Question 3

What is one role of unpaired valance electrons?

A)They take part in the formation of different types of bonds.
B)They keep the paired electrons separated to minimize interaction.
C)They are the nonbonding electrons.
D)They provide the number of Lewis dots.
E)They tell us which Lewis dot structure is correct.

Answer 3

A

Question 4

An atom loses an electron to another atom. Is this an example of a physical or chemical change?

A)physical change involving the formation of negative ions
B)chemical change involving the formation of neutral atoms
C)physical change involving the formation of positive ions
D)chemical change involving the formation of ions

Question 5

How many more electrons can fit within the valence shell of a hydrogen atom?

A)1
B)2
C)7
D)0

Question 6

How do the electron-dot structures of elements in the same group in the periodic table compare with one another?

A)The structures differ by exactly two electrons between vertically consecutive elements.
B)The number of valence shell electrons increases by one for each element from the top to the bottom of the group.
C)Elements of the same group have the same number of valence electrons.
D)The number of electrons in the electron-dot-structure will equal the group number for each element of the group.

Question 7

How is it possible for a neutral molecule, such as water, to form an ion?

A)It can combine with a hydrogen ion to form a positively charged species.
B)It can combine with a chloride ion to form a negatively charged species.
C)It can fragment into protons and electrons.
D)It can absorb electrons and become negatively charged.
E)It can absorb electrons and become positively charged.

Question 8

How is the number of unpaired valence electrons in an atom related to the number of bonds that the atom can form?

A)There is no defined relationship between the number of unpaired valence electrons and number of bonds that the atom can form.
B)The number of unpaired valence electrons in an atom is one-half the number of bonds that the atom can form.
C)The number of unpaired valence electrons in an atom is twice the number of bonds that the atom can form.
D)The number of unpaired valence electrons in an atom is the same as the number of bonds that the atom can form.

Question 9

If carbonic acid (H₂CO₃)were to undergo ionization, what would one of the products be?

A)H^-
B)CO₂
C)H₂O
D)CO₃^-1
E)CO₃^-2

Question 10

How many valence electrons does bromine (Br, atomic no. = 35)have?

A)1
B)7
C)21
D)28
E)35

Question 11

Which of the following elements has six valence electrons?

A)Be
B)B
C)C
D)N
E)O

Question 12

Which of the following is the correct electron dot structure for carbon (atomic no. = 6)?

A)a
B)b
C)c
D)d
E)e

Question 13

The concept of a chemical bond is ________.

A)how two or more atoms are held together
B)the sharing of nucleons
C)how two or more electrons reside in an orbital
D)how much energy it takes to remove an electron from a set of atoms
E)none of the above

Question 14

Many of the macroscopic properties of a compound depend on ________.

A)how the atoms of the molecules are held together
B)the mass of the constituent atoms
C)the number of nucleons present in the sample
D)the size of the sample
E)how the atoms absorb light and the shape of the orbitals

Question 15

How many valence electrons does boron (B, atomic no. = 5)have?

A)1
B)2
C)3
D)4
E)5

Question 16

Which of the following is the correct electron dot structure for chlorine (atomic no. = 17)?

A)a
B)b
C)c
D)d
E)e

Question 17

Which of the following has the greatest number of nonbonding pairs of electrons ?

A)C
B)H
C)He
D)F
E)S

Question 18

What is the name for the following polyatomic ion? CH₃CO₂^-1

A)acetate
B)monocarboxylate
C)carboxylic
D)acidic
E)acetic

Question 19

Why is it so easy for a magnesium atom to lose two electrons?

A)The nuclear charge of the magnesium atoms is relatively weak.
B)These two electrons are found relatively far from the nucleus.
C)These two electrons are well shielded from the nuclear charge.
D)There are lots of electron-electron repulsions that go on within the valence shell.

Question 20

Which of the following elements has two valence electrons?

A)Na
B)Mg
C)H
D)Ne
E)Li

Question 21

What needs to be done to convert a neutral nitrogen atom into an N^-3 species?

A)add three electrons
B)remove three electrons
C)remove three protons
D)add three protons
E)add three nitrogens

Question 22

Which should be larger, the potassium atom, K, or the potassium ion, K⁺?

A)The potassium ion, K⁺ is larger since charging an atom always makes it larger.
B)The potassium atom, K, with an additional shell of electrons is larger.
C)The potassium ion, K⁺ is larger since it has an extra electron which increases its size.
D)The potassium atom and the potassium ion are exactly the same size and only differ in charge.

Question 23

The neon atom tends NOT to gain any additional electrons because

A)its nuclear charge is not great enough.
B)that would result in a positive ion.
C)of the repulsions they would experience with electrons in the same shell.
D)there is no more room available in its outermost occupied shell.

Question 24

If a neutral atom gains two electrons, what is the electrical charge of the atom?

A)-1
B)+1
C)-2
D)+2
E)neutral

Question 25

Which of the following elements will most likely form an ion with a +1 charge?

A)Na
B)Mg
C)Al
D)Si
E)Cl

Question 26

Why doesn't the sodium atom gain seven electrons so that its third shell becomes the filled outermost shell?

A)It would be too difficult for another atom to lose seven electrons.
B)Only six additional electrons are required to fill the outermost shell of sodium.
C)In gaining seven more electrons, sodium's fourth outer shell becomes filled.
D)Sodium's nuclear charge is not strong enough to hold that many more electrons.

Question 27

Which of the following would be an ion with a double positive charge?

A)an Mg atom that gains two electrons
B)an Mg atom that gains one electron
C)an Mg atom that loses two electrons
D)an Mg atom that loses one electron
E)none of the above

Question 28

Which of the following is a positive ion?

A)Na⁺¹
B)Ca⁺²
C)Mg⁺²
D)Al⁺³
E)all of the above

Question 29

Which of the following elements will most likely not form an ion at all?

A)Na
B)O
C)Ar
D)Mg
E)Br

Question 30

Which of the following elements will most likely form an ion with a -2 charge?

A)Na
B)S
C)Ne
D)Mg
E)Cl

Question 31

Which of the following would be a negative ion with a single charge?

A)an atom with 11 protons and 12 electrons
B)an atom with 11 protons and 11 electrons
C)an atom with 12 protons and 11 electrons
D)an atom with 10 protons and 12 electrons
E)none of the above

Question 32

What is the name for the following polyatomic ion? PO₄^-3

A)phosphate
B)phosphorus oxide
C)phosphinate
D)trioxo phosphoride
E)potassium

Question 33

Which of the following elements will most likely form an ion with a +2 charge?

A)Na
B)Mg
C)Ne
D)Si
E)Cl

Question 34

Which of the following is NOT an ion?

A)H⁺¹
B)Br^-
C)O₂
D)Mg⁺²
E)NO₃^-

Question 35

Which of the following is an ion?

A)2 H₂
B)Br₂
C)HCl
D)Au + 3 Br₂
E)none of the above

Question 36

Which of the following is a negative ion?

A)Na⁺¹
B)Na
C)O^-2
D)O
E)all of the above

Question 37

If a neutral atom loses one electron, what is the electrical charge of the atom?

A)-1
B)+1
C)-2
D)+2
E)neutral

Question 38

Which of the following elements will most likely form an ion with a -1 charge?

A)Na
B)S
C)Ne
D)Mg
E)Cl

Question 39

Why does an atom with many valence electrons tend to gain electrons rather than lose any?

A)Atoms with many valence electrons tend to have relatively weak forces of attraction between the valence electrons and the nucleus. Therefore, the outer electrons are free to attract other electrons.
B)There is stability in numbers. Atoms with many valence electrons are always attracting new electrons.
C)The old adage that "he who has, gets" is also true in atomic structure. Atoms with many valence electrons can essentially overpower atoms with few valence electrons and attract additional electrons.
D)Atoms with many valence electrons tend to have relatively strong forces of attraction between the valence electrons and the nucleus. This makes it easy for them to gain additional electrons.

Question 40

The neon atom tends NOT to lose any electrons because

A)of its relatively strong effective nuclear charge.
B)that would result in a negative ion.
C)its electrons are paired together within the same orbitals.
D)the ionization energy is so high.

Question 41

Is an ionic compound an example of a chemical compound, or is a chemical compound an example of an ionic compound?

A)An chemical compound is an example of a ionic compound.
B)Neither is an example of the other.
C)Each is an example of the other.
D)An ionic compound is an example of a chemical compound.

Question 42

If the following generic atom were to undergo ionization, what would be the charge of the most likely product?

A)+2
B)-2
C)-6
D)+6
E)would probably not ionize

Question 43

What is the compound that forms if you react potassium and sulfur?

A)K₂S
B)KS
C)SP
D)PS₂
E)SkP

Question 44

How many oxide ions (O^-2)are needed to balance the positive charge of a titanium ion (Ti⁺⁴)?

A)2
B)1
C)3
D)4
E)6

Question 45

Which of the following compounds contains ionic bonds?

A)CH₄
B)K₂O
C)Cl₂
D)OF₂
E)none of the above

Question 46

Which are closer together: the two nuclei within potassium fluoride, KF, or the two nuclei within molecular fluorine, F₂?

A)KF
B)F₂
C)Both are the same. Any atom bonded to F will have the same inter-nuclear separation.
D)It makes little sense to compare two molecules which exist in different physical states. KF is a solid while F₂ is a gas.

Question 47

Which of the following substances contains F^- ions?

A)PF₃
B)F₂
C)CF₄
D)CaF₂
E)all of the above

Question 48

Which would you expect to have a higher melting point: sodium chloride, NaCl, or aluminum oxide, Al₂O₃?

A)The aluminum oxide has a higher melting point because it is a larger molecule and has a greater number of molecular interactions.
B)NaCl has a higher melting point because it is a solid at room temperature.
C)The aluminum oxide has a higher melting point because of the greater charges of the ions, and hence the greater force of attractions between them.
D)The aluminum oxide has a higher melting point because of the covalent bonds within the molecule.

Question 49

Magnesium ions carry a 2+ charge, and chloride ions carry a 1- charge. What is the chemical formula for the ionic compound magnesium chloride?

A)MgCl
B)M_g2Cl
C)MgCl₂
D)M_g2Cl₂

Question 50

Which of the following best describes ionic bonding?

A)two atoms sharing a set of electrons
B)two atoms exchanging a set of electrons
C)one atom giving up some of its electrons to another atom
D)when two elements with same charge are held together by electrostatic forces
E)none of the above

Question 51

If the following generic atom were to undergo ionization, what would be the charge of most likely product?

A)+3
B)-3
C)-5
D)8
E)would probably not ionize

Question 52

Which of the following molecules contains an ionic bond?

A)MgCl₂
B)Cl₂
C)SF₃
D)PO₄^-3
E)none of the above

Question 53

Which of the following does not describe ionic compounds?

A)They have a tendency to melt easily.
B)They consist of positive and negative ions.
C)They are held together by electrostatic attraction.
D)They are usually very ordered.
E)none of the above

Question 54

What molecule loses a proton to form the hydroxide ion, OH⁻?

A)The oxygen molecule, O₂
B)The water molecule, H₂O
C)The hydrogen peroxide molecule, H₂O₂
D)The hydrogen molecule, H₂

Question 55

If the following generic atom were to undergo ionization, what would the most likely product be?

A)+1
B)-2
C)-3
D)+4
E)would probably not ionize

Question 56

Take money away from your bank account and the bank will show a negative credit. Take an electron away from an atom, however, and the atom shows up positive. Explain.

A)Electrons are already negative. Therefore, we know from basic math that subtracting a negative (number)from a neutral (atom), will make the result positive.
B)Neutral atoms contain identically charged but oppositely signed protons and electrons. Removing one of the negative electrons results in an excess of positively charged protons.
C)Removing an electron from an atom does not have the atom show up positive. It simply leaves the atom short one electron.
D)Atoms are constantly exchanging electrons. Having an atom "show up positive" is only an expression indicating that it has taken its turn in the game of electron exchange.

Question 57

If you mix a typical iodine ion (I, atomic no. = 53)with a typical barium ion (Ba, atomic no. = 56), what compound is formed?

A)BaI₂
B)BaI
C)Ba₅₆I₅₃
D)Ba₂I
E)Ba₂I₂

Question 58

If you mix a typical aluminum ion (Al, atomic no. = 13)with a typical oxygen ion (O, atomic no. = 8), what compound is formed?

A)Al₂O₃
B)Al₃O₂
C)Al₁₃O₈
D)Al₃O
E)Al₂O₂

Question 59

Barium ions carry a 2+ charge, and nitrogen ions carry a 3-charge. What would be the chemical formula for the ionic compound barium nitride?

A)Ba₃N₂
B)Ba₂N₃
C)Ba₃N₄
D)Ba₂N₂

Question 60

How many chloride ions (Cl^-1)are needed to balance the positive charge of a barium ion (Ba⁺²)?

A)2
B)1
C)-2
D)-1
E)3

Question 61

What does the line in the following example actually represent? H-H

A)a shared pair of electrons
B)a covalent bond
C)an ionic bond
D)a pair of nonbonding electrons
E)A and B

Question 62

There is more gold in 1 km³ of the ocean than the amount of gold mined in all of recorded history. How come we do not mine the oceans?

A)It is too dilute to separate.
B)It would take too much energy.
C)It would cost too much.
D)all of the above
E)none of the above

Question 63

Metals are useful for the structural support of buildings because they

A)do not conduct heat well
B)are shiny
C)conduct electricity
D)are strong but can be bent
E)c and d

Question 64

How many covalent bonds would the following atom usually form?

A)1
B)2
C)4
D)6
E)It would tend to form ionic bonds.

Question 65

Distinguish between a metal and a metal-containing compound.

A)There is no distinction between the two.
B)Only one of these contains ionic bonds.
C)Only one of these contains covalent bonds.
D)Only one of these occurs naturally.

Question 66

How many nonbonding pairs of electrons are in the following molecule? H-H

A)1 pair
B)6 pairs
C)0 pairs
D)8 pairs
E)none of the above

Question 67

Metals are often used for making designer jewelry because they

A)do not conduct heat well
B)conduct electricity
C)are shiny
D)are strong but can be bent
E)c and d

Question 68

What it the main difference between an ionic and a covalent bond?

A)One is the sharing of a pair of electrons, the other is the transfer of at least one electron.
B)One involves electrons, the other does not involve any electrons.
C)The electrons in both types of bonding undergo an exchange.
D)The electrons are traded between the two atoms and this keeps the atoms close.
E)Both bonds are the same, but named different to describe different atoms involved.

Question 69

What property of metal atoms account for many of the observed bulk phenomena seen in metal samples?

A)Metal atoms easily lose one or more outer electrons.
B)Metal atoms easily gain one or more outer electrons.
C)Metals readily form ionic bonds.
D)Metals readily form covalent bonds.
E)none of the above

Question 70

Why is metal shiny?

A)The loose electrons reflect most wavelengths of light.
B)The electrons transmit most wavelengths of light.
C)The electrons absorb each light wave.
D)The electrons emit light due to electronic excitation.
E)all of the above

Question 71

If the concentration of gold in seawater is 2.0 milligram per ton of sea water and the mass of the ocean is 1.5 × 10¹⁸ tons, how much gold is in the ocean?

A)3.0 × 10¹² kg
B)3.0 kg
C)300 g
D)36 mg
E)3,000 lb

Question 72

Why is it better to recycle metals than to mine more?

A)It takes far less energy to recycle.
B)Mining is less expensive than recycling but not environmentally friendly.
C)Ores contain toxic elements.
D)all of the above
E)none of the above

Question 73

What is a molecule?

A)a group of atoms that are held together by covalent bonds
B)a group of atoms that are held together by ionic bonds
C)pair of atoms sharing a set of valence electrons
D)pair of shared valence electrons
E)group of covalent compounds held together by ionic bonds

Question 74

What property of alloys make them ideal for developing new materials?

A)The characteristics of the material change depending on how much of each component is present.
B)Alloys are very rigid and are extremely resistant to chemical decomposition.
C)The size of the atoms involved is directly related the electrical conductivity.
D)all of the above
E)none of the above

Question 75

Which would you expect to have a higher melting point: sodium chloride, NaCl, or cesium chloride, CsCl? Why?

A)The cesium chloride has a higher melting point because larger ions of the same charge are able to attract more ions of the opposite charge.
B)The cesium chloride has a higher melting point because its ions are smaller, which makes the charges more dense.
C)The sodium chloride has a higher melting point because of the greater charges of the ions, and hence the greater force of attractions between them.
D)The sodium chloride has a higher melting point because its ions are smaller, which allows oppositely charged ions to get closer.

Question 76

MgCl₂ crystals are composed of

A)units of MgCl₂ molecules held together by dipole interactions.
B)groups of Mg²⁺ ions and Cl₂ molecules.
C)units composed of six Mg atoms and six Cl₂ molecules.
D)a multitude of Mg²⁺ ions and ions grouped together in a three-dimensional array with a 1:2 ratio of Mg²⁺ to .
E)a two-dimensional array of [-Mg-Cl-Cl-] units.

Question 77

Which of the following is not a property of metal?

A)does not conduct heat well
B)conducts electricity
C)is shiny
D)is strong, but can be bent
E)All of the above are properties of metals.

Question 78

Given that the total number of atoms on our planet remains fairly constant, how is it ever possible to deplete a natural resource such as a metal?

A)The problem remains that not everyone recycles as they should.
B)Recycling only forestalls the inevitable depletion of metal resources.
C)The atoms don't leave our planet, which is why naturally occurring materials never really reach the point of depletion.
D)The problem is with the expense of collecting metal atoms that are uniformly dispersed.

Question 79

Which of the following describes how a metal atoms behaves in a bulk metallic object?

A)The metal ion shares its outermost electrons freely with its neighbors.
B)The metal atoms have limited interaction with neighboring atoms.
C)The metal atom shares its electrons in a very directional manner.
D)The metal atom shares its electrons with only one other atom.
E)none of the above

Question 80

Why are ores so valuable?

A)They are sources of naturally occurring gold.
B)Metals can be efficiently extracted from them.
C)They tend to occur in scenic mountainous regions.
D)They hold many clues to Earth's natural history.