Chemistry 110 Exam 7

The most common sulfur ion has a charge of __________.

-2

Hydrogen is unique among the elements because __________. 1. It is not really a member of any particular group. 2. Its electron is not at all shielded from its nucleus. 3. It is the lightest element. 4. It is the only element to exist at room temperature as a diatomic gas. 5. It exhibits some chemical properties similar to those of groups 1A and 7A.

1, 2, 3, 5

Consider the general valence electron configuration of ns2np5 and the following statements: 1.) Elements with this electron configuration are expected to form -1 anions. 2.) Elements with this electron configuration are expected to have large positive electron affinities. 3.) Elements with this electron configuration are nonmetals. 4.) Elements with this electron configuration form acidic oxides. Which statements are true? A) 1 and 2 B) 1, 2, and 3 C) 2 and 3 D) 1, 3, and 4 E) All statements are true

1, 3, and 4

What is the coefficient of H2O when the following equation is completed and balanced? Ba (s) + H2O (l) → ________

2

What is the coefficient of M when the following equation is completed and balanced if M is an alkali metal? M (s) + H₂O (l) →________

2

Hydrogen is unique among the elements because __________. 1. It has only one valence electron. 2. It is the only element that can emit an atomic spectrum. 3. Its electron is not at all shielded from its nucleus. 4. It is the lightest element. 5. It is the only element to exist at room temperature as a diatomic gas

3, 4

2 F₂ (g) + 2 H₂O (l) → __________.

4 HF (aq) + O₂ (g)

All the elements in group 8A are gases at room temperature. Of all the groups in the periodic table, only group__________ contains examples of elements that are gas, liquid, and solid at room temperature.

7A

Which periodic table group contains only nonmetals __________?

8A

Which one of the following elements has the largest atomic radius? A) O B) F C) Al D) P E) B

Al

Which equation correctly represents the first ionization of aluminum? A) Al- (g) → Al (g) + e- B) Al (g) → Al- (g) + e- C) Al (g) + e- → Al- (g) D) Al (g) → Al+ (g) + e- E) Al+ (g) + e- → Al (g)

Al (g) → Al+ (g) + e-

Which of the following correctly represents the second ionization of aluminum? A) Al+ (g) + e- → Al (g) B) Al (g) → Al+ (g) + e- C) Al- (g) + e- → Al²- (g) D) Al+ (g) + e- → Al²+ (g) E) Al+ (g) → Al²+ (g) + e-

Al+ (g) → Al²+ (g) + e-

Of the choices below, which gives the order for first ionization energies? A) Cl > S > Al > Ar > Si B) Ar > Cl > S > Si > Al C) Al > Si > S > Cl > Ar D) Cl > S > Al > Si > Ar E) S > Si > Cl > Al > Ar

Ar > Cl > S > Si > Al

In which of the following atoms is the 3s orbital closest to the nucleus? A) Br B) Cl C) At D) I E) The 3s orbitals are the same distance from the nucleus in all of these atoms.

At

Element M reacts with oxygen to form an oxide with the formula MO. When MO is dissolved in water, the resulting solution is basic. Element M could be __________.

Ba

Which one of the following atoms has the largest radius? A) I B) Co C) Ba D) Sr E) Ca

Ba

Which alkaline earth metal will not react with liquid water or with steam __________?

Be

This element reacts with hydrogen to produce a gas with the formula HX. When dissolved in water, HX forms an acidic solution. X is __________.

Br

Of the following species, __________ has the largest radius. A) Rb+ B) Sr²+ C) Br- D) Kr E) Ar

Br-

Which ion below has the largest radius? A) Cl- B) K+ C) Br- D) F E) Na+

Br-

Of the following oxides, __________ is the most acidic. A) CaO B) CO₂ C) Al₂O₃ D) Li₂O E) Na₂O

CO₂

Which one of the following compounds would produce an acidic solution when dissolved in water? A) Na₂O B) CaO C) MgO D) CO₂ E) SrO

CO₂

Element X reacts with chlorine to form a compound with the formula XCl2 . The oxide of element X is basic. Element X is __________.

Ca

Of the following elements, which has the largest first ionization energy? A) K B) Rb C) Sr D) Ca E) Ba

Ca

Na reacts with element X to form an ionic compound with the formula Na₃X . Ca will react with X to form __________.

Ca₃X₂

In which of the following atoms is the 2s orbital closest to the nucleus? A) S B) Cl C) P D) Si E) The 2s orbitals are the same distance from the nucleus in all of these atoms.

Cl

Of the following elements, __________ has the most negative electron affinity. A) S B) Cl C) Se D) Br E) I

Cl

Of the following elements, which has the largest first ionization energy? A) Na B) Al C) Se D) Cl E) Br

Cl

Which element would be expected to have chemical and physical properties closest to those of fluorine? A) S B) Fe C) Ne D) O E) Cl

Cl

Which one of the following has the smallest radius? A) Na B) Cl C) Fe D) P E) Br

Cl

Of the following statements, __________ is not true for oxygen. A) The most stable allotrope of oxygen is O₂ . B) The chemical formula of ozone is O₃ . C) Dry air is about 79% oxygen. D) Oxygen forms peroxide and superoxide anions. E) Oxygen is a colorless gas at room temperature.

Dry air is about 79% oxygen.

Of the following elements, __________ has the most negative electron affinity. A) Na B) Li C) Be D) N E) F

F

Which of the following correctly lists the five atoms in order of increasing size (smallest to largest)? A) F < K < Ge < Br < Rb B) F < Ge < Br < K < Rb C) F < K < Br < Ge < Rb D) F < Br < Ge < K < Rb E) F < Br < Ge < Rb < K

F < Br < Ge < K < Rb

Which of the following correctly lists the five atoms in order of increasing size (smallest to largest)? A) O < F < S < Mg < Ba B) F < O < S < Mg < Ba C) F < O < S < Ba < Mg D) O < F < S < Ba < Mg E) F < S < O < Mg < Ba

F < O < S < Mg < Ba

The ion with the smallest diameter is __________. A) Br- B) Cl- C) I- D) F- E) O²-

F-

Of the elements below, __________ has the highest melting point. A) Ca B) K C) Fe D) Na E) Ba

Fe

Which one of the following is a metalloid? A) Ge B) S C) Br D) Pb E) C

Ge

Cl₂ (g) + H₂O (l) → __________.

HCl (aq) + HOCl (aq)

Of the hydrogen halides, only __________ is a weak acid.

HF (aq)

__________ is credited with developing the concept of atomic numbers.

Henry Moseley

The substance, __________ is always produced when an active metal reacts with water.

H₂

Which element is solid at room temperature? A) Cl₂ B) F₂ C) Br₂ D) I₂ E) H₂

I₂

Of the elements below, __________ is the most metallic. A) Na B) Mg C) Al D) K E) Ar

K

Of the compounds below, __________ has the smallest ionic separation. A) KF B) K₂S C) RbCl D) SrBr₂ E) RbF

KF

The reaction of potassium metal with elemental hydrogen produces __________.

KH

Which of these oxides is most basic? A) K₂O B) Al₂O₃ C) CO₂ D) MgO E) Na₂O

K₂O

An alkali metal forms a compound with chlorine with the formula __________. (The symbol M represents any one of the alkali metals.)

MCL

An alkaline earth metal forms a compound with oxygen with the formula __________. (The symbol M represents any one of the alkaline earth metals.)

MO

This element is more reactive than lithium and magnesium but less reactive than potassium. This element is __________.

Na

Which of the following has the largest second ionization energy? A) Si B) Mg C) Al D) Na E) P

Na

Of the following, which gives the correct order for atomic radius for Mg, Na, P, Si and Ar? A) Mg > Na > P > Si > Ar B) Ar > Si > P > Na > Mg C) Si > P > Ar > Na > Mg D) Na > Mg > Si > P > Ar E) Ar > P > Si > Mg > Na

Na > Mg > Si > P > Ar

Electrons in the 1s subshell are much closer to the nucleus in Ar than in He due to the larger __________ in Ar.

Nuclear Charge

Of the following atoms, which has the largest first ionization energy? A) Br B) O C) C D) P E) I

O

In which set of elements would all members be expected to have very similar chemical properties? A) O, S, Se B) N, O, F C) Na, Mg, K D) S, Se, Si E) Ne, Na, Mg

O, S, Se

Which of the following is an isoelectronic series? A) B⁵- , Si⁴- , As³- , Te²- B) F- , Cl- , Br- , I C) S, Cl, Ar, K D) Si²- , P²- , S²- , Cl²- E) O²- , P- , Ne, Na+

O²- , P- , Ne, Na+

Which equation correctly represents the first ionization of phosphorus? A) P (g) + e- → P- (g) B) P (g) → P- (g) + e- C) P (g) → P+ (g) + e- D) P- (g) → P (g) + e- E) P+ (g) + e- → P (g)

P (g) → P+ (g) + e-

Which of the following correctly represents the second ionization of phosphorus? A) P+ (g) + e- → P²+ (g) B) P (g) → P+ (g) + e- C) P- (g) + e- → P²- (g) D) P+ (g) → P² (g) + e- E) P+ (g) + e- → P (g)

P+ (g) → P²+ (g) + e-

Which one of the following atoms has the largest radius? A) Sr B) Ca C) K D) Rb E) Y

Rb

Of the following elements, which has the largest first ionization energy? A) Se B) As C) S D) Sb E) Ge

S

Which one of the following atoms has the largest radius? A) O B) F C) S D) Cl E) Ne

S

Which one of the following elements has the largest atomic radius? A) Se B) As C) S D) Sb E) Te

Sb

The list that correctly indicates the order of metallic character is __________. A) B > N > C B) F > Cl > S C) Si > P > S D) P > S > Se E) Na > K > Rb

Si > P > S

All of the following are ionic compounds except __________. A) K₂O B) Na₂SO₄ C) SiO₂ D) Li₃N E) NaCl

SiO₂

Element M reacts with chlorine to form a compound with the formula MCl₂ . Element M is more reactive than magnesium and has a smaller radius than barium. This element is __________.

Sr

The element(s) __________ could be used to produce a red or crimson color in fireworks.

Sr

The most common and stable allotrope of sulfur is __________.

S₈

Which one of the following is not true about the alkali metals? A) They are low density solids at room temperature. B) They all readily form ions with a +1 charge. C) They all have 2 electrons in their valence shells. D) They are very reactive elements. E) They have the lowest first ionization energies of the elements.

They all have 2 electrons in their valence shells.

Of the following metals, __________ exhibits multiple oxidation states. A) Al B) Cs C) V D) Ca E) Na

V

The first noble gas to be incorporated into a compound was __________.

Xe

The effective nuclear charge, Zeff, is found this way:

Zeff = Z − S, where Z is the atomic number and S is a screening constant, usually close to the number of inner electrons.

When two elements combine to form a compound, the greater the difference in metallic character between the two elements, the greater the likelihood that the compound will be __________.

a solid at room temperature

Which of the following is not a characteristic of metals? A) acidic oxides B) low ionization energies C) malleability D) ductility E) These are all characteristics of metals.

acidic oxides

__________ have the lowest first ionization energies of the groups listed. A) Alkali metals B) Transition elements C) Halogens D) Alkaline earth metals E) Noble gases

alkali metals

Alkali metals tend to be more reactive than alkaline earth metals because __________.

alkali metals have lower ionization energies

The element phosphorus exists in two forms in nature called white phosphorus and red phosphorus. These two forms are examples of __________.

allotropes

Oxides of most nonmetals combine with water to form __________.

an acid

Elements in the modern version of the periodic table are arranged in order of increasing __________.

atomic number

Of the elements below, __________ is the most metallic. A) sodium B) barium C) magnesium D) calcium E) cesium

cesium

Chlorine is much more apt to exist as an anion than is sodium. This is because __________.

chlorine has a greater electron affinity than sodium does

Sodium is much more apt to exist as a cation than is chlorine. This is because __________.

chlorine has a greater ionization energy than sodium does

Ionic size ____________ with an _____________ nuclear charge.

decreases, increasing

In general, as you go across a period in the periodic table from left to right: (1) the atomic radius __________; (2) the electron affinity becomes __________ negative; and (3) the first ionization energy __________.

decreases, increasingly, increases

Atomic radius generally increases as we move __________.

down a group and from right to left across a period

Second ionization energy:

energy required to remove the second electron, etc. (It requires more energy to remove each successive electron.)

Of the halogens, which are gases at room temperature and atmospheric pressure?

fluorine and chlorine

Alkaline earth metals __________.

form basic oxides

All of the halogens __________.

form salts with alkali metals with the formula MX

The __________ have the most negative electron affinities.

halogens

The only noble gas that does not have the ns2np6 valence electron configuration is __________.

helium

__________ is a unique element and does not truly belong to any family.

hydrogen

Ions __________ in size as you go down a column.

increase (due to increasing value of n.)

The first ionization energies of the elements __________ as you go from left to right across a period of the periodic table, and __________ as you go from the bottom to the top of a group in the table.

increase, increase

Which nonmetal exists as a diatomic solid?

iodine

In an isoelectronic series_____________.

ions have the same number of electrons

First ionization energy:

is that energy required to remove the first electron. (generally, as one goes across a row, it gets harder to remove an electron. as you go from left to right, Zeff increases)

Anions are _________ than their parent atoms.

larger (electrons are added and repulsions are increased)

Screening by the valence electrons in atoms is __________.

less efficient than that by core electrons

Electron affinity _____________.

measures how easy an atom gains an electron

In nature, sulfur is most commonly found in __________.

metal sulfides

Most of the elements on the periodic table are __________.

metals

In nature, the noble gases exist as________________.

monatomic gaseous atoms

Screening by core electrons in atoms is __________.

more efficient than that by valence electrons

Effective nuclear charge (Zeff) increases when:

moving across any row on the periodic table left to right (the rows are called periods)

Ionic size depends upon:

nuclear charge, number of electrons, orbitals in which electrons reside.

Which group 6A element is a metal?

polonium

The reaction of a metal with a nonmetal produces a(n) __________.

salt

Cations are __________ than their parent atoms

smaller (the outermost electron is removed and repulsions are reduced.)

Consider the following properties of an element: (i) It is solid at room temperature. (ii) It easily forms an oxide when exposed to air. (iii) When it reacts with water, hydrogen gas evolves. (iv) It must be stored submerged in oil. Which element fits the above description the best? A) sulfur B) copper C) mercury D) sodium E) magnesium

sodium

The oxide of which element below can react with hydrochloric acid?

sodium

Metals can be __________ at room temperature.

solid or liquid

Nonmetals can be __________ at room temperature.

solid, liquid, gas

Xenon has been shown to form compounds only when it is combined with __________.

something with a tremendous ability to remove electrons from other substances

Ionization Energy:

the amount of energy required to remove an electron from the ground state of a gaseous atom or ion.

Which of the following traits characterizes the alkali metals? A) very high melting point B) existence as diatomic molecules C) formation of dianions D) the lowest first ionization energies in a period E) the smallest atomic radius in a period

the lowest first ionization energies in a period

The atomic radius of main-group elements generally increases down a group because __________.

the principal quantum number of the valence orbitals increases

Elements in the same column on the periodic table contain _____________.

the same number of electrons in their valence orbital

Coulomb's law tells us___________.

the strength of the interaction between two electrical charges depends on the magnitude of the charge and the distance between them

Oxides of most nonmetals combine with base to form __________.

water and salt

Oxides of the active metals combine with acid to form __________.

water and salt

The noble gases were, until relatively recently, thought to be entirely unreactive. Experiments in the early 1960s showed that Xe could, in fact, form compounds with fluorine. The formation of compounds consisting of Xe is made possible by __________.

xenon's relatively low ionization energy

Of the following elements, which have been shown to form compounds? helium | neon | argon | krypton | xenon

xenon, krypton, argon