Chem 152 test 2 review

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The __________ quantum number defines the shape of an orbital.

D) azimuthal

There are __________ orbitals in the third shell.

C) 9

The __________ subshell contains only one orbital.

C) 4s

There are __________ orbitals in the second shell.

C) 4

The n = 1 shell contains __________ p orbitals. All the other shells contain __________ p orbitals.

B) 0,3

The lowest energy shell that contains f orbitals is the shell with n = __________.

C) 4

The principal quantum number of the first d subshell is __________.

C) 3

__________-orbitals are spherically symmetrical.

A) s

How many p-orbitals are occupied in a Ne atom __________?

D) 2

Each p-subshell can accommodate a maximum of __________ electrons.

A) 6

How many quantum numbers are necessary to designate a particular electron in an atom __________?

B) 4

[AR]4s²3d¹⁰4p³ is the electron configuration of a(n) __________ atom.

A) As

The electron configuration of Ag atom is __________.

B) [Kr]5s¹4D¹⁰

The electron configuration for Zn is __________.

B) [Ar]4s²3D¹⁰

There are __________ unpaired electrons in a phosphorus atom.

D) 3

There are __________ unpaired electrons in a fluorine atom.

B) 1

In a manganese atoms, the __________ subshell is partially filled.

D) 3d

What is the correct electron configuration for molybdenum __________?

C) [Kr]5s¹4d⁵

All of the __________ have a valence shell electron configuration ns¹.

D) alkali metals

The largest principal quantum number in the electron configuration of iodine is __________.

C) 5

The largest principal quantum number in the electron configuration of barium is __________.

E) 6

The largest principal quantum number in the electron configuration of cobalt is __________.

C) 4

Elements in group __________ have a np⁶ electron configuration in the outer shell.

D) 8A

Which group in the periodic table contains elements with the valence electron configuration of ns²np¹ __________?

C) 3A

At maximum, an f-subshell can hold __________ electrons, a d-subshell can hold __________ electrons, and a p-subshell can hold __________ electrons.

A) 14, 10, 6

Which electron configuration represents a violation of the Pauli exclusion principle?

C) [↑↓] [↑↑] [↑]

Which one of the following is the correct electron configuration for a nitrogen atom?

D) [↑↓] [↑↓] [↑][↑][↑]

The electron configuration of the element __________ is [Kr]5s14d5.

B) Mo

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

B) atomic mass

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.

B) increase, decrease

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

D) Ra

Metals can be __________ at room temperature.

C) solid or liquid

Most of the elements on the periodic table are __________.

E) metals

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

D) Ca₃x₂

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

A) MO

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

D) MCl

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

B) Ca

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

B) salt

Which nonmetal exists as a diatomic solid?

D) iodine

Which group 6A element is a metal?

E) polonium

The most common sulfur ion has a charge of __________.

A) -2

Which periodic table group contains only nonmetals __________?

A) 8A

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.

C) 7A

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

E) fluorine and chlorine

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

C) helium

In which set of elements would all members be expected to have very similar chemical properties?

A) O, S, Se

Which element would be expected to have chemical and physical properties closest to those of fluorine?

E) Cl

Atomic radius generally increases as we move __________.

A) down a group and from right to left across a period

Of the following, which gives the correct order for atomic radius for Mg, Na, P, Si and Ar?

D) Na > Mg > Si > P > Ar

Which one of the following atoms has the largest radius?

D) Rb

Which one of the following has the smallest radius?

B) Cl

Which of the following correctly lists the five atoms in order of increasing size (smallest to largest)?

B) F < O < S < Mg < Ba

Of the choices below, which gives the order for ionization energies?

B) Ar > Cl > S > Si > Al

Of the following atoms, which has the largest ionization energy?

B) O

__________ have the lowest ionization energies of the groups listed.

A) Alkali metals

Which ion below has the largest radius?

C) Br⁻

The ion with the smallest diameter is __________.

D) F⁻

Of the following species, __________ has the largest radius

C) Br⁻

Which of the following is an isoelectronic (same number of electrons) series?

E) O²⁻ F, Ne, Na⁺

Which series is correctly arranged in order of increasing radius?

D. Ca2+ < K+< Ar < Cl-

Of the elements below, __________ is the most metallic

E) cesium

Which one of the following is a metalloid?

A) Ge

The list that correctly indicates the order of metallic character is __________.

C) Si > P > S

Nonmetals can be __________ at room temperature.

A) solid, liquid, or gas

Between which two elements is the difference in metallic character the greatest?

A) Rb and O

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

A) Na

All of the following are ionic compounds except __________.

C) SiO₂

Which element is solid at room temperature?

D) I₂

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

C) Hydrogen

Hydrogen is unique among the elements because __________.

A) 1, 2, 3, 5

There are __________ paired and __________ unpaired electrons in the Lewis symbol for a phosphorus atom.

C) 2, 3

In the Lewis symbol for a fluorine atom, there are __________ paired and __________ unpaired electrons.

D) 6, 1

Magnesium is most likely forms a __________ ion.

A) Mg²⁺

Phosphorus most likely forms a __________ ion.

B) P³⁻

How many unpaired electrons are there in the Lewis structures of a N³ ion?

A) 0

The halogens, alkali metals, and alkaline earth metals have __________ valence electrons, respectively.

D) 7, 1, and 2

The only noble gas without eight valence electrons is __________.

C) He

Which of the following would have to lose two electrons in order to achieve a noble gas electron
configuration __________?

B) Sr

Which of the following would have to gain two electrons in order to achieve a noble gas electron
configuration __________?

D) O, Se

The formula of palladium(IV) sulfide is __________.

D) PdS₂

Elements from opposite sides of the periodic table tend to form __________.

B) ionic compounds

A __________ covalent bond between the same two atoms is the longest.

A) single

A double bond consists of __________ pairs of electrons shared between two atoms.

B) 2

The ability of an atom in a molecule to attract electrons is best quantified by the __________.

C) electronegativity

Electronegativity __________ from left to right within a period and __________ from top to bottom within a group.

C) increases, decreases

Of the ions below, only __________ has a noble gas electron configuration

E) Cl⁻

Which of the following has eight valence electrons?

E) all of the above

Which of the following does not have eight valence electrons?

A) Ca⁺

The type of compound that is most likely to contain a covalent bond is __________.

C) one that is composed of only nonmetals

Of the bonds C-N, C=N, and C≡N, the C-N bond is __________.

D) weakest/longest

In the periodic table, the rows are called __________ and the columns are called __________.

C) periods, groups

Which group in the periodic table contains only nonmetals?

E) 8A

The element __________ is the most similar to strontium in chemical and physical properties

D) Ba

Elements in Group 1A are known as the __________.

C) alkali metals

Elements in Group 2A are known as the __________.

A) alkaline earth metals

Elements in Group 7A are known as the __________.

D) halogens

Elements in Group 8A are known as the __________.

E) noble gases

Potassium is a __________ and chlorine is a __________.

A) metal, nonmetal

When a metal and a nonmetal react, the __________ tends to lose electrons and the __________ tends to gain electrons

C) metal, nonmetal

What is the formula of the compound formed between strontium ions and nitrogen ions?

B) Sr₃N₂

Magnesium reacts with a certain element to form a compound with the general formula MgX. What would the most likely formula be for the compound formed between potassium and element X?

A) K₂X

The formula of a salt is XCl₂. The X-ion in this salt has 28 electrons. The metal X is __________.

A) Ni

The charge on the manganese in the salt is __________.

E) +3

Aluminum reacts with a certain nonmetallic element to form a compound with the general formula AlX. Element X is a diatomic gas at room temperature. Element X must be __________.

D) nitrogen

Predict the formula of the ionic compound that forms from sodium and fluorine.

A) NaF

Predict the formula of the ionic compound that forms from magnesium and fluorine.

E) MgF₂

The correct name for SrO is __________.

A) strontium oxide

The correct name for K₂S is __________.

D) potassium sulfide

The correct name for CaH₂ is __________.

E) calcium hydride

The correct name for SO is __________.

B) sulfur monoxide

The correct name for CCl₄ is __________.

D) carbon tetrachloride

The correct name for H₂CO₃ iS __________.

C) carbonic acid

The correct name for H₂SO₃ is __________.

B) sulfurous acid

The correct name for HCIO₃ is __________.

D) chlorous acid

The correct name for Na₃N is __________.

A) sodium nitride

The correct formula for molybdenum(IV) hypochlorite is __________.

B) Mo(C10)₄

The ions Ca²⁺ and PO₄³⁻ form a salt with the formula __________.

E) Ca₃(PO₄)₂

The correct formula of iron(III) bromide is __________.

B) FeBr₃

The formula of ammonium carbonate is __________.

A) (NH₄)₂CO₃

What is the correct formula for ammonium sulfide?

C) (NH₄)₂S

Chromium and chlorine form an ionic compound whose formula is CrCl₃. The name of this compound is _.

B) chromium(III) chloride

The name of the binary compound N₂O₄ is __________.

A) nitrogen oxide

The name of the ionic compound KBrO₄ is __________.

B) potassium bromate

The name of the ionic compound V₂O₃ is __________.

A) Vanadium (III) oxide

The name of the ionic compound NH₄CN is __________.

C) ammonium cyanide

The correct name for HIO₂ is __________.

D) iodous acid

Which one of the following does not occur as diatomic molecules in elemental form?

C) sulfur

Which formula/name pair is incorrect?

D) magnesium nitrite

Which formula/name pair is incorrect?

E) Fe₂(SO₄)₃

The suffix -ide is used __________.

A) for monoatomic anion names

Which one of the following compounds is chromium(III) oxide?

A) Cr₂O₃

Which one of the following compounds is copper(I) chloride?

A) CuCl

Which one of the following polyatomic ions has the same charge as the hydroxide ion?

C) nitrate

The formula for the compound formed between aluminum ions and phosphate ions is __________.

A) Al₃(PO₄)₃

Which metal does not form cations of differing charges?

A) Na

Which metal forms cations of variable charges?

E) Sn

The correct name for Ni(CN)₂ is __________.

D) Nickel (II) cyanide

Which metal does not require to have its charge specified in the names of ionic compounds it forms?

D) Ca

When the following equation is balanced, the coefficients are: NH₃(g) + O₂(g)→NO₂(g) + H₂O(g)

B) 4, 7, 4, 6

When the following equation is balanced, the coefficients are: Al(NO₃) + Na₂S→ Al₂S₃ + NaNO₃

A) 2, 3, 1, 6

When the following equation is balanced, the coefficient of H₂ is: K(s) + H₂O(L) → KOH (aq)+H₂(g)

A) 1

When the following equation is balanced, the coefficient of Al is: Al(s)+H₂O(L)→Al(OH)₃(s)+h₂(g)

B) 2

the following equation is balanced, the coefficient of H₂O is: Ca(s)+H₂O(L)→Ca(OH)₂(aq)+H₂(g)

B) 2

When the following equation is balanced, the coefficient of HCl is:

B) 2

When the following equation is balanced, the coefficient of HNO₃ is:

B) 2

When the following equation is balanced, the coefficient of H₃PO₄ is:

A) 1

When the following equation is balanced, the coefficient of O₂ is: C₂H₄O(g)+O₂(g)→CO₂(g)+H₂O(g)

D) 5

When the following equation is balanced, the coefficient of H₂SO₄ is: H₂SO₄(aq)+NaOH(aq)→Na₂SO₄(aq)+H₂O(L)

A) 1

When the following equation is balanced, the coefficient of nitric acid is: N₂O₅(g)+H₂O(L)→HNO₃(aq)

B) 2

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