Exam #2

Write the formula for copper (II) sulfate pentahydrate.

CuSO4∙5H2O

Choose the ground state electron configuration for Cr3+

[Ar]4s23d1

Give the ground state electron configuration for Sr.

[Kr]5s2

Calculate the molar mass of Al(C2H3O2)3.

204.13 g/mol

Give the name for KMnO4.

potassium permanganate

Calculate the molar mass of Ca3(PO4)2.

310.18 g/mol

A covalent bond is best described as A) the sharing of electrons between atoms. B) the transfer of electrons. C) a bond between a metal and a nonmetal. D) a bond between a metal and a polyatomic ion. E) a bond between two polyatomic ions.

A) the sharing of electrons between atoms.

Give the correct formula for aluminum sulfate.

Al2(SO4)3

Electrons filling up the orbitals from low to high is known as (the)

Aufbau principle.

Which atom in each group (I and II) has the smallest atomic radius? I) Ca, Ti, Br. (II) O, S, Se

Br; O

Write a possible molecular formula for C4H4O.

C24H24O6

Give the formula for sulfurous acid

H2SO3

What is the empirical formula for Hg2(NO3)2

HgNO3

Place the following in order of decreasing metallic character. P As K

K > As > P

An element that has the valence electron configuration 5s25p5 belongs to which period and group?

period 5; group 7A

Give the name for P4O10.

tetraphosphorus decoxide

Identify rubbing alcohol.

(CH3)2CHOH

How many unpaired electrons are present in the ground state Xe atom?

0

How many moles of N2O4 are in 76.3 g N2O4? The molar mass of N2O4 is 92.02 g/mol.

0.829 moles

How many valence electrons do the alkali metals possess?

1

How many atoms of oxygen are contained in 47.6 g of Al2(CO3)3? The molar mass of Al2(CO3)3 is 233.99 g/mol

1.10 × 1024 O atoms

How many molecules of butane are contained in 25.0 mL of butane? The density of butane is 0.6011 g/mL and the molar mass is 58.12 g/mol.

1.56 × 1023 molecules butane

Determine the volume of hexane that contains 5.33 × 1022 molecules of hexane. The density of hexane is 0.6548 g/mL and its molar mass is 86.17 g/mol.

11.6 mL

Determine the number of moles of oxygen in 3.20 moles of sodium hydrogen phosphate.

12.80 moles of oxygen

Calculate the mass percent composition of lithium in Li3PO4.

17.98%

Give the ground state electron configuration for F−.

1s22s22p6

Write a balanced equation to show the reaction of gaseous ethane with gaseous oxygen to form carbon monoxide gas and water vapor.

2 C2H6(g) + 5 O2(g) → 4 CO(g) + 6 H2O(g)

Calculate the mass percent composition of sulfur in Al2(SO4)3.

28.12%

How many unpaired electrons are present in the ground state N atom?

3

How many valence electrons does an atom of Tl possess?

3

How many valence shell electrons does an atom of thallium have?

3

How many atoms of carbon are contained in 47.6 g of Al2(CO3)3? The molar mass of Al2(CO3)3 is 233.99 g/mol.

3.68 × 1023 C atoms

How many molecules of N2O4 are in 76.3 g N2O4? The molar mass of N2O4 is 92.02 g/mol.

4.99 × 1023 N2O4 molecules

Give the number of core electrons for Te.

46

What is the mass (in kg) of 6.89 × 1025 molecules of CO2? The molar mass of CO2 is 44.01 g/mol.

5.04 kg

Determine the number of moles of sodium in 3.20 moles of sodium hydrogen phosphate.

6.40 moles of sodium

The molecular weight of urea ((NH2)2CO), a compound used as a nitrogen fertilizer, is________ amu (rounded to one decimal place).

60.1

Calculate the molar mass of H2CO3

62.03 g/mol

How many millimoles of Ca(NO3)2 contain 4.78 × 1022 formula units of Ca(NO3)2? The molar mass of Ca(NO3)2 is 164.10 g/mol.

79.4 mmol Ca(NO3)2

How many valence electrons do the noble gases possess?

8

How many valence electrons does an atom of Ar possess?

8

How many C2H4 molecules are contained in 45.8 mg of C2H4? The molar mass of C2H4 is 28.05 g/mol.

9.83 × 1020 C2H4 molecules

Choose the statement that is TRUE. A) Outer electrons efficiently shield one another from nuclear charge. B) Core electrons effectively shield outer electrons from nuclear charge. C) Valence electrons are most difficult of all electrons to remove. D) Core electrons are the easiest of all electrons to remove. E) All of the above are true.

B) Core electrons effectively shield outer electrons from nuclear charge.

An ionic bond is best described as A) the sharing of electrons. B) the transfer of electrons from one atom to another. C) the attraction that holds the atoms together in a polyatomic ion. D) the attraction between two nonmetal atoms. E) the attraction between two metal atoms.

B) the transfer of electrons from one atom to another.

Choose the valence orbital diagram that represents the ground state of Sr2+ (look at question 15 page 2)

E)

A cation of +2 indicates that an element has

lost two electrons.

Give the name for SnO.

tin(II) oxide

Write the name for Sn(SO4)2. Remember that Sn forms several ions.

tin(IV) sulfate

Give the name for TiCO3. Remember that titanium forms several ions.

titanium(II) carbonate

Describe the reaction of the alkali metals with non-metals.

vigorous

Which of the following statements is TRUE? A) An orbital that penetrates into the region occupied by core electrons is less shielded from nuclear charge than an orbital that does not penetrate and therefore has a lower energy. B) An orbital that penetrates into the region occupied by core electrons is more shielded from nuclear charge than an orbital that does not penetrate and therefore has a lower energy. C) It is possible for two electrons in the same atom to have identical values for all four quantum numbers. D) Two electrons in the same orbital can have the same spin. E) None of the above is true.

A) An orbital that penetrates into the region occupied by core electrons is less shielded from nuclear charge than an orbital that does not penetrate and therefore has a lower energy.

Write a balanced equation to show the reaction of aqueous aluminum acetate with aqueous ammonium phosphate to form solid aluminum phosphate and aqueous ammonium acetate.

Al(C2H3O2)3(aq) + (NH4)3PO4(aq) → AlPO4(s) + 3 NH4C2H3O2(aq)

Which of the following contains BOTH ionic and covalent bonds? A) BaF2 D) SF6 B) Cl2 C) MgSO4 E) None of the above contains both ionic and covalent bonds.

C) MgSO4

Identify the isoelectronic elements. A) Cl-, F-, Br-, I-, At- B) N3-, S2-, Br-, Cs+, Sr2+ C) P3-, S2-, C1-, K+, Ca2+ D) Zn2+, Co2+, Cu2+, Cr2+, Cd2+ E) Ne, Ar, Kr, Xe, He

C) P3-, S2-, C1-, K+, Ca2+

Identify a characteristic of halogens. A) powerful reducing agents B) forms water in reactions C) powerful oxidizing agents D) absorbs water in reactions E) inert

C) powerful oxidizing agents

What is the empirical formula for C10H20O5?

C2H4O

Determine the empirical formula for a compound that contains C, H and O. It contains 52.14% C and 34.73% O by mass.

C2H6O

Combustion analysis of 63.8 mg of a C, H and O containing compound produced 145.0 mg of CO2 and 59.38 mg of H2O. What is the empirical formula for the compound?

C3H6O

Give a possible molecular formula for the empirical formula of C3H5ClO.

C6H10ClO2

Determine the molecular formula of a compound that has a molar mass of 183.2 g/mol and an empirical formula of C2H5O2.

C6H15O6

Determine the molecular formula of a compound that is 49.48% carbon, 5.19% hydrogen, 28.85% nitrogen, and 16.48% oxygen. The molecular weight is 194.19 g/mol.

C8H10N4O2

Identify the alcohol in fermented drinks.

CH3CH2OH

Identify the compound with covalent bonds.

CH4

Identify the most reactive alkali metal with water.

Cs

Identify the FALSE statement about acid rain. A) Acid rain contains nitric acid and sulfuric acid. B) Acid rain dissolves marble statues C) Acid rain comes from coal-powered electric power plants. D) Acid rain corrodes steel bridges. E) Acid rain comes from hydroelectric power plants.

E) Acid rain comes from hydroelectric power plants.

Write a balanced equation to show the reaction of sulfurous acid with lithium hydroxide to form water and lithium sulfite.

H2SO3(aq) + 2 LiOH(aq) → 2 H2O(l) + Li2SO3(aq)

When filling degenerate orbitals, electrons fill them singly first, with parallel spins. This is known as (the)

Hund's rule

Identify the compound with ionic bonds. A) Ne B) CO C) N2 D) H2O E) KCl

KCl

Place the following in order of increasing atomic radius. Sr Li Ca

Li < Ca < Sr

Which reaction below represents the electron affinity of Li? A) Li(g) + e− → Li−(g) C) Li(g) + e− → Li+(g) B) Li(g) → Li+(g) + e− D) Li+(g) → Li(g) + e− E) Li+(g) + e− → Li(g)

Li(g) + e− → Li−(g)

Determine the empirical formula for a compound that is 36.86% N and 63.14% O by mass.

N2O3

Determine the molecular formula of a compound that has a molar mass of 92.0 g/mol and an empirical formula of NO2.

N2O4

Identify the elements correctly shown by decreasing radii size.

N3- > N

Place the following in order of increasing metallic character. Rb Cs K Na

Na < K < Rb < Cs

Place the following elements in order of increasing atomic radius S Te O

O < S < Te

Determine the empirical formula for a compound that is found to contain 10.15 mg P and 34.85 mg Cl.

PCl3

No two electrons can have the same four quantum numbers is known as (the)

Pauli exclusion principle.

Which reaction below represents the electron affinity of S? A) S(g) + e− → S−(g) C) S(g) → S+(g) + e− B) S−(g) + e− → S2−(g) D) S−(g) → S(g) + e− E) S2−(g) → S−(g) + e−

S(g) + e− → S−(g)

Give the ground state electron configuration for Se.

[Ar]4s23d104p4

Choose the ground state electron configuration for Zn2+.

[Ar]4s23d8

Give the ground state electron configuration for Pb.

[Xe]6s24f145d106p2

Choose the orbital diagram that represents the ground state of N. (look at page 6 number 39)

answer: A

Identify the element that chlorine forms a covalent bond with.

carbon

Give the name for H2CO3.

carbonic acid

For a particular element, identify the species that has the smallest radius.

cation

The element that corresponds to the electron configuration 1s22s22p63s23p64s13d5 is

chromium.

Give the name for CoCl2∙6H2O. Remember that Co forms several ions.

cobalt(II) chloride hexahydrate

Identify the noble gas that is used by researchers to cool down samples for analysis.

helium

Describe the reaction of the noble gases with metals.

inert