Test 2

How many molecules of N₂O₄ are in 76.3 g N₂O₄? The molar mass of N₂O₄ is 92.02 g/mol. A.) 7.26 x 10²³ N₂O₄ molecules B.) 1.38 x 10²⁴ N₂O₄ molecules C.) 5.54 x 10²⁵ N₂O₄ molecules D.) 4.59 x 10²⁵ N₂O₄ molecules E.) 4.99 x 10²³ N₂O₄ molecules

E

Give the ground state electron configuration for Ag. A.) [Ar]4s23d104p6 B.) [Ar]3d104p4 C.) [Ar]4s24d104p4 D.) [Ar]4s23d10 E.) [Ar]4s23d104p5

E.)

Give the ground state electron configuration for N. A.) 1s22s23s22p2 B.) 1s22s23s23p3 C.) 1s22s23s2 D.) 1s22s22p2 E.) 1s22s22p3

E.)

Give the ground state electron configuration for Sr. A.) [Kr]5s24d105p2 B.) [Kr]5s24d10 C.) [Kr]5s24d2 D.) [Kr]5s25d105p2 E.) [Kr]5s2

E.)

Give the ground state electron configuration for the ion of Ba. A.) [Kr]5s25p6 B.) [Kr]5s24d105p66s2 C.) [Kr]5s24d105p66s1 D.) [Kr]5s24d105p66s26p2 E.) [Kr]5s24d105p6

E.)

Place the following elements in order of increasing atomic radius. P Ba CI A,) Ba<CI<P B.) P<CI<Ba C.) CI<Ba<P D.) Ba<P<CI E.) CI<P<Ba

E.)

Place the following in order of decreasing metallic character. P As K A.) As<K<P B.) As<P<K C.) P<As<K D.) K<P<As E.) K<As<P

E.)

Identify the compound with covalent bonding A.) NaCl B.) K C.) H₂O D.) He E.) S

C

What is the charge on the Fe ions in Fe₂O₃? A.) 3+ B.) 1+ C.) 2- D.) 2+

A

Which ionic compound would be expected to have the highest lattice energy A.) Al Cl₃ B.) CCl₄ C.) NaCl D.) MgCl₂

A

Which of the following elements is a transition element (D group)? A.) Ag B.) U C.) Rg D.) Ar E.) Na

A

Write the formula for magnesium nitrite A.) Mg(NO₂)₂ B.) MgNO₃ C.) Mg(NO₂)₃ D.) Mg₃N₂ E.) MgN

A

Identify the compound with ionic bonds A.) KCL B.) H₂ C.) CO D.) H₂O E.) Ne

A.

Give the ground state election configuration for Br. A.) [Ar]4s23d104p6 B.) [Ar]4s23d104p5 C.) [Ar]4s24p6 D.) [Ar]4s23d104p4 E.) [Ar]4s24d104p6

A.)

Give the number of core electrons for Sr. A.) 36 B.) 54 C.) 18 D.) 28 E.) 38

A.)

How many valence electrons do the halogens posses? A.) 7 B.) 2 C.) 5 D.) 6 E.) 1

A.)

How many valence electrons does an atom of B posses. A.) 3 B.) 2 C.) 1 D.) 5 E.) 8

A.)

No two elements can have the same four quantum numbers is know as the A.) Pauli exclusion principle B.) Hund" s rule C.) Aufbau principle D.) Heisenberg uncertainty principle

A.)

Place the following in order of increasing IE1. N F As A.) As<N<F B.) As<F<N C.) F<N<As D.) N<As<F E.) F<As<N

A.)

In which set do all elements tend to form cations in binary ionic compounds? A.) P, As, Sb B.) S, Cl, Br C.) Ca, Mn, Sn D.) Na, Al, S `

C

What is the empirical formula of Hg₂(NO₃)₂? A.)Hg(NO₃)₂ B.) Hg₂(NO₃)₂ C.) HgNO₃ D.) Hg₂NO₃ E.) Hg₄(NO₃)₄

C

The chemical formula for barium nitride is A.)Ba(NO₂)₂ B.) Ba₃N₂ C.) BaN₂ D.)Ba(NO₃)₂

B

Use Lewis theory to determine the chemical formula for the compound formed between Rb and O. A.) RbO B.) Rb₂O C.) Rb₃O₂ D.) Rb₂O₃ E.) RbO₂

B

Give the ground state electron configuration for Ag. A.) [Kr]5s24d75p2 B.) [Kr]5s14d10 C.) [Kr]5s24d10 D.) [Kr]5s25d65p3 E.) [Kr]5s24d9

B.)

Ifentify the element that has a ground state electronic configuration of [Kr]5s24d5. A.) Mn B.) Tc C.) Ru D.) Ar E.) Nb

B.)

Place the following isoeletronic series in order of increasing radius. F- Na+ Mg+2 A.) F-<Na+<Mg+2 B.) Mg+2<Na+<F- C.) Na+<F-<Mg+2 D.) F-<Mg+2<Na+ E.) Mg+2<F-<Na+

B.)

Predict the charge that a calcium ion would have. A.) 1+ B.) 2+ C.) 2- D.) 3+ E.) 6-

B.)

Which of the following elements is not a metal? A.) Ba B.) Ar C.) Pb D.) Mg E.) Ga

B.)

Calculate the mass percent composition of sulfur in Al₂(SO₄)₃. A.) 9.372% B.) 42.73% C.) 28.12% D.) 35.97% E.) 21.38%

C

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. A.) 3.68 x 10²³ O atoms B.) 1.23 x 10²³ O atoms C.) 1.10 x 10²⁴ O atoms D.) 2.87 x 10²⁵ O atoms E.) 2.96 x 10²⁴ O atoms

C

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

C.)

Give the number of valence electrons for Sr. A.) 6 B.) 12 C.) 2 D.) 10 E.) 8

C.)

How many electrons does the Se2-ion posses? A.) 32 B.) 34 C.) 36 D.) 8 E.) 4

C.)

Place the following in order of increasing atomic radius. C O N A.) N<O<C B.) C<N<O C.) O<N<C D.) N<C<O E.) O<C<N

C.)

Which element has the chemical symbol, N? A.) nickel B.) nobelium C.) nitrogen D.) niobium

C.)

Which reaction below represents the second electron affinity of 5. A.) S(g) --->S+(g)+e- B.) S2(g)+e- --> S-(g)+e- C.) S-(g) + e- --> S2-(g) D.) S-(g) +e- --> S(g) +e- E.) S(g) + e - --> S-(g)

C.)

An ionic bond is best described as A.) the sharing of electrons B.) the attraction between 2 metal atoms C.) the attraction that holds the atoms together in a polyatomic ion D.) the transfer of electrons from one atom to another. E.) the attraction between 2 nonmetal atoms.

D

Which of the following represent the Lewis structure for Mg?

D

Which of the following represents the Lewis structure for S²⁻?

D

Identify a cation. A.) an atom that has lost a neutron. B.) an atom that has gained an electron C.) an atom that has gained a proton. D.) an atom that has lost an electron

D.)

Which of the following elements is a metal? A.) Ge B.) N C.) I D.) Sn E.) Ne

D.)

Which of the following elements is an actinide? A.) Ar B.) Na C.) Rg D.) U E.) Ce

D.)

Which of the following statements is false? A.) Sulfur is a main group element B.) Noble gases do not usually from ions C.) Halogens are very reactive elements D.) Alalki earth metals generlly do not react with halogens E.) Zn is a transition metal

D.)