Chem test chapter 8 Flashcards


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1

1.

“Each electron in an atom must have its own unique set of quantum numbers” is a statement of

A) the aufbau principle.

D) the periodic law.

B) the Pauli exclusion principle.

E) Heisenberg's principle.

C) Hund's rule.

B

2

2.

Energy states of atoms containing more than one electron arise from nucleus-electron and electron-electron interactions. Which of the following statements correctly describes these effects?

A)

Larger nuclear charge lowers energy, more electrons in an orbital lowers energy.

B)

Larger nuclear charge lowers energy, more electrons in an orbital increases energy.

C)

Smaller nuclear charge lowers energy, more electrons in an orbital lowers energy.

D)

Smaller nuclear charge lowers energy, more electrons in an orbital increases energy.

E)

None of the above statements is generally correct.

B

3

3.

Which one of the following statements about orbital energies is incorrect?

A)

In the hydrogen atom, the energy of an orbital depends only on the value of the quantum number n.

B)

In many-electron atoms the energy of an orbital depends on both n and l.

C)

Inner electrons shield outer electrons more effectively than do electrons in the same orbital.

D)

The splitting of sublevels in many-electron atoms is explained in terms of the penetration effect.

E)

The energy of a given orbital increases as the nuclear charge Z increases.

E

4

4.

The effective nuclear charge for an atom is less than the actual nuclear charge due to

A) shielding.

D) electron-pair repulsion.

B) penetration.

E) relativity.

C) paramagnetism.

A

5

5.

In many-electron atoms, which quantum numbers specify the energy of an electron?

A) n and l B) n and ml C) l and ml D) n and ms E) n, l, and ml

A

6

6.

Which of the following sublevels is filled last? 3d, 4s, 4p, 4d, 5s

A) 3d B) 4s C) 4p D) 4d E) 5s

D

7

7.

“Electrons added to atomic orbitals of the same energy will remain unpaired with parallel spins until the subshell is more than half-filled” is a statement of

A) the aufbau principle.

D) the periodic law.

B) Hund's rule.

E) the singularity rule.

C) the Pauli exclusion principle.

B

8

8.

Which one of the following statements about atomic structure and quantum numbers is incorrect?

A)

In a given atom, the maximum number of electrons having principal quantum number n = 3, is 18.

B)

The number of orbitals in a given f subshell is 7.

C)

For n = 4, the largest possible value of l is 3.

D)

For n = 4, the largest possible value of ml is 2.

E)

The following set of quantum numbers for a single orbital is not allowed: n = 3, l = 1, ml = –2.

D

9

9.

In a single atom, what is the maximum number of electrons which can have quantum number n = 4?

A) 16 B) 18 C) 32 D) 36 E) none of the above

C

10

10.

Select the correct set of quantum numbers (n, l, ml, ms) for the highest energy electron in the ground state of potassium, K.

A) 4, 1, –1,

B) 4, 1, 0,

C) 4, 0, 1,

D) 4, 0, 0,

E) 4, 1, 1,

D

11

11.

Select the correct set of quantum numbers (n, l, ml, ms) for the highest energy electron in the ground state of tin, Sn.

A) 5, 2, –1,

B) 5, 2, 0,

C) 5, 1, 2,

D) 5, 1, 0,

E) 5, 2, 1,

D

12

12.

Select the correct set of quantum numbers (n, l, ml, ms) for the first electron removed in the formation of a cation for strontium, Sr.

A) 5, 1 , 0, –

D) 5, 1, 1,

B) 5, 1, 0,

E) 5, 0, 0, –

C) 5, 0, 1,

E

13

13.

Which of the following electron configurations is impossible?

A) 1s 22s22p 63s 23p 4

D) 1s 22s 22p 63s 33p 4

B) 1s 22s 22p 53s 13p 4

E) 1s 12s 22p 63s 23p 4

C) 1s 22s 22p 63s 23p 63d104s 2

D

14

14.

Select the correct electron configuration for sulfur (Z = 16).

A) 1s 21p 62s 22p 6

D) 1s 22s 22p 63s 23p 4

B) 1s 22s 22p 83s 23p 4

E)1s 22s 22p 63s 23d 4

C) 1s 22s 22p 83s 23p 2

D

15

15.

Select the correct electron configuration for Cu (Z = 29).

A) [Ar]4s 23d 9

D) [Ar]4s 24d 9

B) [Ar]4s 13d 10

E) [Ar]5s 24d 9

C) [Ar]4s 24p 63d 3

B

16

16.

Select the correct electron configuration for Te (Z = 52).

A) [Kr]5s 25p 64d 8

D) [Kr]5s 24f 14

B) [Kr]5s 25d 105p 4

E) [Kr]5s 24d 105p 4

C) [Kr]5s 24d 105p 6

E

17

17.

The electronic structure 1s 22s 22p 63s 23p 64s 23d 8 refers to the ground state of

A) Kr. B) Ni. C) Fe. D) Pd. E) none of the above.

B

18

18.

In the ground state of an atom of silver (Ag), how many electrons will there be with the quantum number l = 1? (The n, ml, and ms quantum numbers may have any appropriate values.)

A) 9 B) 12 C) 18 D) 24 E) 36

C

19

19.

An atom of element number 33 (As) is in its ground electronic state. Which one of the following sets quantum numbers could not apply to any of its electrons?

A)

n = 2 l = 1 ml = –1 ms = +

B)

n = 3 l = 0 ml = 0 ms = –

C)

n = 3 l = 2 ml = –2 ms = –

D)

n = 4 l = 0 ml = 0 ms = –

E)

n = 4 l = 2 ml = 1 ms = +

E

20

20.

How many valence electrons are there in an atom with the electron configuration [noble gas]ns 2(n – 1)d 10 np 3?

A) 2 B) 3 C) 5 D) 10 E) 15

C

21

21.

How many valence electrons are there in an atom with the electron configuration [noble gas]ns 2(n – 1)d 8?

A) 2 B) 6 C) 8 D) 10 E) none of the above

D

22

22.

Which of the following electron configurations represents the ground state of an element?

A) [Ne]3s 13p 1

D) [Ne]3s 23p 33d 1

B) [He]2s 12p 3

E) [Ne]3s 23p 3

C) [Ne]3s 23p 23d 1

E

23

23.

Which of the following sets of elements have the [noble gas]ns 2 np 2 valence electron configuration?

A) O, S, Se, Te, Po

D) C, Si, Ge, Sn, Pb

B) N, P, As, Sb, Bi

E) Ti, Zr, Hf

C) F, Cl, Br, I, At

D

24

24.

In the electron configuration [Ar]4s 23d 104p 4, which are valence electrons?

A) all of the electrons after the [Ar]

D) only the 4p 4 electrons

B) only the 4s 2 electrons

E) both the 4s 2 and the 4p 4 electrons

C) only the 3d 10 electrons

E

25

25.

Which of the following electron configurations is correct for the excited state of an element?

A) [He]2s 22p 5

B) [Ne]3s 23p 1

C) [Ar]4s 14p 1

D) [Kr]5s 24d 7

E) [He]1p 1

C

26

26.

Which of the following electron configurations is not possible for an atom in an excited state?

A) 1s 22s 22p 63s 23p 63d 104s 14p 1

D) 1s 22s 22p 63s 23p 63d 104s 2

B) 1s 22s 22p 63s 13p 5

E) 1s 22s 22p 63s 23p 63d 104s 14 p 3

C) 1s 22s 22p 63s 23p 23d 2

D

27

27.

Which of the following fourth-period elements has the smallest atomic radius?

A) K B) Ti C) Cu D) Ge E) Kr

E

28

28.

Which of the following elements has the largest atomic size?

A) S B) Ca C) Ba D) Po E) Rn

C

29

29.

Which of the following elements has the smallest atomic size?

A) Na B) Ar C) K D) Ca E) Kr

B

30

30.

Which of the following elements has the smallest atomic radius?

A) Li B) Ne C) Rb D) Sr E) Xe

B

31

31.

Which of the following elements has the greatest atomic radius?

A) Li B) Ne C) Rb D) Sr E) Xe

C

32

32.

Which one of the following equations correctly represents the process relating to the ionization energy of X?

A) X(s) ® X+(g) + e

D) X(g) ® X(g) + e

B) X2(g) ® X+(g) + X(g)

E) X(g) ® X+(g) + e

C) X(g) + e® X(g)

E

33

33.

Which of the following elements has the largest first ionization energy?

A) Na B) Cl C) Ca D) Te E) Br

B

34

34.

Which of the following elements has the smallest first ionization energy?

A) Rb B) Mg C) I D) As E) F

A

35

35.

When comparing the successive ionization energies of an element, an unusually big increase in ionization energy is seen when

A)

the first valence electron is removed.

B)

the second valence electron is removed.

C)

the eighth electron of is removed.

D)

the first core electron is removed.

E)

the last valence electron is removed.

D

36

36.

Identify the element of Period 2 which has the following successive ionization energies, in kJ/mol.

IE1, 1314 IE2, 3389 IE3, 5298 IE4, 7471

IE5, 10992 IE6, 13329 IE7, 71345 IE8, 84087

A) Li B) B C) O D) Ne E) none of the above

C

37

37.

Which of the following elements has the largest second ionization energy (IE2)?

A) Li B) B C) O D) F E) Na

A

38

38.

Elements with the highest first ionization energies are found in the ___________ region of the periodic table.

A) lower left B) upper left C) center D) lower right E) upper right

E

39

39.

Which one of the following equations correctly represents the process involved in the electron affinity of X?

A) X(g) ® X+(g) + e

D) X(g) + e® X(g)

B) X+(g) ® X+(aq)

E) X+(g) + Y(g) ® XY(s)

C) X+(g) + e® X(g)

D

40

40.

Select the element with the most negative electron affinity (i.e., accepts an electron most readily).

A) H B) Li C) C D) F E) Ne

D

41

41.

Which of the following has the most negative electron affinity?

A) H B) Li C) Na D) K E) Rb

A

42

42.

Elements with ________________ first ionization energies and ___________ electron affinities generally form cations.

A)

low, very negative

B)

high, positive or slightly negative

C)

low, positive or slightly negative

D)

high, very negative

E)

None of the above is generally correct.

C

43

43.

Elements with _______________ first ionization energies and ___________ electron affinities generally form anions.

A)

low, very negative

B)

high, positive or slightly negative

C)

low, positive or slightly negative

D)

high, very negative

E)

None of the above is generally correct.

D

44

44.

Select the element with the greatest metallic character.

A) Li B) Ca C) Al D) Pb E) Cs

E

45

45.

Select the element with the least metallic character.

A) Sn B) Sr C) Tl D) Ge E) Ga

D

46

46.

Metallic behavior is generally associated with

A)

elements with very negative electron affinities.

B)

elements with low ionization energies.

C)

elements with small atomic radii.

D)

elements with unpaired electrons.

E)

elements with partially filled p orbitals.

B

47

47.

The most acidic oxides are formed from elements found in the _________________ region of the periodic table.

A) upper right B) upper left C) center D) lower right E) lower left

A

48

48.

The most basic oxides are formed from elements found in the __________________ region of the periodic table.

A) upper right B) upper left C) center D) lower right E) lower left

E

49

49.

Select the most acidic compound from the following:

A) SO2 B) Al2O3 C) CaO D) PbO E) H2O

A

50

50.

Select the most basic compound from the following:

A) Bi2O3 B) SiO2 C) Cs2O D) Na2O E) H2O

C

51

51.

Which of the following elements will form a cation with a +2 charge?

A) Si B) Sr C) Ga D) Cs E) S

B

52

52.

Which of the following ions will be most likely to form when selenium ionizes?

A) Se6+ B) Se4+ C) Se2+ D) Se2– E) Se4–

D

53

53.

Which of the following atoms will be diamagnetic?

A) Cr B) Ru C) Fe D) Pt E) Cd

E

54

54.

Which of the following elements is paramagnetic?

A) Kr B) Zn C) Sr D) V E) Ar

D

55

55.

Select the paramagnetic ion.

A) Cu+ B) Ag+ C) Fe3+ D) Cd2+ E) Ca2+

C

56

56.

Select the diamagnetic ion.

A) Cu2+ B) Ni2+ C) Cr3+ D) Sc3+ E) Cr2+

D

57

57.

Consider the set of isoelectronic atoms and ions A2–, B, C, D+, and E2+. Which arrangement of relative radii is correct?

A) A2– > B> C > D+ > E2+

D) A2– < B < C > D+ > E2+

B) E2+ > D+ > C > B > A2–

E) None of the above is correct.

C) A2– > B > C < D+ < E2+

A

58

58.

What is the correct order of decreasing size of the following ions?

A) P3– > Cl> K+ > Ca2+

D) K+ > Cl > P3– > Ca2+

B) Ca2+ > K+ > Cl > P3–

E) None of the above is correct.

C) K+ > Cl> Ca2+ > P3–

A