1. Identify the shell and subshell of an orbital with the quantum numbers n=3,l=1 and ml=1.

Shell Subshell

A. 3 3s

B. 3 3p

C. 3 3d

D. 2 2p

2.Give the possible combinations of quantum numbers for a 4p orbital.

n l ml MsA 4 -1 1 -1/2B 4 1 -2 -1/2C 4 0 0 +1/2D 4 1 -1 +1/2

3.What is similar about 3p and 4p sublevels?

A. Both are spherical

B. Both contain three p orbitals

C. Both are part of third energy levels

D.All have lobes and belong in the third energy level

4. Indicate the maximum number of electrons in principal energy lvel n=4?

A.16 B.32

C.44 D.54

5.Indicate the number of orbitals in the energy level n=3?

A.3 B.6

C.9 D.12

6.Which of the following orbital cannot exist?

2p 3p 4d 3f 6s 2d

A 3f and 2d B 3f and 2p

C 4d and 6s D 2p and 2d

7.According to the afbau principle, which orbital is filled immediately after each of the following in a multielectrom atom?

Before AfterA 4s 4dB 5f 6sC 3d 4pD 5p 5d

8. Write the symbol for the group 6A element in the fourth period.

A.Se B.Te

C.W D.Mo

9.Which of the following is electronic configuration for Ru?

A. 1s2,2s2,2p6,3s2,3p6,4s2,3d10,4p6

B. 1s2,2s2,2p6,3s2,3p6,4s2,3d10,4p6,5s2

C. 1s2,2s2,2p6,3s2,3p6,4s2,3d10,4p6,5s2,4d6

D. 1s2,2s2,2p6,3s2,3p6,4s2,3d10,4p6,5s2,4d9

10.How many unpaired electrons are present in As?

A.2 B.3

C.4 D.6

11.Determine how many inner electrons are present in Cu atom.

A.12 B.18

C.24 D.36

12.Determine how many valence electrons are present in Cr⁺ atom

A.5 B.6

C.9 D.10

13.Which of the following is a correct equation represent the first ionization for Mg atom?

A.Mg(g) →Mg⁺(g) + e⁻ C. Mg(g) + e⁻ →Mg⁺(g)

B. Mg(g) →Mg2⁺(g) + 2e⁻ D. Mg(g) →Mg⁺(g) e⁻

14.Which of the following elemets has the largest second ionization energy(IE₂)?

A.Li B.B

C.O D.F

15.Arrange the species below in order of increasing ionization energy

A.K⁺ < Ar < Cl⁻ B. Ar < Cl⁻ < K⁺

C. Cl⁻ < K⁺ < Ar D. Cl⁻ < Ar < K⁺

16.Which of the following is the general electron configuration for the outermost electrons of elements in group 6A?

A.ns¹ B.ns²

C.ns²np4 D.ns²np₅

17.What shape of orbital must an electron with the angular quantum number l=2 occupy?

A. B.

C. D.

18. What is the valence electron for Cr ?

A.6 B.7

C.8 D.10

19.The electron affinity process of gaseous fluorine ions from fluorine molecules can be considered a two steps process in which the first step is listed below. What is the second step in this process?

F₂(g)→2F(g)

A.2F⁻(g)→cl(g)+2e⁻

B.F⁺(g)→2F(g)-2e⁻

C.F²(g) + 2e⁻→2F⁻(g)

D.2F(g)+2e⁻→2F⁻(g)

20.Which of the following is the general electron configuration for the outermost electrons of elements in group 4A?

A.ns¹ B.ns²

C.ns²np² D.ns²np₅

21.What shape of orbital must an electron with the angular quantum number l=1 occupy?

A. B.

C. D.

22. Which group of elements has electron affinities with the smallest negative values?

A.5A B.6A

C.1A D.7A

23. What is the name for the element that forms 1+ ions with electronic configuration [Ar]3d¹°?

A.Cu⁺ B.Ti

C.Cr³⁺ D.Sc

Part B

1.a)Which of the quantum numbers relate to the electron only?

b)Which of the quantum numbers relate to the orbital only?

c)How many electrons in an atom can have each of the following quantum number or sublevel designations?

i.5p

ii.n=4;l=3

d)Draw two shape of possible orbitals must electrons with the principle quantum number n=2 occupy?

2.a)Identify the element represents by the electronis configuration below and give the symbosl of other element in the group.

[He] 2s²2p¹

3.a)Write the full set of quantum numbers for the electron gained when Br⁻ ion forms from Br atom.

b)How many inner , outer and valence electrons are present in a Cs atom?

4,a)Which group in periodic table hass elements withvery negative first electron affinities(EA₁)?

b)The EA₂ of an oxygen atom is positive even though its EA₁ is negative. Give a suitable reason on why does this change occur?

5.Rank the ions in each set in order of increasing size and explain your ranking.

a)Se²⁻,S²⁻,O²⁻

b)Te²⁻,I⁻,Cs⁺

6.a)An element X has the following successive ionization energies

IE₁ IE₂ IE₃ IE₄ IE₅

738 1450 7732 10 539 13 628

a)Write the valence electronic configuration fo X.

b)What is the group number belong to X

c)If x is allocated in Period 3 write the full electronic configuration for x.

d) What is the element X?

7.

N³⁻, O²⁻, F⁻,Na⁺,Mg²⁺,Al³⁺

a)Rank the above ions in order of decreasing size.

b)Give an explanation for the observation above.

8.Explain the irregularities in ionization energy in oxygen.

9.a)i.Write the condensed electronic configurations for the element which is located in group 7A and period 3.

ii.Determine the inner, outer and valence electrons for the above element.

b)i.Determine the following are isoelectronic ions or not.Explain.

P³⁻,Ca²⁻,K⁺,S²⁻

ii.Rank these ions in order of increasing size.

iii.Determine which noble gas element have the same electronic configuration as Mg²⁺?

10.The first five ionization energies (kJ/mol) for element magnesium is given below

744,1450,7730,10500,13600

Based on the data given, why there is a bigger change between IE₂ and IE₃ in lement magnesium?

11.

1s²2s²2p₆

i.Give the period number and group number for the element that has the given electronic configuratiob.

ii.Write the set of quantum numbers for any two highest energy level electrons as stated in the electronic configuration above.

12.i)State Hund’s rule and show how it applies to the ground state of chromium atoms.

ii.Write the chemical equations for third electron affinity of phosphorous.

iii.Third electron affinity will always have positive value.Explain.