Deck 8: Electron Configuration and Chemical Periodicity

Question 1

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 m_l is 2.
E)The following set of quantum numbers for a single orbital is not allowed: n = 3,l = 1,m_l = -2.

Answer 1

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

Question 2

Select the correct set of quantum numbers (n,l,m_l,m_s)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,

Answer 2

5,1,0,

Question 3

The electronic structure 1s²2s²2p⁶3s²3p⁶4s²3d⁸ refers to the ground state of

A)Kr
B)Ni
C)Fe
D)Pd
E)None of these choices is correct.

Answer 3

Ni

Question 4

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

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

Question 5

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

A)the aufbau principle.
B)the Pauli exclusion principle.
C)Hund's rule.
D)the periodic law.
E)Heisenberg's principle.

Question 6

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

A)5,1 ,0,

B)5,1,0,

C)5,0,1,

D)5,1,1,

E)5,0,0,

Question 7

The ____________________ quantum numbers are associated with the energy of an electron in a many-electron atom.

A)n and l
B)n and m_l
C)l and m_l
D)n and m_s
E)n,l and m_l

Question 8

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

A)[Ne]3s¹3p¹
B)[He]2s¹2p³
C)[Ne]3s²3p²3d¹
D)[Ne]3s²3p³3d¹
E)[Ne]3s²3p³

Question 9

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

A)1s²1p⁶2s²2p⁶
B)1s²2s²2p⁸3s²3p⁴
C)1s²2s²2p⁸3s²3p²
D)1s²2s²2p⁶3s²3p⁴
E)1s²2s²2p⁶3s²3d⁴

Question 10

Select the correct set of quantum numbers (n,l,m_l,m_s)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,

Question 11

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.

Question 12

"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.
B)Hund's rule.
C)the Pauli exclusion principle.
D)the periodic law.
E)the singularity rule.

Question 13

An element with the electron configuration [noble gas]ns²(n - 1)d⁸ has ___________ valence electrons.

A)2
B)6
C)8
D)10
E)None of these choices is correct.

Question 14

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 these choices is correct.

Question 15

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

A)[Kr]5s²5p⁶4d⁸
B)[Kr]5s²5d¹⁰5p⁴
C)[Kr]5s²4d¹⁰5p⁶
D)[Kr]5s²4f¹⁴
E)[Kr]5s²4d¹⁰5p⁴

Question 16

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

A)[Ar]4s²3d⁹
B)[Ar]4s¹3d¹⁰
C)[Ar]4s²4p⁶3d³
D)[Ar]4s²4d⁹
E)[Ar]5s²4d⁹

Question 17

An element with the electron configuration [noble gas]ns²(n - 1)d¹⁰np³ has ____________ valence electrons.

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

Question 18

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 these statements is generally correct.

Question 19

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

A)a
B)b
C)c
D)d
E)e

Question 20

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

A)shielding.
B)penetration.
C)paramagnetism.
D)electron-pair repulsion.
E)relativity.

Question 21

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

A)X(s) $\to$ X⁺(g)+ e^-
B)X₂(g) $\to$ X⁺(g)+ X^-(g)
C)X(g)+ e^- $\to$ X^-(g)
D)X^-(g) $\to$ X(g)+ e^-
E)X(g) $\to$ X⁺(g)+ e^-

Question 22

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

Question 23

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

Question 24

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 these is generally correct.

Question 25

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

Question 26

Select the element with the least metallic character.

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

Question 27

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

A)X(g) $\to$ X⁺(g)+ e^-
B)X⁺(g) $\to$ X⁺(aq)
C)X⁺(g)+ e^- $\to$ X(g)
D)X(g)+ e^- $\to$ X^-(g)
E)X⁺(g)+ Y^-(g) $\to$ XY(s)

Question 28

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

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

Question 29

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

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

Question 30

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

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

Question 31

Which of the following elements has the smallest atomic size?

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

Question 32

Which of the following elements has the greatest atomic radius?

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

Question 33

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

A)[He]2s²2p⁵
B)[Ne]3s²3p¹
C)[Ar]4s¹4p¹
D)[Kr]5s²4d⁷
E)[He]1p¹

Question 34

Select the most acidic compound from the following.

A)SO₂
B)Al₂O₃
C)CaO
D)PbO
E)H₂O

Question 35

Which of the following elements has the largest atomic size?

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

Question 36

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

Question 37

Select the element with the greatest metallic character.

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

Question 38

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

A)Li
B)B
C)O
D)Ne
E)None of these choices is correct.

Question 39

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 these is generally correct.

Question 40

Which of the following elements has the smallest atomic radius?

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

Question 41

Which of the following atoms will be diamagnetic?

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

Question 42

With the aid of a diagram,describe how the atomic radii of main group elements vary with position in the periodic table.

Question 43

State Hund's rule,and show how it applies to the ground state of phosphorus atoms.

Question 44

Describe how the ionization energies of main group elements vary across a period in the periodic table,using a diagram if necessary.

Question 45

Select the paramagnetic ion.

A)Cu⁺
B)Ag⁺
C)Fe³⁺
D)Cd²⁺
E)Ca²⁺

Question 46

Write down the maximum number of electrons in an atom which can have
a.quantum number n = 4.
b.orbital designation 3d.
c.orbital designation 2p_z.

Question 47

Select the diamagnetic ion.

A)Cu²⁺
B)Ni²⁺
C)Cr³⁺
D)Sc³⁺
E)Cr²⁺

Question 48

Write down the full electron configuration for ground state atoms of
a.element number 12.
b.element number 23.
c.element number 32.

Question 49

Write down the full electron configuration for ground state atoms of
a.S (element 16).
b.Pd (element 46).

Question 50

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

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

Question 51

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

A)Se⁶⁺
B)Se⁴⁺
C)Se²⁺
D)Se^2-
E)Se^4-

Question 52

In Mendeleev's version of the periodic table,the elements were arranged in order of increasing atomic number.

Question 53

Briefly describe how the atomic radii and ionization energies of group 1A(1)elements compare with those of group 8A(18).Also,explain why the values of these properties are so different between these two groups.

Question 54

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

A)P^3- > Cl^- > K⁺ > Ca²⁺
B)Ca²⁺ > K⁺ > Cl^- > P^3-
C)K⁺ > Cl^- > Ca²⁺ > P^3-
D)K⁺ > Cl^- > P^3- > Ca²⁺
E)None of these is correct.

Question 55

Define what is meant by ionization energy,and write a balanced chemical equation to represent the relevant process for element X.

Question 56

Which of the following elements is paramagnetic?

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

Question 57

Define what is meant by electron affinity,and write a balanced chemical equation to represent the relevant process for element Y.

Question 58

Select the most basic compound from the following.

A)Bi₂O₃
B)SiO₂
C)Cs₂O
D)Na₂O
E)H₂O

Question 59

In a single atom,write down the maximum possible number of electrons
a.with n = 3.
b.with the designation 4d_xy.
c.with n = 5,l = 3,m_s = +
.

Question 60

Consider the set of isoelectronic atoms and ions A^2-,B^-,C,D⁺,and E²⁺.Which arrangement of relative radii is correct?

A)A^2- > B^- > C > D⁺ > E²⁺
B)E²⁺ > D⁺ > C > B^- > A^2-
C)A^2- > B^- > C < D⁺ < E²⁺
D)A^2- < B^- < C > D⁺ > E²⁺
E)None of these is correct.

Question 61

In moving down a group in the periodic table,the oxides of the elements become more acidic in nature.

Question 62

Atomic size decreases across a period due to an increase in the effective nuclear charge,Z_eff.

Question 63

In neutral atoms,the 3d orbitals have higher energy than the 4s orbitals.

Question 64

Electron affinities of neutral atoms may be positive or negative.

Question 65

In forming ions of the first series of transition metals,the 4s electrons are lost before the 3d electrons.

Question 66

The maximum number of electrons in an atom with the same value of n is 2n².

Question 67

Elements in which the outermost electron has the same principal quantum number n,show similar chemical properties.

Question 68

First ionization energies of neutral atoms may be positive or negative.

Question 69

According to the exclusion principle,two is the maximum number of electrons in an atom which can share the same four quantum numbers.

Question 70

The difference in energies between the 1s and 2s orbitals is due to the penetration effect.