Deck 7: The Periodic Table and Periodic Trends

Question 1

The _____ have the highest molar volumes of the solid elements.

A) halogens
B) semimetals
C) non-metals
D) alkaline earth metals
E) alkali metals

Answer 1

alkali metals

Question 2

Copper, gold, and silver are grouped in a triad.

Answer 2

True

Question 3

According to the Newlands arrangement of elements into octaves, copper would belong to the same octave as _____.

A) potassium
B) oxygen
C) fluorine
D) carbon
E) calcium

Answer 3

potassium

Question 4

The noble gases have the highest molar volumes among all the other groups.

Question 5

Meyer aligned the elements in his table according to periodic variations in _____.

A) atomic shapes
B) atomic number
C) atomic volume
D) chemical properties
E) their natural occurrence

Question 6

In Mendeleev's periodic table, the element with a mass number of 31 would have been called eka-_____.

A) chlorine
B) zirconium
C) nitrogen
D) boron
E) carbon

Question 7

The elements in an isoelectronic series have the same ionic radii.

Question 8

H. G. J. Moseley showed that the periodic arrangement of elements was determined by _____.

Question 9

John Newlands proposed that elements be classified into _____, a group of seven elements corresponding to the horizontal rows in the main group elements.

A) periods
B) rows
C) septanes
D) cohorts
E) octaves

Question 10

The outermost electrons in xenon feel a greater amount of electronic shielding as compared to those of cadmium.

Question 11

Write a note on John Newlands "octaves" classification.

Question 12

Chlorine, _____, and iodine constitute a triad.

Question 13

In the periodic table, atomic radii increase from top to bottom down a column.

Question 14

A comparison of ionic radii with atomic radii shows that a cation is always smaller than the parent neutral atom.

Question 15

The discovery of _____ with properties similar to aluminum and silicon respectively provided convincing evidence in support of Mendeleev's arrangement of the elements.

A) scandium and titanium
B) gallium and germanium
C) technetium and rubidium
D) selenium and iodine
E) neon and krypton

Question 16

A comparison of ionic radii with atomic radii shows that an anion is always smaller than the parent neutral atom.

Question 17

In the Mendeleev's periodic table, if bromine was a newly discovered element, it would have been called eka-chlorine.

Question 18

How did Mendeleev's periodic table differ from Meyer's model?

Question 19

The electrons in the 1s shell of a nitrogen atom will face greater electrostatic attraction than the electrons in the 1s shell of an aluminum atom.

Question 20

Mendeleev correctly predicted the existence of gallium which he called eka-_____.

Question 21

The atomic radius of Br is _____ than the atomic radius of I.

Question 22

Which member of the isoelectronic series having the closed shell electronic configuration of neon has the smallest radius?

A) N^3-
B) O^2-
C) F^-
D) Xe
E) Mg²⁺

Question 23

How does the effective nuclear charge on electrons in the outermost shell vary across a row and down a group?

Question 24

The _____ is half the distance between the nuclei of two adjacent metal atoms.

Question 25

Which of the following has the smallest radius?

A) C
B) Si
C) Ge
D) Sn
E) Pb

Question 26

Define the different types of atomic radii measured in different types of molecules. How does atomic radii vary across a row in the periodic table?

Question 27

The atomic radius of Cu is _____ than the atomic radius of As.

Question 28

Cobalt occurs in nature in compounds with multiple oxidation states. Cobalt ions with the oxidation state of _____ will have the largest radius.

A) +5
B) -½
C) 0
D) +1
E) -1

Question 29

Out of the five elements given below, the outermost electrons of _____ will experience the maximum shielding.

A) vanadium
B) chromium
C) copper
D) zinc
E) nickel

Question 30

Which of the following has the smallest radius?

A) K
B) Ca
C) Sc
D) Ti
E) V

Question 31

Half the internuclear distance between two nonbonded atoms in a solid is called the _____ radius.

A) ionic atomic
B) metallic atomic
C) average neutral
D) covalent atomic
E) van der Waals atomic

Question 32

Which of the following atoms has the largest radius?

A) Aluminum
B) Silicon
C) Phosphorous
D) Chlorine
E) Argon

Question 33

Which of the following atoms has the largest radius?

A) Helium
B) Neon
C) Krypton
D) Xenon
E) Argon

Question 34

Which of the following shells will be the most attracted to the nucleus due to electrostatic forces?

A) 1s
B) 1p
C) 2s
D) 2p
E) 3s

Question 35

Which of the following is a member of the isoelectronic series consisting of Cl^-?

A) Kr⁰
B) O^2-
C) K⁺
D) Zn²⁺
E) Br^-

Question 36

The ionic radius of Fe²⁺ is _____ than the ionic radius of Fe³⁺.

Question 37

Electrons in the 1s shell of _____ will face the greatest electrostatic attraction toward the nucleus.

A) helium
B) neon
C) argon
D) krypton
E) chlorine

Question 38

_____ is the radius of a cation or anion.

Question 39

An isoelectronic series is a series of ions, or ions and atoms:

A) with the same charge.
B) having the same atomic mass.
C) having the same number of neutrons.
D) having the same atomic radius.
E) having the same exact electronic configuration.

Question 40

Half the distance between the nuclei of two like atoms joined by a covalent bond in the same molecule is called the _____ radius.

A) ionic atomic
B) metallic atomic
C) average neutral
D) covalent atomic
E) van der Waals atomic

Question 41

What is the general trend in electron affinities of elements down a group? What are the exceptions to this trend?

Question 42

Based on their position in the periodic table, which of the following atoms would have the smallest ionization energy?

A) Sodium
B) Neon
C) Chlorine
D) Bromine
E) Potassium

Question 43

Which of the following atoms would have the greatest ionization energy for the removal of the second electron?

A) Magnesium
B) Beryllium
C) Aluminum
D) Iron
E) Sodium

Question 44

The electron affinities of the alkaline earth metals become more negative from Be to Ba. The energy separation between the filled ns² and the empty np subshells decreases with increasing n, so that formation of an anion from the heavier elements becomes energetically more favorable.

Question 45

The fourth ionization energy of boron will be much higher than that of carbon.

Question 46

Magnesium will have a(n) _____ value for electron affinity.

Question 47

What is the Mulliken electronegativity of sulfur that has an electron affinity value of −200.4 kJ/mol and an ionization energy value of 999.6 kJ/mol?

A) -100.2 kJ/mol
B) 499.8 kJ/mol
C) 799.2 kJ/mol
D) 600.0 kJ/mol
E) 120.0 kJ/mol

Question 48

The _____ of an element is the amount of energy needed to remove an electron from the gaseous atom in its ground state.

A) neutron potential energy
B) half life
C) nuclear charge energy
D) ionization energy
E) configuration energy

Question 49

Which of the following elements has the most negative electron affinity?

A) Fluorine
B) Sulfur
C) Chlorine
D) Argon
E) Selenium

Question 50

Write a note on the differences in electronegativity between metals and non-metals.

Question 51

Elements with a high electronegativity have very positive electron affinities and small ionization potentials.

Question 52

Ionization energies increase from left to right across each row, with discrepancies occurring at ns²np¹ (group 13), _____, and ns²(n − 1)d¹⁰ (group 12) electron configurations.

Question 53

The second electron affinity is always positive regardless of the element.

Question 54

Based on their position in the periodic table, which of the following elements would have the highest fourth ionization energy?

A) Aluminum
B) Silicon
C) Phosphorus
D) Sulfur
E) Chlorine

Question 55

Ionization energies increase from left to right across each row, with discrepancies occurring at _____.

A) ns¹
B) ns²
C) ns²np¹
D) ns²np²
E) ns²np³

Question 56

Which of the following elements has the greatest electronegativity?

A) Carbon
B) Chlorine
C) Silicon
D) Sodium
E) Arsenic

Question 57

Electron affinities of the main-group elements become less negative as we proceed _____ a column of the periodic table.

Question 58

Which of the following elements of the same period will have the lowest first ionization energy?

A) Germanium
B) Arsenic
C) Selenium
D) Bromine
E) Krypton

Question 59

The ionization energy of an element is always positive.

Question 60

Fluorine is the least electronegative nonradioactive element.

Question 61

All of the group 14 elements form compounds in the _____ oxidation state.

A) +4
B) +2
C) -4
D) -2
E) +1

Question 62

Nitrogen and phosphorous belong to the group of elements referred to as chalcogens.

Question 63

The elements of _____ are called the alkali metals.

A) group 1
B) group 3
C) group 13
D) group 17
E) group 18

Question 64

Which halogen does not have a positive oxidation state in any of its compounds?

A) Fluorine
B) Chlorine
C) Bromine
D) Iodine
E) Astatine

Question 65

Write a note on the oxidation states of group 13 elements.

Question 66

What is the valence electron configuration of alkali metals?

A) ns¹
B) ns²
C) np¹
D) np²
E) (n - 1)d¹

Question 67

Transition metals have multiple oxidation states that are separated by only one electron.

Question 68

Which of the following is a common oxidation state of elements in group 15?

A) +1
B) +2
C) -2
D) -5
E) +3

Question 69

Elements with a small first ionization energy and a small electron affinity have a(n) _____ electronegativity.

Question 70

Write a note on the allotropes of carbon.

Question 71

Which of the following elements belong to group 2 in the periodic table?

A) Sodium
B) Strontium
C) Osmium
D) Bismuth
E) Lithium

Question 72

The elements in group 16 are known as _____.

A) pnicogens
B) alkali metals
C) halogens
D) chalcogens
E) alkaline earth metals

Question 73

Fullerenes and nanotubes are allotropes of carbon.

Question 74

Which of the following is a pnicogen?

A) He
B) Ne
C) F
D) Bi
E) Cl

Question 75

If X is an alkali metal, what sort of compound would it form with oxygen?

A) XO
B) XO₂
C) X₂O
D) X₂O₃
E) X₃O₂

Question 76

The valence electron configuration of the elements in group 13 is _____.

Question 77

Which of the following elements in group 3 of the periodic table is a semimetal?

A) Boron
B) Aluminum
C) Gallium
D) Indium
E) Thallium

Question 78

Pure group 1 elements are powerful oxidizing agents.

Question 79

What are the two oxidation states important in group 13 elements?

A) +2, +4
B) +1, +2
C) +1, +4
D) +2, +3
E) +1, +3

Question 80

Which of the following elements belongs to group 14?

A) Antimony
B) Tellurium
C) Tin
D) Bismuth
E) Indium