Introductory Chemistry: Concepts and Critical Thinking

Problem 1

Why did Mendeleev not include helium in his periodic table of $1871 ?$

David Collins

Numerade Educator

01:10

Problem 2

Why did Mendeleev not include krypton in his periodic table of $1871 ?$

David Collins

Numerade Educator

01:15

Problem 3

Why did Mendeleev not include radium in his periodic table of $1871 ?$

David Collins

Numerade Educator

01:06

Problem 4

Why did Mendeleev not include plutonium in his periodic table of $1871 ?$

David Collins

Numerade Educator

01:41

Problem 5

Before Moseley's discovery in $1913,$ the periodic law stated that physical and chemical properties tend to repeat periodically when elements are arranged according to what trend?

David Collins

Numerade Educator

01:41

Problem 6

After Moseley's discovery in $1913,$ the periodic law stated that physical and chemical properties tend to repeat periodically when elements are arranged according to what trend?

David Collins

Numerade Educator

01:38

Problem 7

Which two elements in the fourth period violate the original periodic law as stated by Mendeleev?

David Collins

Numerade Educator

01:38

Problem 8

Which two elements in the fifth period violate the original periodic law as stated by Mendeleev?

David Collins

Numerade Educator

01:25

Problem 9

Vertical columns in the periodic table are referred to by what two terms?

David Collins

Numerade Educator

01:25

Problem 10

Horizontal rows in the periodic table are referred to by what two terms?

David Collins

Numerade Educator

Problem 11

What is the term for the elements that belong to Groups IA-VIIIA (Groups $1,2,$ and $13-18) ?$

David Collins

Numerade Educator

Problem 12

What is the term for the elements that belong to Groups IIIB-IIB (Groups 3-12)?

David Collins

Numerade Educator

Problem 13

What is the term for the elements in the series that follows element $57 ?$

David Collins

Numerade Educator

Problem 14

What is the term for the elements in the series that follows
element $89 ?$

David Collins

Numerade Educator

Problem 15

What is the term for the two series of elements that include Ce-Lu and Th-Lr?

David Collins

Numerade Educator

Problem 16

Which three elements are rare earth elements, but not lanthanides?

David Collins

Numerade Educator

Problem 17

What is the term for the elements on the left side of the periodic table?

David Collins

Numerade Educator

Problem 18

What is the term for the elements on the right side of the periodic table?

David Collins

Numerade Educator

Problem 19

Which radioactive elements are semimetals because their appearance resembles that of metals?

David Collins

Numerade Educator

Problem 20

Which nonradioactive elements are semimetals because their appearance resembles that of metals?

David Collins

Numerade Educator

Problem 21

Identify the group number corresponding to each of the following families of elements:
(a) alkali metals
(b) alkaline earth metals
(c) halogens
(d) noble gases

David Collins

Numerade Educator

Problem 22

Identify the group number corresponding to each of the following families of elements:
(a) boron group
(b) oxygen group
(c) nickel group
(d) copper group

David Collins

Numerade Educator

02:30

According to IUPAC, what is the designation for each of the following groups indicated by the American convention?
(a) Group IA
(b) Group IIIA
(c) Group VA
(d) Group VIIA
(e) Group IB
(f) Group IIIB
(g) Group VB
(h) Group VIIB

David Collins

Numerade Educator

02:30

Problem 24

According to the American convention using Roman numerals, what is the group number designation for each of the following?
(a) Group 2
(b) Group 4
(c) Group 6
(d) Group 8
(e) Group 11
(f) Group 12
(g) Group 16
(h) Group 18

David Collins

Numerade Educator

01:28

Problem 25

Refer to the periodic table and select the symbol of the element that fits each of the following descriptions:
(a) the Group VA/15 semimetal in the fifth period
(b) the sixth-period representative element with properties similar to Sr
(c) the fifth-period transition element with properties similar to Ti
(d) the lighter-than-air noble gas used in blimps and party balloons

David Collins

Numerade Educator

01:32

Problem 26

Refer to the periodic table and select the symbol of the element that fits each of the following descriptions:
(a) the Group IVA/14 semimetal in the fourth period
(b) the third-period alkali metal
(c) the halogen that is normally a solid and not radioactive
(d) the lanthanide that is not naturally occurring

David Collins

Numerade Educator

01:44

Problem 27

Refer to the periodic table and select the symbol of the element that fits each of the following descriptions:
(a) the third-period alkaline earth metal
(b) the halogen that exists as a reddish-brown liquid at normal conditions
(c) the rare earth element whose atomic number is greatest
(d) the actinide with properties similar to Ce.

David Collins

Numerade Educator

Problem 28

Refer to the periodic table and select the symbol of the element that fits each of the following descriptions:
(a) the fourth-period representative element with properties similar to $\mathrm{O}$
(b) the sixth-period transition element with properties similar to $\mathrm{Ni}$
(c) the rare earth element whose atomic mass is lowest
(d) the radioactive noble gas

David Collins

Numerade Educator

Problem 29

According to the general trend, metallic character for a period of elements (increases/decreases) proceeding from left to right in the periodic table.

David Collins

Numerade Educator

Problem 30

According to the general trend, metallic character (increases/decreases) proceeding up a group of elements in the periodic table.

David Collins

Numerade Educator

Problem 31

According to the general trend, the atomic radius for a period of elements (increases/decreases) proceeding from left to right in the periodic table.

David Collins

Numerade Educator

Problem 32

According to the general trend, the atomic radius (increases/decreases) proceeding up a group of elements in the periodic table.

David Collins

Numerade Educator

01:20

Problem 33

According to general trends in the periodic table, predict which element in each of the following pairs has greater metallic character:
(a) $\mathrm{B}$ or $\mathrm{Al}$
(b) Na or K
(c) $\mathrm{Mg}$ or Ba
(d) $\mathrm{H}$ or $\mathrm{Fe}$

David Collins

Numerade Educator

01:32

Problem 34

According to general trends in the periodic table, predict which element in each of the following pairs has greater metallic character:
(a) $\mathrm{K}$ or $\mathrm{Ca}$
(b) $\mathrm{Mg}$ or $\mathrm{Al}$
(c) Fe or Cu
(d) S or Ar

David Collins

Numerade Educator

01:17

Problem 35

According to general trends in the periodic table, predict which element in each of the following pairs has the larger atomic radius:
(a) Li or Na
(b) $\mathrm{N}$ or $\mathrm{P}$
(c) $\mathrm{Mg}$ or $\mathrm{Ca}$
(d) Ar or Kr

David Collins

Numerade Educator

01:39

Problem 36

According to general trends in the periodic table, predict which element in each of the following pairs has the larger atomic radius:
(a) $\mathrm{Rb}$ or $\mathrm{Sr}$
(b) As or Se
(c) Pb or Bi
(d) I or Xe

David Collins

Numerade Educator

02:08

Problem 37

Predict the missing value (?) for each property listed below. The atomic radius, density, and melting point are given for elements in Group IA/1.
$$\begin{array}{cccc}\hline \text { Element } & \text { Atomic Radius } & \text { Density at } 20^{\circ} \mathrm{C} & \text { Melting Point } \\
\hline \mathrm{K} & (?) \mathrm{nm} & 0.86 \mathrm{~g} / \mathrm{mL} & 63.3^{\circ} \mathrm{C} \\\mathrm{Rb} & 0.248 \mathrm{nm} & (?) \mathrm{g} / \mathrm{mL} & 38.9^{\circ} \mathrm{C} \\\mathrm{Cs} & 0.266 \mathrm{nm} & 1.90 \mathrm{~g} / \mathrm{mL} & (?){ }^{\circ} \mathrm{C} \\\hline\end{array}$$

David Collins

Numerade Educator

02:07

Problem 38

Predict the missing value (?) for each property listed below. The atomic radius, density, and melting point are given for elements in Group VIB/6.
$$\begin{array}{cccc}\hline \text { Element } & \text { Atomic Radius } & \text { Density at } 20^{\circ} \mathrm{C} & \text { Melting Point } \\
\hline \mathrm{Cr} & 0.125 \mathrm{nm} & 7.14 \mathrm{~g} / \mathrm{mL} & (?){ }^{\circ} \mathrm{C} \\\mathrm{Mo} & (?)\mathrm{nm} & 10.28 \mathrm{~g} / \mathrm{mL} & 2617^{\circ} \mathrm{C} \\\mathrm{W} & 0.137 \mathrm{nm} & (?) \mathrm{g} / \mathrm{mL} & 3410^{\circ} \mathrm{C}\end{array}$$

David Collins

Numerade Educator

02:02

Problem 39

Predict the missing value (?) for each property listed below. The atomic radius, density, and boiling point are given for elements in Group VIIA/17.
$$\begin{array}{cccc}\hline \text { Element } & \text { Atomic Radius } & \text { Density at } 20^{\circ} \mathrm{C} & \text { Boiling Point } \\
\hline \mathrm{Cl} & (?) \mathrm{nm} & 1.56 \mathrm{~g} / \mathrm{mL} & -34.6^{\circ} \mathrm{C} \\\mathrm{Br} & 0.115 \mathrm{nm} & (?) \mathrm{g} / \mathrm{mL} & 58.8^{\circ} \mathrm{C} \\\mathrm{I} & 0.133 \mathrm{nm} & 4.97 \mathrm{~g} / \mathrm{mL} & (?)^{\circ} \mathrm{C} \\\hline\end{array}$$

David Collins

Numerade Educator

01:53

Problem 40

Predict the missing value (?) for each property listed below. The atomic radius, density, and boiling point are given for elements in Group VIIIA/18.
$$\begin{array}{cccc}\hline \text { Element } & \text { Atomic Radius } & \text { Density at STP } & \text { Boiling Point } \\\hline \mathrm{Ar} & 0.180 \mathrm{nm} & 1.78 \mathrm{~g} / \mathrm{L} & (?){ }^{\circ} \mathrm{C} \\\mathrm{Kr} & (?) \mathrm{nm} & 3.74 \mathrm{~g} / \mathrm{L} & -152{ }^{\circ} \mathrm{C} \\\mathrm{Xe} & 0.210 \mathrm{nm} & (?) \mathrm{g} / \mathrm{L} & -107{ }^{\circ} \mathrm{C} \\\hline\end{array}$$

David Collins

Numerade Educator

01:18

Problem 41

The formulas for the chlorides of potassium, calcium, boron, and germanium are, respectively, $\mathrm{KCl}, \mathrm{CaCl}_{2}, \mathrm{BCl}_{3}$, and $\mathrm{GeCl}_{4}$. Using the periodic table, predict the chemical formulas for each of the following similar compounds:
(a) potassium fluoride
(b) calcium fluoride
(c) boron bromide
(d) germanium iodide

David Collins

Numerade Educator

01:19

Problem 42

The formulas for the oxides of sodium, magnesium, aluminum, and silicon are, respectively, $\mathrm{Na}_{2} \mathrm{O}, \mathrm{MgO}, \mathrm{Al}_{2} \mathrm{O}_{3},$ and $\mathrm{SiO}_{2}$. Using the periodic table, predict the chemical formulas for each of the following similar compounds:
(a) lithium oxide
(b) barium oxide
(c) gallium oxide
(d) tin oxide

David Collins

Numerade Educator

01:24

Problem 43

The chemical formula for zinc oxide is $\mathrm{ZnO}$. Predict the formulas for each of the following similar compounds:
(a) cadmium oxide
(b) cadmium sulfide
(c) cadmium selenide
(d) cadmium telluride

David Collins

Numerade Educator

01:10

Problem 44

David Collins

Numerade Educator

01:08

Problem 45

Depending upon reaction conditions, nitrogen and oxygen can produce either $\mathrm{N}_{2} \mathrm{O}_{3}$ and $\mathrm{N}_{2} \mathrm{O}_{5} .$ Predict two formulas for each of the following compounds:
(a) arsenic oxide
(b) antimony oxide

David Collins

Numerade Educator

01:06

Problem 46

Depending upon reaction conditions, phosphorus and sulfur can produce either $\mathrm{P}_{2} \mathrm{~S}_{3}$ and $\mathrm{P}_{2} \mathrm{~S}_{5} .$ Predict two formulas for each of the following compounds:
(a) arsenic sulfide
(b) antimony sulfide

David Collins

Numerade Educator

Problem 47

What type of energy sublevel is being filled by the elements in Groups IA/1 and IIA/2?

David Collins

Numerade Educator

Problem 48

What type of energy sublevel is being filled by the elements in Groups IIIA/13 through VIIIA/18?

David Collins

Numerade Educator

Problem 49

What type of energy sublevel is being filled by the transition elements?

David Collins

Numerade Educator

Problem 50

What type of energy sublevel is being filled by the inner transition elements?

David Collins

Numerade Educator

Problem 51

Which energy sublevel is being filled by the lanthanide series?

David Collins

Numerade Educator

Problem 52

Which energy sublevel is being filled by the actinide series?

David Collins

Numerade Educator

Problem 53

Refer to the periodic table and state the highest energy sublevel for each of the following elements:
(a) H
(b) $\mathrm{Na}$
(c) Sm
(d) Br
(e) Sr
(f) $C$
(g) Sn
(h) Cs

David Collins

Numerade Educator

01:42

Problem 54

Refer to the periodic table and state the highest energy sublevel for each of the following elements:
(a) He
(b) $K$
(c) U
(d) $\mathrm{Pd}$
(e) Be
(f) Co
(g) Si
(h) $\mathrm{Pt}$

David Collins

Numerade Educator

05:22

Problem 55

Refer to the periodic table and write the predicted electron configuration for each of the following elements:
(a) $\mathrm{Li}$
(b) F
(c) $\mathrm{Mg}$
(d) $P$
(f) $\mathrm{Mn}$
(g) Ga
(h) $\mathrm{Rb}$

David Collins

Numerade Educator

05:34

Problem 56

Refer to the periodic table and write the predicted electron configuration for each of the following elements:
(a) B
(b) Ti
(c) Na
(d) O
(e) Ge
(f) Ba
(g) Pd
(h) $\mathrm{Kr}$

David Collins

Numerade Educator

01:21

Problem 57

State the number of valence electrons in each of the following groups as predicted from the periodic table:
(a) Group IA/1
(b) Group $\mathrm{IIIA} / 13$
(c) Group VA/15
(d) Group VIIA/17

David Collins

Numerade Educator

01:18

Problem 58

State the number of valence electrons in each of the following groups as predicted from the periodic table:
(a) Group IIA/2
(b) Group IVA/14
(c) Group VIA/16
(d) Group VIIIA/18

David Collins

Numerade Educator

01:25

Problem 59

State the number of valence electrons for each of the following elements:
(a) $\mathrm{H}$
(b) B
(c) $N$
(d) F
(e) $\mathrm{Ca}$
(f) Si
(g) O
(h) Ar

David Collins

Numerade Educator

01:45

Problem 60

State the number of valence electrons for each of the following elements:
(a) He
(b) $\mathrm{Pb}$
(c) Se
(d) Ne
(e) $\mathrm{Cs}$
(f) Ga
(g) Sb
(h) Br

David Collins

Numerade Educator

01:32

Problem 61

Draw the electron dot formula for each of the following elements:
(a) $\mathrm{H}$
(b) B
(c) $N$
(d) F
(e) Ca
(f) Si
(g) O
(h) Ar

David Collins

Numerade Educator

02:07

Problem 62

Draw the electron dot formula for each of the following elements:
(a) He
(b) $\mathrm{Pb}$
(c) Se
(d) Ne
(e) $\mathrm{Cs}$
(f) Ga
(g) Sb
(h) Br

David Collins

Numerade Educator

Problem 63

According to the general trend, the ionization energy for a group of elements (increases/decreases) proceeding up a group in the periodic table.

David Collins

Numerade Educator

Problem 64

According to the general trend, the ionization energy for a period of elements (increases/decreases) proceeding from left to right in the periodic table.

David Collins

Numerade Educator

Problem 65

Which group of elements has the lowest ionization energy?

David Collins

Numerade Educator

Problem 66

Which group of elements has the highest ionization energy?

David Collins

Numerade Educator

01:24

Problem 67

Refer to the periodic table and predict which element in each of the following pairs has the higher ionization energy:
(a) $\mathrm{Mg}$ or $\mathrm{Ca}$
(b) S or Se
(c) Sn or Pb
(d) N or P

David Collins

Numerade Educator

01:27

Problem 68

Refer to the periodic table and predict which element in each of the following pairs has the higher ionization energy:
(a) Ga or Ge
(b) Si or P
(c) Br or Cl
(d) As or Sb

David Collins

Numerade Educator

01:35

Problem 69

Refer to the periodic table and predict which element in each of the following pairs has the lower ionization energy:
(a) $\mathrm{Rb}$ or $\mathrm{Cs}$
(b) He or Ar
(c) $\mathrm{B}$ or $\mathrm{Al}$
(d) For I

David Collins

Numerade Educator

01:18

Problem 70

Refer to the periodic table and predict which element in each of the following pairs has the lower ionization energy:
(a) $\mathrm{Mg}$ or $\mathrm{Si}$
(b) $\mathrm{Pb}$ or $\mathrm{Bi}$
(c) Ca or Ga
(d) $P$ or $C l$

David Collins

Numerade Educator

02:09

Problem 71

State the predicted ionic charge of metal ions in each of the following groups of elements:
(a) Group IA/1
(b) Group IIA/2
(c) Group IIIA/13
(d) Group IVA/14

David Collins

Numerade Educator

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Problem 72

State the predicted ionic charge of nonmetal ions in each of the following groups of elements:
(a) Group IVA/14
(b) Group $\mathrm{VA} / 15$
(c) Group VIA/16
(d) Group VIIA/17

Ronald Prasad

Numerade Educator

01:39

Problem 73

Write the ionic charge for each of the following ions as predicted from the group number in the periodic table:
(a) $\mathrm{Cs}$ ion
(b) Ga ion
(c) Oion
(d) I ion

David Collins

Numerade Educator

01:36

Problem 74

Write the ionic charge for each of the following ions as predicted from the group number in the periodic table:
(a) Be ion
(b) Sn ion
(c) $\mathrm{P}$ ion
(d) Sion

David Collins

Numerade Educator

01:42

Problem 75

Refer to the periodic table and predict which of the following ions are isoelectronic with the noble gas argon:
(a) $\mathrm{Al}^{3+}$
(b) $\mathrm{Ca}^{2+}$
(c) $S^{2-}$
(d) $\mathrm{N}^{3-}$

David Collins

Numerade Educator

01:42

Problem 76

Refer to the periodic table and predict which of the following ions are isoelectronic with the noble gas krypton:
(a) $\mathrm{K}^{+}$
(b) $\mathrm{Sr}^{2+}$
(c) $\mathrm{Cl}^{-}$
(d) $\mathrm{Se}^{2-}$

David Collins

Numerade Educator

06:23

Problem 77

Refer to the periodic table and write the predicted electron configuration for each of the following positive ions using core notation:
(a) $\mathrm{Mg}^{2+}$
(b) $K^{+}$
(c) $\mathrm{Fe}^{2+}$
(d) $Z r^{2+}$

David Collins

Numerade Educator

06:09

Problem 78

Refer to the periodic table and write the predicted electron configuration for each of the following positive ions using core notation:
(a) $\mathrm{Ti}^{2+}$
(b) $Z n^{2+}$
(c) $Y^{3+}$
(d) $\mathrm{Cs}^{+}$

David Collins

Numerade Educator

04:37

Problem 79

Refer to the periodic table and write the predicted electron configuration for each of the following negative ions using core notation:
(a) $\mathrm{F}^{-}$
(b) $S^{2-}$
(c) $\mathrm{N}^{3-}$
(d) $\mathrm{I}^{3-}$

David Collins

Numerade Educator

04:19

Problem 80

Refer to the periodic table and write the predicted electron configuration for each of the following negative ions using core notation:
(a) $\mathrm{Br}^{-}$
(b) $\mathrm{Te}^{2-}$
(c) $\mathrm{As}^{3-}$
(d) $\mathrm{O}^{2-}$

David Collins

Numerade Educator

01:11

Problem 81

Use the American convention to designate the group number corresponding to each of the following groups listed by the European convention:
(a) Group IA
(b) Group IB
(c) Group IIIA
(d) Group IIIB

David Collins

Numerade Educator

01:23

Problem 82

Use the IUPAC convention to designate the group number corresponding to each of the following groups listed by the European convention:
(a) Group IIA
(b) Group IIB
(c) Group IVA
(d) Group IVB

David Collins

Numerade Educator

01:36

Problem 83

Predict the atomic radius, density, and melting point for radioactive francium.
$$\begin{array}{cccc}\hline \text { Element } & \text { Atomic Radius } & \text { Density at } 20^{\circ} \mathrm{C} & \text { Melting Point } \\
\hline \mathrm{Rb} & 0.248 \mathrm{nm} & 1.53 \mathrm{~g} / \mathrm{mL} & 38.9^{\circ} \mathrm{C} \\\mathrm{Cs} & 0.266 \mathrm{nm} & 1.87 \mathrm{~g} / \mathrm{mL} & 28.4{ }^{\circ} \mathrm{C} \\\mathrm{Fr} & (?) \mathrm{nm} & (?) \mathrm{g} /\mathrm{mL} & (?){ }^{\circ} \mathrm{C} \\\hline\end{array}$$

David Collins

Numerade Educator

01:20

Problem 84

Predict the atomic radius, density, and melting point for radioactive radium.
$$\begin{array}{cccc}\hline \text { Element } & \text { Atomic Radius } & \text { Density at } 20^{\circ} \mathrm{C} & \text { Melting Point } \\\hline \mathrm{Sr} & 0.215 \mathrm{nm} & 2.63 \mathrm{~g} / \mathrm{mL} & 769^{\circ} \mathrm{C} \\\mathrm{Ba} & 0.217 \mathrm{nm} & 3.65 \mathrm{~g} / \mathrm{mL} & 725^{\circ} \mathrm{C} \\\mathrm{Ra} & (?) \mathrm{nm} & (?) \mathrm{g} / \mathrm{mL} & (?){ }^{\circ} \mathrm{C} \\\hline\end{array}$$

David Collins

Numerade Educator

02:16

Problem 85

Refer to the periodic table and write the predicted electron configuration for each of the following elements using core notation:
(a) Sr
(b) $R u$
(c) Sb
(d) $\mathrm{Cs}$

David Collins

Numerade Educator

02:05

Problem 86

Refer to the periodic table and write the predicted electron configuration for each of the following elements using core notation:
(a) W
(b) Bi
(c) $\mathrm{Ra}$
(d) $A C$

David Collins

Numerade Educator

01:41

Problem 87

Explain why the ionization energy for hydrogen is much higher than that of other Group IA/1 elements.

David Collins

Numerade Educator

01:12

Problem 88

Predict two ionic charges for hydrogen. Write the formulas of the two ions and explain the ionic charges.

David Collins

Numerade Educator

01:30

Problem 89

Examine Figure 1 and determine the name of the element that Mendeleev predicted before its discovery and called ekaboron.

David Collins

Numerade Educator

01:30

Problem 90

Examine Figure 1 and determine the name of the element that Mendeleev predicted before its discovery and called ekaaluminum.

David Collins

Numerade Educator

01:51

Problem 91

Explain why the ionization energy for the alkali metals is less than the ionization energy for the alkaline earth metals.

David Collins

Numerade Educator