Chemistry for Changing Times

John W. Hill; Terry W. McCreary; Doris K. Kolb

Chapter 3

Atomic Structure - all with Video Answers

Educators

Chapter Questions

Problem 1

What did each of the following scientists contribute to our knowledge of the atom?
a. William Crookes
b. Eugen Goldstein
c. Michael Faraday
d. J. J. Thomson
e. Ernest Rutherford
f. Iames Chadwick

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Problem 2

What is radioactivity? How did the discovery of radioactivity contradict Dalton's atomic theory?

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Problem 3

How are X-rays and gamma rays similar? How are they different?

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Problem 4

How was Goldstein's experiment different from Thomson's, and how did it reveal different information about the atom?

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Problem 5

In Rutherford's model of the atom, where are the protons, the neutrons, and the electrons found?

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Problem 6

Define or identify each of the following.
a. deuterium
b. tritium
c. photon

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Problem 7

The following table describes four atoms, $A, B, C,$ and $D$.
$$\begin{array}{l|l|l|l|l} & \text { Atom } \mathrm{A} & \text { Atom B } & \text { Atom } \mathrm{C} & \text { Atom D } \\\hline \begin{array}{l}\text { Number of } \\\text { protons }\end{array} & 15 & 19 & 18 & 15 \\\begin{array}{l}\text { Number of } \\\text { neutrons }\end{array} & 16 & 21 & 22 & 17 \\\hline\begin{array}{l}\text { Number of } \\\text { electrons }\end{array} & 15 & 19 & 18 & 15 \\\hline\end{array}$$
a) Which pairs of atoms are isotopes?
b) Which elements represent different elements and are not isotopes?

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Problem 8

Which two atoms in Question 7 have about the same mass but do not represent the same element?

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Problem 9

Compare Dalton's model of the atom with the nuclear model of the atom.

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Problem 10

What are the symbol, name, and atomic number of the element with $Z=57$ ? You may use the periodic table and a table of atomic masses.

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Problem 11

What are the symbol, name, and atomic number of the element that has 34 protons?

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Problem 12

What are the symbol, name, and atomic number of the element that has 34 protons?

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Problem 13

Which atom absorbs more energy, one in which an electron moves from the second shell to the third shell or an
otherwise identical atom in which an electron moves from the first to the third shell?

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Problem 14

How did Bohr and Schrödinger refine the model of the atom?

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Problem 15

What theory uses wave properties to describe the motion of particles at the atomic and subatomic levels?

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Problem 16

Using the Periodic Table determine the number of protons in an atom of each of the following elements.
a. beryllium
b. rubidium
c. arsenic
d. sulfur
e. bismuth
f. radon

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Problem 17

How many electrons are there in each atom of the elements listed in Question $16 ?$

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Problem 18

What subatomic particle makes up cathode rays?

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Problem 19

Rank the three types of radioactivity by charge and by mass.

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Problem 20

An atom with an electric charge is
a. an ion
b. a molecule
$c_{s}$ a nucleus
d. radioactive

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Problem 21

Radioactive elements
a. are those essential to the electronics industry
b. readily form ionic bonds
c. split into nearly equal fragments
d. spontaneously give off particles or rays

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Problem 22

How many electrons are present in an atom that has 11 protons but also a plus two charge?

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Problem 23

Give the symbol and name for (a) an isotope with a mass number of 35 and an atomic number of 17 and
(b) an isotope with 136 neutrons and 86 protons.

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Problem 24

$$\begin{array}{l|l|l|l}\text { Element } & \begin{array}{l}\text { Mass } \\\text { Number }\end{array} & \begin{array}{l}\text { Number } \\\text { of Protons }\end{array} & \begin{array}{l}\text { Number } \\\text { of Neutrons }\end{array} \\\hline \text { Nickel } & 60 & & \\\hline & 108 & 46 & \\\hline & & 7 & 7 \\\hline \text { Iodine } & & & 74 \\\hline\end{array}$$

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Problem 25

How many different elements are listed here?

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Problem 26

How many different isotopes of silver are listed here? (The $X$ does not necessarily represent any specific element.) $\begin{array}{ccccc}108 & 108 & 110 & 109 & 107 \\ 47 & 48 & 47 & 46 & 47\end{array} X$

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Problem 27

The most likely mass number of atom with an atomic number of 14 is

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Problem 28

A magnesium atom has 12 protons, 12 electrons, and 12 neutrons. What is the atom's mass number?

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Problem 29

When an atom loses two electrons, the charge on its ion is ______________

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Problem 30

Which subshell can be occupied by a maximum of 10 electrons?

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Problem 31

Without referring to the periodic table, give the atomic numbers of the elements with the following electron configurations.
a. $1 s^{2} 2 s^{2} 2 p^{3}$
b. $1 s^{2} 2 s^{2} 2 p^{6} 3 s^{2} 3 p^{2}$
c. $1 s^{2} 2 s^{2} 2 p^{6} 3 s^{2} 3 p^{6} 4 s^{1}$

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Problem 32

Without referring to the periodic table, give the atomic numbers of the elements with the following electron configurations.
a. $1 s^{2} 2 s^{2} 2 p^{6} 3 s^{2} 3 p^{3}$
b. $1 s^{2} 2 s^{2} 2 p^{6} 3 s^{2} 3 p^{3}$
c. $1 s^{2} 2 s^{2} 2 p^{6} 3 s^{2} 3 p^{2}$

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Problem 33

Indicate whether each electron configuration represents an atom in the ground state, or in a possible excited state, or is incorrect. In each case, explain why.
a. $1 s^{1} 2 s^{1} 2 p^{1}$
b. $1 s^{2} 2 s^{3} 2 p^{4}$
c. $1 s^{2} 2 s^{1} 2 y^{5}$
d. $1 s^{2} 2 s^{2} 2 p^{3}$

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Problem 34

Indicate whether each electron configuration represents an atom in the ground state or in a possible excited state or is incorrect. In each case, explain why.
a. $1 s^{2} 2 s^{2} 3 s^{2}$
b. $1 s^{2} 2 s^{2} 2 p^{2} 3 s^{1}$
c. $1 s^{2} 2 s^{2} 2 p^{6} 2 d^{5}$
d. $1 s^{2} 2 s^{4} 2 p^{2}$

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Problem 35

Suppose that two electrons are added to the outermost shell of a gallium atom. What element's electron configuration would the atom then have?

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Problem 36

Suppose that each of the following changes is made. Give the symbol for the element whose electron configuration matches the result.
a. Three electrons are added to a tellurium atom.
b. One electron is removed from an iodine atom.
c. Three electrons are removed from an aluminum atom.

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Problem 37

Referring only to the periodic table, tell how the electron configurations of silicon (Si) and germanium (Ge) are similar. How are they different?

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Problem 38

Referring only to the periodic table, tell how the electron configurations of fluorine (F) and chlorine (Cl) are similar. How are they different? How do you expect the electron configurations of bromine (Br) and iodine (I) to be similar to those of fluorine and chlorine?

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Problem 39

Refer to the periodic table to identify each element as a metal or a nonmetal.
a. sulfur
b. phosphorus
c. carbon
d. argon

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Problem 40

Which element(s) is (are) alkali metals?

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Problem 41

Which element(s) is (are) noble gases?

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Problem 42

Which element(s) is (are) transition metals?

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Problem 43

Which element(s) is (are) transition metals?

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Problem 44

All elements with more than 83 protons are radioactive as we shall see in Chapter 11 . Are any of the elements ir the list above necessarily radioactive? If so, which one(s) Could radioactive isotopes of any of the others exist?

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Problem 45

An atom of an element has two electrons in the first shell, eight electrons in the second shell, and one electron in the third shell. From this information, give the element's (a) atomic number, (b) name, (c) total number of electrons in each of its atoms, (d) total number of s electrons, and (e) total number of $d$ electrons.

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Problem 46

Refer to Problem 36. Explain how you can answer the three parts of that problem just by looking at a periodic table and without writing electron structures.

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Problem 47

Without referring to any tables in the text, color the $s, p$, and $d$ blocks and mark an appropriate location for each of the following in the blank periodic table provided: (a) the fourth period noble gas, (b) the third period alkali metal,
(c) the fourth period halogen, and (d) a metal in the fourth period and in group $3 \mathrm{~B}$.

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Problem 48

Look again at Figure 3.11. A patient is found to be suffering from heavy-metal poisoning. An emission spectrum is obtained from a sample of the patient's blood, by spraying a solution of the blood into a flame. The brightest emission lines are found at $5520,5540,5890,$ and $5900 \AA$. What two elements are likely to be present? Which one is more likely to be the culprit?

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Problem 49

Refer to Figure 3.16 and write the electron configurations of (a) iron (Fe), (b) tin (Sn), and (c) lead (Pb).

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Problem 50

Atoms of two adjacent elements in the third period are in the ground state. An atom of element A has only selectrons in its valence shell. An atom of element $\mathrm{B}$ has at least one $p$ electron in its valence shell. Identify elements $\mathrm{A}$ and $\mathrm{B}$.

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Problem 51

Atoms of two adjacent elements in the fifth period are in the ground state. An atom of element Lhas only $s$ electrons in its valence shell. An atom of element $\mathrm{M}$ has at least one $d$ electron in an unfilled shell. Identify elements $\mathrm{L}$ and $\mathrm{M}$

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Problem 52

Atoms of two elements, one above the other in the same group, are in the ground state. An atom of element Q has two $s$ electrons in its outer shell and no $d$ electrons. An atom of element $\mathrm{R}$ has $d$ electrons in its configuration. Identify elements $\mathrm{Q}$ and $\mathrm{R}$.

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Problem 53

Which of the following is true of the water-splitting reaction on page $114 ?$
a. It produces energy, for example, electricity or heat.
b. It requires an energy input, for example, electricity or sunlight.
c. It produces twice as much oxygen as hydrogen.
d. It occurs inside a fuel cell.

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Problem 54

What is produced when solar energy is converted into chemical-bond energy in the water-splitting reaction?
a. hydrogen and nitrogen
b. oxygen and carbon
c. hydrogen and oxygen
d. oxygen and calcium

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Problem 55

Which of the following is not a benefit of using a solar fuel such as hydrogen?
a. A solar fuel can store the energy of sunlight, which is intermittent.
b. A solar fuel can replace some fossil fuels.
c. Using a solar fuel such as hydrogen produces no carbon dioxide emissions.
d. Electrodes used in electrolysis rely on platinum metal.

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Problem 56

Isotopes played an important role in one of the most important experiments investigating photosynthesis, the chemical reaction that converts water $\left(\mathrm{H}_{2} \mathrm{O}\right)$ and carbon dioxide $\left(\mathrm{CO}_{2}\right)$ into glucose $\left(\mathrm{C}_{6} \mathrm{H}_{12} \mathrm{O}_{6}\right)$ and oxygen $\left(\mathrm{O}_{2}\right) .$ For most of the early twentieth century, scientists thought that the oxygen produced by photosynthetic plants and algae came from carbon dioxide they absorbed. To investigate this question, in the early 1940s, chemists at Stanford University used an isotope of oxygen to study the mechanism of the photosynthetic reaction. The researchers fed photosynthesizing algae with water enriched with oxygen-18 and discovered that the oxygen produced was enriched with oxygen-18. Did this result support or refute the hypothesis that the $\mathrm{O}_{2}$ produced by photosynthesis comes from $\mathrm{CO}_{2} ?$

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Problem 57

Apply knowledge that you have gained in this chapter and one or more of the FLaReS principles (Chapter 1) to evaluate the following statements or claims.
Suppose you read in the newspaper that a chemist in South America claims to have discovered a new element with an atomic mass of $34 .$ Extremely rare, it was found in a sample taken from the Andes Mountains. Unfortunately, the chemist has used all of the sample in his analyses.

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Problem 58

Apply knowledge that you have gained in this chapter and one or more of the FLaReS principles (Chapter 1) to evaluate the following statements or claims.
Some aboriginal tribes have rain-making ceremonies in which they toss pebbles of gypsum up into the air. (Gypsum is the material used to make plaster of Paris

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Problem 59

Apply knowledge that you have gained in this chapter and one or more of the FLaReS principles (Chapter 1) to evaluate the following statements or claims.
Some scientists think that life on other planets might be based on silicon rather than carbon. Evaluate this possibility.

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Problem 60

Apply knowledge that you have gained in this chapter and one or more of the FLaReS principles (Chapter 1) to evaluate the following statements or claims.
You come across a website selling water made from only single isotopes of hydrogen and oxygen. A testimonial on the website claims that drinking only the isotopically pure water helps a person feel more refreshed throughout the day

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