Atomic Structure and Radiation REVIEW GAME

To complete this review game: You will need a copy of the Periodic Table. You will NOT need a calculator.

For additional review, see also: The Atomic Structure Self-QUIZ at http://www.mcwdn.org/chemist/atom/atomquiz.html and The Half-life Self-QUIZ at http://www.softschools.com/quizzes/chemistry/half_life/quiz3544.html

List the following electromagnetic spectrum wave types in order from lowest energy to highest energy: Gamma rays Infrared Microwaves Radiowaves Ultraviolet Visible light X-rays

List the following electromagnetic spectrum wave types in order from lowest energy to highest energy: Radiowaves Microwaves Infrared Visible light Ultraviolet X-rays Gamma rays

What is the relationship between wavelength and frequency in the electromagnetic spectrum?

What is the relationship between wavelength and frequency in the electromagnetic spectrum? As wavelength decreases, frequency increases

What is the relationship between frequency and energy in the electromagnetic spectrum?

What is the relationship between frequency and energy in the electromagnetic spectrum? As frequency increases, energy increases

Which of the wave types within the electromagnetic spectrum are potentially ionizing?

Which of the wave types within the electromagnetic spectrum are potentially ionizing? Ultraviolet X-rays Gamma rays

Which of the statements below is an accurate description of what occurs during ionization of an atom? a. An atom loses a proton and becomes a negatively charged ion. b. An atom loses an electron and becomes a positively charged ion. c. An atom loses an electron and becomes a negatively charged ion. d. An atom gains a neutron and its atomic mass increases by 1.

Which of the statements below is an accurate description of what occurs during ionization of an atom? a. An atom loses a proton and becomes a negatively charged ion. b. An atom loses an electron and becomes a positively charged ion. c. An atom loses an electron and becomes a negatively charged ion. d. An atom gains a neutron and its atomic mass increases by 1.

How many prot0ns, neutrons and electrons in an atom of Platinum?

How many prot0ns, neutrons and electrons in an atom of Platinum? Protons = 78 Neutrons = 117 Electrons = 78 Referring to the Periodic Table, we can see that platinum, Pt, has an atomic number of 78. Thus Pt has 78 protons. As we are speaking of an uncharged atom, we know that the number of electrons is equal to the number of protons, and is therefore also 78. Referring to the Periodic Table, we can see that platinum has an average atomic mass of 195.08 amu. Rounding to the nearest whole number gives 195 amu. As amu = # protons + # neutrons, we can calculate # neutrons = amu - # protons, which is 195 – 78 = 117. Thus platinum has 117 neutrons.

Element identity (what element it is) is determined by its atomic number. its mass number. its neutron number. All of these are correct.

Element identity (what element it is) is determined by its atomic number. its mass number. its neutron number. All of these are correct. Element identity, meaning the element NAME, is determined solely be the number of protons, and hence solely by atomic number.

How many prot0ns, neutrons and electrons in a Ba2+ ion?

How many prot0ns, neutrons and electrons in a Ba2+ ion? Protons = 56, Neutrons = 81, Electrons = 54 Referring to the Periodic Table, we can see that Ba, barium, has an atomic number of 56. Thus Ba2+ has 56 protons. As we are speaking of an ion with a +2 positive charge, this atom has LOST TWO ELECTRONS. Therefore, this ion has 56 - 2 electrons = 54 electrons. Referring to the Periodic Table, we can see that barium has an average atomic mass of 137.327 amu. As electrons do not contribute to the atomic mass (having virtually no mass themselves), this barium ion has the same average atomic mass. Rounding to the nearest whole number gives 137 amu. As amu = # protons + # neutrons, we can calculate # neutrons = amu - # protons, which is 137 – 56 = 81. Thus, our barium ion has 81 neutrons.

Isotopes of an element a. Are always radioactive b. Differ in their number of protons c. Differ in their number of neutrons d. Differ in their number of electrons

Isotopes of an element a. Are always radioactive b. Differ in their number of protons c. Differ in their number of neutrons d. Differ in their number of electrons

Element Q has three common isotopes. If the abundance of 44X is 0 Element Q has three common isotopes. If the abundance of 44X is 0.03, the abundance of 45X is 0.25%, and the abundance of 48X is 99.72%, what is the average atomic mass of element Q? a. 32.89 b. 43.63 c. 47.99 d. 48.76

Element Q has three common isotopes. If the abundance of 44X is 0 Element Q has three common isotopes. If the abundance of 44X is 0.03, the abundance of 45X is 0.25%, and the abundance of 48X is 99.72%, what is the average atomic mass of element Q? a. 32.89 b. 43.63 c. 47.99 d. 48.76 P.S. In this case you don’t even need a calculator to figure it out, since only one of the provided responses is within the atomic mass range of the three isotopes. Clearly the average can’t be LOWER or HIGHER than that range, and therefore responses a., b., and d. CANNOT be correct. Only c. fits within the range of atomic masses of the isotopes.

What atom is depicted in this figure?

What atom is depicted in this figure? Argon: this atom has 18 protons, meaning an atomic number of 18. referring to the Periodic Table, we can see that the element with an atomic number of 18 is Argon.

Which one of the following is a correct representation of an alpha particle? a. 42He b. 0-1e c. 10e d. 00

Which one of the following is a correct representation of an alpha particle? a. 42He b. 0-1e c. 10e d. 00

Following α decay, the total number of protons has a. increased by 2 b. decreased by 4 c. decreased by 2 d. unchanged

Following α decay, the total number of protons has a. increased by 2 b. decreased by 4 c. decreased by 2 d. unchanged

Following α decay, the atomic number has a. increased by 2 b. decreased by 4 c. decreased by 2 d. unchanged

Following α decay, the atomic number has a. increased by 2 b. decreased by 4 c. decreased by 2 d. unchanged

Following α decay, the atomic mass has a. increased by 2 b. decreased by 4 c. decreased by 2 d. unchanged

Following α decay, the atomic mass has a. increased by 2 b. decreased by 4 c. decreased by 2 d. unchanged

Alpha decay produces a new atom whose __________ than those of the original atom. a. atomic number is 2 less and atomic mass is 4 less b. atomic number is 2 less and atomic mass is 2 less c. atomic number is 2 more and atomic mass is 4 more d. atomic number is 2 more and atomic mass is 2 less

Alpha decay produces a new atom whose __________ than those of the original atom. a. atomic number is 2 less and atomic mass is 4 less b. atomic number is 2 less and atomic mass is 2 less c. atomic number is 2 more and atomic mass is 4 more d. atomic number is 2 more and atomic mass is 2 less

Which one of the following is a correct representation of a beta particle? a. 42He b. 0-1e c. 10e d. 00

Which one of the following is a correct representation of a beta particle? a. 42He b. 0-1e c. 10e d. 00

Following beta decay, the total number of protons has not changed decreased by 1 increased by 1 increased by 2

Following beta decay, the total number of protons has not changed decreased by 1 increased by 1 increased by 2

Following beta decay, the atomic mass has not changed decreased by 1 increased by 1 increased by 2

Following beta decay, the atomic mass has not changed decreased by 1 increased by 1 increased by 2

Following beta decay, the atomic number has not changed decreased by 1 increased by 1 increased by 2

Following beta decay, the atomic number has not changed decreased by 1 increased by 1 increased by 2

What happens to the atomic mass and atomic number of an atom when it undergoes beta (β) decay? a. The mass number increases by 2 and the atomic number increases by 1. b. The mass number decreases by 4 and the atomic number decreases by 2. c. The mass number does not change and the atomic number increases by 1. d. Neither the mass number nor the atomic number change.

What happens to the atomic mass and atomic number of an atom when it undergoes beta (β) decay? a. The mass number increases by 2 and the atomic number increases by 1. b. The mass number decreases by 4 and the atomic number decreases by 2. c. The mass number does not change and the atomic number increases by 1. d. Neither the mass number nor the atomic number change.

By what process does uranium-238 decay to thorium-234? a. alpha decay b. beta decay c. gamma ray emission d. electron capture

By what process does uranium-238 decay to thorium-234? a. alpha decay b. beta decay c. gamma ray emission d. electron capture Uranium 238 must have undergone alpha decay to produce thorium-234, since atomic mass has decreased by 4. Furthermore, according to the Periodic Table, uranium has an atomic number of 92, while thorium has an atomic number of 90. Therefore, atomic number has decreased by 2. The complete nuclear decay equation is: 23892U → 23490Th + 42He

What is the missing product from this nuclear decay reaction: 13755Cs → 13756Ba + _______________ a. 42He b. 0+1e c. 0-1e d. 00

What is the missing product from this nuclear decay reaction: 13755Cs → 13756Ba + _______________ a. 42He b. 0+1e c. 0-1e d. 00 Cesium-137 has an atomic number of 55, while Barium-137 has an atomic number of 56. Therefore, during this decay reaction, atomic number has gone up by one while atomic mass is unchanged. Such changes are characteristic of beta decay, thus the missing product is a beta particle. The complete nuclear decay equation is: 13755Cs → 13756Ba + 0-1e

Thorium undergoes alpha decay Thorium undergoes alpha decay. The product of this reaction also undergoes alpha decay. What is the final product of this second decay reaction __________ ?

Thorium undergoes alpha decay Thorium undergoes alpha decay. The product of this reaction also undergoes alpha decay. What is the final product of this second decay reaction _radon_ ? The problem tells you that two alpha decay events occur. Since atomic number decreases by two for each alpha decay event, the total decrease in atomic number will be 4. The starting thorium atom has an atomic number of 90. Subtracting 4 gives a final atomic number of 86. Referring to the Periodic Table, we can see that the element radon has an atomic number of 86.

What type of radioactive decay does not change the atomic number or atomic mass of an element? a. electron capture b. gamma ray emission c. alpha decay d. beta decay

What type of radioactive decay does not change the atomic number or atomic mass of an element? a. electron capture b. gamma ray emission c. alpha decay d. beta decay Gamma rays have no charge and no mass, being a wave rather than a particle, therefore the emission of gamma rays during decay affects neither atomic mass nor atomic number.

A 39Cl atom ejects a beta particle A 39Cl atom ejects a beta particle. What is the product of this reaction? a. 39Ar b. 39Cl c. 39S d. 38Ar

A 39Cl atom ejects a beta particle A 39Cl atom ejects a beta particle. What is the product of this reaction? a. 39Ar b. 39Cl c. 39S d. 38Ar Referring to the Periodic Table we can see that the atomic number of Cl is 17. We know that beta decay causes atomic number to increase by 1, therefore the final atomic mass is 18. Referring to the Periodic Table we see that argon (Ar) has an atomic mass of 18. We also know that beta emission causes no change in the atomic mass, therefore the specific isotope generated is argon-39 . The overall nuclear decay equestion is: 3917Cl  o-1e + 3918Ar

A 200 g sample of lawrencium is left in a container from 8:00 AM one morning until 2:00 PM the next afternoon. If the mass of the sample of lawrencium was 25 g, what is the half-life of lawrencium?? 10 hours 1 day 5 hours 30 hours

A 200 g sample of lawrencium is left in a container from 8:00 AM one morning until 2:00 PM the next afternoon. If the mass of the sample of lawrencium was 25 g, what is the half-life of lawrencium?? 10 hours 1 day 5 hours 30 hours Since we started with 200g, after the first half life, 100 g would remain, after the second half life 50 g would remain, and after the third half life 25 g would remain. Thus, the sample in this question has gone through 3 half lives. The total amount of time elapsed from 8:00 am day 1 through 2:00 PM day 1 is a total of 16 + 14 hours. Thus a total of 30 hours have passed. 30 hours divided by 3 half lives, gives a half-life time of 10 hours.

According to this graph, what is that half-life of radioactive material X? 5,000 years 10,000 years 15,000 years 20,000 years Time (X 1000 years)

The graph shows that 50 % of material is left after 5 X 1000 According to this graph, what is that half-life of radioactive material X? 5,000 years 10,000 years 15,000 years 20,000 years The graph shows that 50 % of material is left after 5 X 1000 years, which is equal to 5000 years. Time (X 1000 years)

Complete the following table to describe the decay of carbon-14. Half-life # Time in years Fraction of carbon-14 remaining in sample Mass of carbon-14 remaining in sample 1 100 g 5,700 50 g 2 ¼ 17,100 6.25 g 6

Complete the following table to describe the decay of carbon-14. Half-life # Time in years Fraction of carbon-14 remaining in sample Mass of carbon-14 remaining in sample 1 100 g 5,700 ½ 50 g 2 11,400 ¼ 25 g 3 17,100 1/8 12.5 g 4 22,800 1/16 6.25 g 5 28,500 1/32 3.125 g 6 34,200 1/64 1.562

¼ Consider the following table describing the decay of carbon-14. ½ Given that carbon-14 undergoes beta decay to form nitrogen-14, how much nitrogen-14 will be present in a sample of carbon-14 after 5,700 years, if that sample originally contained 40 g of carbon-14? Half-life # Time in years Fraction of carbon-14 remaining in sample Mass of carbon-14 remaining in sample 1 100 g 5,700 ½ 50 g 2 11,400 ¼ 25 g 3 17,100 1/8 12.5 g 4 22,800 1/16 6.25 g 5 28,500 1/32 3.125 g 6 34,200 1/64 1.562

¼ Consider the following table describing the decay of carbon-14. ½ Given that carbon-14 undergoes beta decay to form nitrogen-14, how much nitrogen-14 will be present in a sample of carbon-14 after 5,700 years, if that sample originally contained 40 g of carbon-14? 20 g of nitrogen-14 will be present in the sample after 5,700 years. We know that half of the carbon-14 sample will have decayed into nitrogen-14 by 5,700 years. We also know that during beta decay, atomic mass does not change. Therefore the mass of nitrogen produced will be equal to the mass of carbon-14 that has been lost. Since ½ of 40 g of carbon-14 = 20 g of carbon-14 decayed by year 5,700, the same mass of nitrogen-14 will have been generated by beta decay = 20 g of nitrogen-14 . Half-life # Time in years Fraction of carbon-14 remaining in sample Mass of carbon-14 remaining in sample 1 100 g 5,700 ½ 50 g 2 11,400 ¼ 25 g 3 17,100 1/8 12.5 g 4 22,800 1/16 6.25 g 5 28,500 1/32 3.125 g 6 34,200 1/64 1.562