1. What is the nuclear charge of an iron atom?
Multiple Choice F
iRespond Question
A.) +26
Iron has 26 protons in the nucleus each with a charge of +1. Neutrons have no charge. Electrons are outside of the nucleus.
B.) +30
C.) +56
D.) +82
E.)

2. What is the total number of electrons in a completely filled fourth principal energy level?
Multiple Choice F
iRespond Question
A.) 8
2n2
2(42)
2(16) = 32
B.) 10
C.) 16
D.) 32
E.)

3. How do the energy and the most probable location of an electron in the third shell of an atom compare to the energy and the most probable location of an electron in the first shell of the same atom?
iRespond Question F
Multiple Choice
A.) In the third shell, an electron has more energy and is closer to the nucleus.
B.) In the third shell, an electron has more energy and is farther from the nucleus.
C.) In the third shell, an electron has less energy and is closer to the nucleus.
D.) In the third shell, an electron has less energy and is farther from the nucleus.
E.)

4. How many protons, electrons, and neutrons does an atom of Tin have?
iRespond Question F
Multiple Choice
A.) 50 protons, 50 electrons, 50 neutrons
B.) 50 protons, 50 electrons, 69 neutrons
C.) 50 protons, 69 electrons, 50 neutrons
D.) 50 protons, 69 electrons, 69 neutrons
E.) none of the above

5. What is the total number of electrons found in an atom of sulfur?
Multiple Choice F
iRespond Question
A.) 6
Sulfur has an atomic number of 16 (16 protons). It will have an equal number of electrons to balance the charge.
B.) 8
C.) 16
D.) 32
E.)

6. How many energy sublevels are in the second principal energy level?
Multiple Choice F
iRespond Question
A.) 1
Each energy level as many sublevels as its number. The second energy level has 2 (s and p)
B.) 2
C.) 3
D.) 4
E.)

7. What types of atomic orbitals are in the third principal energy level?
Multiple Choice F
iRespond Question
A.) s and p only
Each energy level has as many sublevels as its number. The third energy level has 3.
B.) p and d only
C.) s, p, and d only
D.) s, p, d, and f
E.)

8. Which sublevel contains a total of 5 orbitals?
Multiple Choice F
iRespond Question
A.) s 1 3 5 7
B.) p
C.) d
D.) f
E.)

9. The total number of orbitals in a p sublevel is
Multiple Choice F
iRespond Question
A.) 1 s p d f
B.) 3
C.) 5
D.) 7
E.)

10. Which principal energy level has no f sublevel?
Multiple Choice F
iRespond Question
A.) 3
Each energy level has as many sublevels as its number. The third energy level only has 3 sublevels (s,p, and d)
B.) 4
C.) 5
D.) 6
E.)

11. What is the maximum number of electrons that can be found in an energy levels p sublevel?
iRespond Question F
Multiple Choice
A.) 2
B.) 3
The p sublevel has 3 orbitals, each of which can hold a maximum of 2 electrons
C.) 5
D.) 6
E.) 10

12. The superscripts represent the number of electrons
How many electrons are present in the atom with electronic structure 1s22s22p63s1?
Multiple Choice F
iRespond Question
A.) 88
The superscripts represent the number of electrons
B.) 8
C.) 6
D.) 11
E.) 12

13. Which orbital notation represents a boron atom in the ground state?
iRespond Question
Multiple Choice F
Must fill lowest energy level first
Must fill lowest energy level first
Must fill lowest energy level first
E.)
A.) 1
C.) 4
B.) 3
D.) 5

14. The superscripts add up to 20 electrons.
Assuming that the atom is neutral, identity the element with electronic structure 1s22s22p63s23p64s2
Multiple Choice F
iRespond Question
A.) K
The superscripts add up to 20 electrons.
B.) Ar
C.) Ca
D.) Mg
E.) Cr

15. Superscripts must add up to 13
If an atom has 13 electrons, which of the following represent the electron configuration?
Multiple Choice F
iRespond Question
A.) 1s22s22p63s23p6
Superscripts must add up to 13
B.) 1s22s22p63s23p1
C.) 1s22s22p63s23p4
D.) 1s22s22p63s23p2
E.)

16. Which one of the following represents the energy level diagram for carbon?
Multiple Choice
iRespond Question F A C
Aufbau /
Hund
Aufbau B D
Hund
E.)
B.)
D.)
A.)
C.)

17. In the electron cloud model, an orbital is a region of space in an atom where there is
iRespond Question F
Multiple Choice
A.) a high probability of finding an electron
B.) a high probability of finding a neutron
C.) a circular path in which electrons are found
D.) a circular path in which neutrons are found
E.)

18. What is the next atomic orbital in the series 1s, 2s, 2p, 3s, 3p?
iRespond Question F
Multiple Choice
A.) 2d
B.) 3d
C.) 3f
D.) 4s
E.)

19. What is the highest energy level assigned to an electron in an atom of zinc in the ground state?
Multiple Choice F
iRespond Question
A.) 1
Zinc is in the fourth row and has electrons in four energy levels
B.) 2
C.) 3
D.) 4
E.)

20. Locate in the periodic table the element that has the first 4d electron.
iRespond Question F
Multiple Choice
A.) Sc
B.) La
C.) Ga
D.) Y
E.) K

21. What is the electron configuration of potassium?
iRespond Question
Multiple Choice
2p2 and only 11e-
A.) 1s22s22p23s23p24s1
1s1 and only 18e-
B.) 1s12s22p103s23p3
No 2p and only 13e-
C.) 1s22s23s23p63d1
D.) 1s22s22p63s23p64s1
E.)

22. What is the electron configuration of a Mn atom in the ground state?
Multiple Choice
iRespond Question
A.) 1s22s22p63s2
Only 12e-
B.) 1s22s22p63s23p64s23d5
C.) 1s22s22p63s23p64s13d54p1
4s1 and 3d5
D.) 1s22s22p63s23p63d7
4s before 3d
E.)

23. What is represented by the dots in a Lewis electron dot diagram of an atom of an element in Period 2 of the Periodic Table?
iRespond Question F
Multiple Choice
A.) the number of neutrons in the atom
B.) the number of protons in the atom
C.) the number of valence electrons in the atom
D.) the total number of electrons in the atom
E.)

24. What is the total number of valence electrons in an atom of boron in the ground state?
iRespond Question F
Multiple Choice
A.) 1
B.) 3
C.) 5
D.) 7
E.)

25. How many electrons are in the outermost principal energy level of an atom of carbon in the ground state?
iRespond Question F
Multiple Choice
A.) 2
B.) 3
C.) 4
D.) 6
E.)

26. What is the total number of valence electrons in an atom of sulfur in the ground state?
iRespond Question F
Multiple Choice
A.) 3
B.) 4
C.) 6
D.) 8
E.)

27. Which of the following atoms has three unpaired electrons?
Multiple Choice
iRespond Question F
A.) Boron B
B.) Carbon C
C.) Nitrogen N
D.) Oxygen O
E.)

28. Which electron-dot symbol represents an atom of chlorine in the ground state?
iRespond Question
Multiple Choice F
E.)
D.) 1
B.) 1
A.) 1
C.) 1

29. There is not change in the number of electrons, just their location
Compared to a sodium atom in the ground state, a sodium atom in the excited state must have
iRespond Question
Multiple Choice F
There is not change in the number of electrons, just their location
A.) a greater number of electrons
B.) a smaller number of electrons
C.) an electron with greater energy
D.) an electron with less energy
E.)

30. Which electron configuration is possible for a nitrogen atom in the excited state?
Multiple Choice
iRespond Question
A.) 1s22s22p3
Ground
B.) 1s22s22p23s1
C.) 1s22s22p4
Oxygen
D.) 1s22s22p2
Carbon
E.)

31. Which electron configuration represents a potassium atom in the excited state?
Multiple Choice
iRespond Question
A.) 1s22s22p63s23p3
Phosphorous
B.) 1s22s22p63s13p4
Excited Phosphorous
C.) 1s22s22p63s23p64s1
Chlorine
D.) 1s22s22p63s23p54s2
E.)

32. The farther from the nucleus the greater the energy
Which electron transition represents a gain of energy?
iRespond Question
Multiple Choice F
The farther from the nucleus the greater the energy
A.) from 2nd to 3rd shell
B.) from 2nd to 1st shell
C.) from 3rd to 2nd shell
D.) from 3rd to 1st shell
E.)

33. High to low releases energy
The characteristic bright-line spectrum of an element occurs when electrons
iRespond Question F
Multiple Choice
A.) move from lower to higher energy levels
B.) move from higher to lower energy levels
C.) are lost by a neutral atom
D.) are gained by a neutral atom
High to low releases energy
E.)

34. The characteristic spectral lines of elements are caused when electrons in an excited atom move from
iRespond Question F
Multiple Choice
A.) lower to higher energy levels, releasing energy
B.) lower to higher energy levels, absorbing energy
C.) higher to lower energy levels, releasing energy
D.) higher to lower energy levels, absorbing energy
E.)

35. Electron X can change to a higher energy level or a lower energy level
Electron X can change to a higher energy level or a lower energy level. Which statement is true of electron X?
iRespond Question F
Multiple Choice
A.) Electron X emits energy when it changes to a higher energy level.
B.) Electron X absorbs energy when it changes to a higher energy level.
C.) Electron X absorbs energy when it changes to a lower energy level.
D.) Electron X neither emits nor absorbs energy when it changes energy level.
E.)

36. Which of the following quantum leaps would be associated with the greatest energy of emitted light?
iRespond Question F
Multiple Choice
A.) n = 5 to n = 1
B.) n = 4 to n = 5
C.) n = 2 to n = 5
D.) n = 5 to n = 4
E.)

37. Each element has a unique spectra that is unchanged based on locations
The atomic emission spectra of a sodium atom on Earth and of a sodium atom in the sun would be
iRespond Question F
Multiple Choice
A.) the same
B.) different from each other
C.) the same as those of several other elements
D.) the same as each other only in the ultraviolet range
Each element has a unique spectra that is unchanged based on locations
E.)

38. Which two elements are present in the unknown spectra below?
iRespond Question F
Multiple Choice
A.) Li & H
B.) Li & Na
C.) H & He
D.) Li & He
E.)