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CHAPTER 8 REGULAR HOMEWORK:

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Question 1

Give the number of unpaired electrons present in a ground-state atom of Fe.
Hint given in feedback

Correct

 

Explanation

 

Question 2

Give the number of unpaired electrons present in a ground-state atom of S.
Hint given in feedback

Correct


 

Explanation

  

 

Question 3

Give the number of unpaired electrons present in a ground-state atom of Fe2+.


Correct

 

Explanation

  

 

Question 4

Give the number of unpaired electrons present in a ground-state of the ion formed when one electron is ionized from an O atom to form the O+ ion


Correct

 

Explanation

Summarizing Atomic Radii for Main-Group Elements:

  • As we move down a column in the periodic table, the principal quantum number (n) of the electrons in the outermost principal energy level increases, resulting in larger orbitals and therefore larger atomic radii.
  • As we move to the right across a row in the periodic table, the effective nuclear charge experienced by the electrons in the outermost principal energy level increases, resulting in a stronger attraction between the outermost electrons and the nucleus, and smaller atomic radii.

 

Question 5

Give the number of unpaired electrons present in a ground-state atom of Se2- .

Correct

 

Explanation

Summarizing Atomic Radii for Main-Group Elements:

  • As we move down a column in the periodic table, the principal quantum number (n) of the electrons in the outermost principal energy level increases, resulting in larger orbitals and therefore larger atomic radii.
  • As we move to the right across a row in the periodic table, the effective nuclear charge experienced by the electrons in the outermost principal energy level increases, resulting in a stronger attraction between the outermost electrons and the nucleus, and smaller atomic radii.

 

Question 6

Using the abbreviated notation, the ground-state electron configuration of Y3+ is

Select one:
 Correct

 

Explanation

Summarizing Atomic Radii for Main-Group Elements:

  • As we move down a column in the periodic table, the principal quantum number (n) of the electrons in the outermost principal energy level increases, resulting in larger orbitals and therefore larger atomic radii.
  • As we move to the right across a row in the periodic table, the effective nuclear charge experienced by the electrons in the outermost principal energy level increases, resulting in a stronger attraction between the outermost electrons and the nucleus, and smaller atomic radii.

 Y = 39 electrons

Y3+  = 36 electrons   ----->  Kr (36 electrons) 

 

Question 7

Using the abbreviated notation, the ground-state electron configuration of Br- is

Select one:
 Correct

 

Explanation

 

  

Br: 35 electrons

Br - = 36 electrons ---> Kr (36 electrons)

 

Question 8

Using the abbreviated notation, the ground-state electron configuration of Rh 2+  is

Select one:
 Correct

 

Explanation

 Rh: 45 electrons

 Rh2+ : 43 electrons

Rh 2+ :  [Kr] 4d7



 

Question 9

Which electron configuration represents the most highly excited state of C?

Select one:
 Correct

 

Explanation

 Protons Electrons
 F 99  strongest attraction to nucleus (smallest)
 F -19  10 weaker attraction to nucleus (medium)
 O 2- 8 10 weakest attraction to nucleus (largest)
 

Question 10

Write the electron configuration of the copper atom and the 2+ cation of copper. Check the correct choices.

Select one or more:
 Correct
 Correct

 

Explanation

 

Question 11

Arrange the elements lithium, carbon, and oxygen in order of increasing number of unpaired electrons. (There are two correct choices since 2 have the same number.)

Select one or more:
 Correct
 Correct

 

 

Explanation

Li: 1 unpaired electron

C: 2 unpaired electrons

O: 2 unpaired electrons

 

Question 12

In the reaction of lithium with oxygen, what expected compound is formed? If the compound is written LixOy, what is x+y? For example, water is H2O. In this case x =2, y = 1, and you write 3 in the space provided for the answer.

Correct

 

Explanation

 Li2O = 2+1 = 3

 

Question 13

Write the equation for the reaction, if any, of lithium with nitrogen. If there is a reaction forming LixNy, what is x+y?

Correct

 

Explanation

 

 

Question 14

Write the electron configuration of the alkali metal (M) that reacts with oxygen to yield an oxide, M2O, if 1.22 g of the metal reacts with 1.41 g of oxygen to form 2.63 g of the oxide.

Select one:
 Correct

 

Explanation

29.85 g - 16.0g (Oxygen) = 13.85g

13.85 / 2 (Metal) = 6.925g


Li (Molar Mass) = 6.9


 

Question 15

In the reaction of iron and chlorine, what mass of iron is needed to prepare 22.97 g of the iron chloride product if, under the conditions of the reaction, the electron configuration of the iron cation in the product is 1s22s22p63s23p63d6?


Correct

 

Explanation

Fe = +2 (loss 2 electrons)


Final product = FeCl2
Fe + Cl2 -> FeCl2

Molecular mass of FeCl2 is 126.48 

needed to prepare 22.97 g of the iron chloride product


22.97/ 126.48 = 0.1816 mol


Mass of Iron (55.58 g/mol) x (0.1816 mol) = 10.1 g

 

 

Question 16

Using only a periodic table as a guide, arrange each of the following series of atoms in order of increasing size.

Select one:
 Correct

 

Explanation

Summarizing Atomic Radii for Main-Group Elements:

  • As we move down a column in the periodic table, the principal quantum number (n) of the electrons in the outermost principal energy level increases, resulting in larger orbitals and therefore larger atomic radii.
  • As we move to the right across a row in the periodic table, the effective nuclear charge experienced by the electrons in the outermost principal energy level increases, resulting in a stronger attraction between the outermost electrons and the nucleus, and smaller atomic radii.

 

 

Question 17

Using only a periodic table as a guide, arrange each of the following series of atoms in order of increasing size.\

Select one:
 Correct

 

Explanation

 

  

Summarizing Atomic Radii for Main-Group Elements:

  • As we move down a column in the periodic table, the principal quantum number (n) of the electrons in the outermost principal energy level increases, resulting in larger orbitals and therefore larger atomic radii.
  • As we move to the right across a row in the periodic table, the effective nuclear charge experienced by the electrons in the outermost principal energy level increases, resulting in a stronger attraction between the outermost electrons and the nucleus, and smaller atomic radii.

 

Question 18

Using only a periodic table as a guide, arrange each of the following series of atoms in order of increasing size.

Select one:
 Correct

 

Explanation

 

  

Summarizing Atomic Radii for Main-Group Elements:

  • As we move down a column in the periodic table, the principal quantum number (n) of the electrons in the outermost principal energy level increases, resulting in larger orbitals and therefore larger atomic radii.
  • As we move to the right across a row in the periodic table, the effective nuclear charge experienced by the electrons in the outermost principal energy level increases, resulting in a stronger attraction between the outermost electrons and the nucleus, and smaller atomic radii.

 

Question 19

Using only a periodic table as a guide, arrange each of the following series of species in order of increasing size.

Select one:
 Correct

 

Explanation

 Protons Electrons
 F 99  strongest attraction to nucleus (smallest)
 F -19  10 weaker attraction to nucleus (medium)
 O 2- 8 10 weakest attraction to nucleus (largest)
 

Question 20

Using only a periodic table as a guide, arrange each of the following series of species in order of increasing size.

Select one:
 Correct

 

Explanation

 Protons Electrons
Al 3+1310  strongest attraction to nucleus (smallest)
Mg1212right across a row in the periodic table radius becomes smaller
Na1111moving left across the periodic table radius becomes larger

 

Question 21

Using only a periodic table as a guide, arrange each of the following series of species in order of increasing size.

Select one:
 Correct

 

Explanation

 

Question 22

Indicate which species in each pair has the higher ionization energy.
Select one or more:
 Correct
 Correct
 Correct
 Correct

 

Explanation

Ionization Energy - required energy to remove an electron from orbital

  • First ionization energy  decreases as we move down a column (or family) in the periodic table because electrons in the outermost principal level are increasingly farther away from the positively charged nucleus and are therefore held less tightly.
  • First ionization energy increases as we move to the right across a row (or period) in the periodic table because electrons in the outermost principal energy level generally experience a greater effective nuclear charge

 

 

Question 23

Using only a periodic table as a guide, arrange each of the following series of species in order of increasing first ionization energy.

Select one:
 Correct

 

Explanation

 

Question 24

Using only a periodic table as a guide, arrange each of the following series of species in order of increasing first ionization energy.

Select one:
 Correct

 

Explanation

 

Question 25

Using only a periodic table as a guide, arrange each of the following series of species in order of increasing first ionization energy.

Select one:
 Correct

 

Explanation

 

 

Question 26

Which ground-state electron configuration represents the element with the largest size?

Select one:
 Correct

 

Explanation

The electron configuration with least amount of electrons has the largest size. As the number of electrons increases the attraction toward the nucleus increases causing the atom size to become smaller. 

 

Question 27

Which ground-state electron configuration represents the element with the smallest ionization energy?

Select one:
 Correct

 

Explanation

The electron configuration with least amount of electrons has the largest size. Therefore it is requires the least amount of ionization energy to remove an electron because it is least closest to the nucleus.

 

 

Question 28

Which ground-state electron configuration represents the element with the most negative electron affinity?

Select one:
 Correct

 

Explanation

 

Electron affinity generally becomes more negative (adding an electron becomes more exothermic) as we move to the right across a period (row) in the periodic table.
 

Question 29

Arrange the elements lithium, carbon, and oxygen in order of increasing size.

Select one:
 Correct

 

Explanation

 

Question 30

Arrange the elements lithium, carbon, and oxygen in order of increasing first ionization energy.

Select one:
 Correct

 

Explanation

 

 

Question 31

Arrange the elements lithium, carbon, and oxygen in order of increasing second ionization energy.

Select one:
 Correct

 

Explanation

count the ionization energy by the number the elements prior to the select element. 

 

 

Question 32

Write the equation for the reaction, if any, of lithium with water. What products are formed?

Select one or more:
 Correct
 Correct
 Correct

 

Explanation

 

2Li + H2O = Li2O + H2 = Li + OH + H
 

Question 33

Which of the following reactions produce H2 gas?

Select one or more:
 Correct
 Correct

 

Explanation

 

Question 34

Write the electron configuration of the alkali metal (M) that reacts with oxygen to yield an oxide, M2O, if 1.22 g of the metal reacts with 1.41 g of oxygen to form 2.63 g of the oxide.

Select one:
 Correct


 

Explanation

Hint, determine the molecular weight of the metal.

 

Question 35

In the reaction of iron and chlorine, what mass of iron is needed to prepare 3.85 g of the iron chloride product if, under the conditions of the reaction, the electron configuration of the iron cation in the product is 1s22s22p63s23p63d6?

Correct


 

Explanation

Procedure: (1) Determine what the iron chloride is. (2) Go from grams iron chloride to moles of iron chloride to moles Fe to grams Fe.

 

Question 36

Which of the following reactions produce H2 gas?
Select one or more:

 Correct
 Correct

 

Explanation

  Explained Above

 

Question 37

Which of the following reactions produce a basic solution (the hydroxide ion)?
Select one or more:

 Correct
 Correct
 Correct

 

Explanation

 A basic solutions contains OH ions

  •  Na(s) + cold water               all contain OH ions in final product
  •            
  •  Na2O + cold water


 

Question 38

Which of the following reactions produces iron, the metal?
Select one:

 Correct

 

Question 39

Which of the following reactions produces chlorine gas?
Select one:

 Correct

 

Explanation

 

2FeCl3 + 3F2 = 2FeF3 + 3Cl2
 

Question 40

Match oxides with correct property.

CaO Correct
K2O Correct
CO2 Correct
N2O5 Correct
Al2O3 Correct

 

Explanation

 


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