Name: _______________________
Period: _____ Date: ____________
1. Explain what each number letter means in the following notation: 3p 6 a. 3 – b. p
– c. 6 –
2. Describe the first four energy levels. a. Which shape orbitals does each energy level contain?
1:
2:
3:
4: b. How many total orbitals does this energy level contain?
1:
2:
3:
4:
Chapter 4 & 5 ( 1) | P a g e

Name: _______________________
Period: _____ Date: ____________ c. How many total electrons can occupy this energy level?
1:
2:
3:
4:
3. Fill in the blanks. a. The 5f orbitals can hold a maximum of _____ electrons. b. The 4s orbital can holds a maximum of _____ electrons.
4. How many electrons can occupy each of the following: a. 2p orbitals: _____ b. A single 5d orbital: _____ c. 3s orbital: _____ d. 5d orbitals: _____
Chapter 4 & 5 ( 2) | P a g e

Name: _______________________
Period: _____ Date: ____________
1. Name the elements from the electron configurations: a. 1s 2 2s 2 2p 6 3s 2 3p 5 _____________________ b. 1s 2 2s 2 2p 6 3s 2 3p 6 4s 2 3d 10 4p 6 5s 2 _____________________ c. [Kr] 5s 2 4d 10 5p 4 d. [Xe] 6s 2 4f 14 5d 7
_____________________
_____________________
2. Which of the three rules is being violated in these orbital notations. Your answer will be either Hund’s rule, Aufbau principle, or Pauli exclusion principle a.
  
__ __
1s 2s 2p
_________________________ b.
    
___
 
_

_
1s 2s 2p 3s 3p
_________________________ c.
        
_
1s 2s 2p 3s 3p
_________________________ d.              
1s 2s 2p 3s 3p 3d
_________________________
Chapter 4 & 5 ( 3) | P a g e

Name: _______________________
Period: _____ Date: ____________
Write the orbital notations ( using arrows) for the following elements:
3. Magnesium_______________________________________________
4. Cobalt__________________________________________________
5. Krypton_________________________________________________
6. Beryllum_________________________________________________
7. Scandium________________________________________________
Write the electron configurations of the following elements.
8. Nickel___________________________________________________
9. Cadmium_______________________________________________
10. Selenium_______________________________________________
11. Strontium________________________________________________
12. Lithium____________________________________________
Chapter 4 & 5 ( 4) | P a g e

Name: _______________________
Period: _____ Date: ____________
Write the Noble gas notation for the elements from questions 12-16
13. Nickel___________________________________________________
14. Cadmium_______________________________________________
15. Selenium_______________________________________________
16. Strontium________________________________________________
17. Lithium____________________________________________
Determine whether the following electron configurations are valid. Your answer will be either valid or invalid.
18. 1s 2 2s 2 2p 6 3s 2 3p 6 4s 2 4d 10 4p 6 __________________
19. [Rn] 7s 2 5f 9 __________________
20. [He]3s 2 3p 1
21. [Ne] 3p 5 3s 2
__________________
__________________
Chapter 4 & 5 ( 5) | P a g e

Name: _______________________
Period: _____ Date: ____________
Chapter 4 & 5 ( 6) | P a g e

Name: _______________________
Period: _____ Date: ____________
Write the formulas for the following covalent compounds:
1) antimony tribromide _________________________________________________
2) hexaboron monosilicide ______________________________________________
3) chlorine dioxide ___________________________________________________
4) hydrogen moniodide_________________________________________________
5) iodine pentaflouride ________________________________________________
6) dinitrogen trioxide _________________________________________________
7) nitrogen trihydride ___________________________________________________
8) phosphorus triiodide _________________________________________________
Chapter 4 & 5 ( 7) | P a g e

Name: _______________________
Period: _____ Date: ____________
Write the names of the following covalent compounds:
9) P
4
S
5
_____________________________________________
10) ClO
2
________________________________________________
11) SeF
6
_______________________________________________
12) Si
2
Br
6
_____________________________________________
13) SCl
4
_______________________________________________
14) CH
4
_______________________________________________
15) B
2
Si _______________________________________________
16) NF
3 ________________________________________________________________________
Chapter 4 & 5 ( 8) | P a g e

Name: _______________________
Period: _____ Date: ____________
SHORT ANSWER - Answer the following questions in the space provided.
1. Elements in the periodic table are arranged by increasing ____________________.
2. State the periodic law: ________________________________________________
__________________________________________________________________
__________________________________________________________________
3. When the noble gases were discovered, a new ____________________ was added to the periodic chart.
4. Give two traits of noble gases: a.
__________________________________________________ b.
__________________________________________________
5. Berylium, the first element in Group 2, has an atomic number of 4. The second
element in this group has an atomic number of ______________.
6. An isotope of oxygen has a mass number of 15 and an atomic number of 8.
______ a. How many protons are in this atom?
______ b. How many neutrons are in this atom?
7. Promethium, Pm, is a member of the lanthanide series.
a. Identify the element just below promethium
in the periodic table.
__________________________ b. The atomic numbers of these two elements
differ by how many units?
8. A certain isotope contains 46 protons, 62 neutrons, and 45 electrons.
a. What is its atomic number?
b. What is the mass number of this atom?
c. Is this element Rh, Pd, Sm, or Hs?
d. Identify two other elements that are in its group.
Chapter 4 & 5 ( 9) | P a g e

Name: _______________________
Period: _____ Date: ____________
9. In the periodic table, the atomic masses of Co and Ni decrease rather than
increase, while their atomic numbers increase. Find two other pairs of
neighboring atoms where this occurs.
________________________________________________________________________
10. Give the symbol, period, group, and block for the following:
Arsenic
Symbol Period Group Block
Palladium
[Ar]4s 2
[Ar4s 2 3d 5
11. There are 18 columns in the periodic table; each has a group number. Give the group numbers that make up each of the following blocks:
___________________________ a. s block
___________________________ b. p block
___________________________ c. d block
12. Who is credited with creating the basis of the modern periodic chart:
_________________
13. Consider the electron configuration: 1s 2 2s 2 2p 6 3s 2 3p 6 4s 2 3d 10 4p 4 .
_______________ a. To which period does the element belong?
_______________ b. To what group does it belong?
_______________ c. How many valence electrons does it have?
14. _______________Metalloids are found in which block, s , p , d , or f ?
15. _______________The softest metals are found in which block s , p , d ,
or f ?
Chapter 4 & 5 ( 10) | P a g e

Name: _______________________
Period: _____ Date: ____________
16. _______________ a. Name the most chemically active halogen.
_______________ b. Write its electron configuration.
_______________ c. Write the configuration of the most-stable ion this
element makes.
17. _______________ Identify all of the ions below that do not have noble gas stability:
K + S 2- Ca + I Al 3+
Give the noble-gas notation of the following:
________________________ a. Br
________________________ b. Br
–
________________________ c. the element in Group 13, Period 5
18. Rank the following elements by increasing atomic radius:
C, Al, O _________________________________
19. Rank the following elements by increasing electronegativity:
S, O,Al _________________________________
20. Rank the following elements by increasing ionization energy:
S, F, Se _________________________________
21. Rank the following elements by increasing electron affinity:
Cl, Na, Cs _________________________________
22. Why does oxygen have a higher ionization energy than selenium?
__________________________________________________________
__________________________________________________________
Chapter 4 & 5 ( 11) | P a g e

Name: _______________________
Period: _____ Date: ____________
Chapter 4 & 5 ( 12) | P a g e

Name: _______________________
Period: _____ Date: ____________
Write the orbital notation for the following elements
1) Oxygen
______________________________________________________
2) Calcium
______________________________________________________
3) Aluminum
______________________________________________________
Write the electron configurations of the following elements:
4) Molybdenum
______________________________________________________
5) Chlorine
______________________________________________________
6) Potassium
______________________________________________________
Write the Noble Gas configurations for the following elements.
7) Strontium
______________________________________________________
8) Molybdenum
______________________________________________________
Determine what elements are denoted by the following electron configurations:
9) 1s 2 2s 2 2p 4 ____________________
10) 1s 2 2s 2 2p 6 3s 2 3p 6 4s 1 _____________________
Chapter 4 & 5 ( 13) | P a g e

Name: _______________________
Period: _____ Date: ____________
11) [Kr] 5s 2 4d 9 ___________________
12) [Xe] 6s 2 4f 14 5d 3 ___________________
13) Rank the following elements in increasing order.
_______________ a. Radius: Se, Ca, Co?
_______________ b. Electronegativity: Ge, C, Sn?
_______________ c. Electronegativity: Os, Tl, Cs
_______________ d. Ionization energy: As, Cl, Ra?
_______________ e. Ionization energy: Si, Cl, Mg
_______________ f. Electron affinity: C, F, K
_______________ g. In general, which has a stronger electron attraction, large
atoms or small atoms?
_______________ h. How many valence electrons are there in a neutral atom of
Sr?
_______________ i. How many valence electrons are there in a neutral atom of
Se?
14) Consider a neutral atom with 42 protons and 54 neutrons to answer the
following questions.
_______________ a. What is its atomic number?
_______________ b. Is the element’s position in a modern periodic table determined by its atomic number or by its atomic mass?
_______________ c. To what block of the periodic table does it belong
Chapter 4 & 5 ( 14) | P a g e

Name: _______________________
Period: _____ Date: ____________
15) Determine which element best fits the following statements using the
elements : Zn, Si, Sr, Ar.
Element found in the p block: ____________________
Has the largest atomic number: ___________________
Alkaline earth metal: ______________
Noble gas: ________________
Found in period 4: ________________
Found in group 14: _______________
Has the highest electronegativity: ______________
Has electrons in the 5s: ______________
Has an octet in its outer shell: ____________
Has unpaired electrons: _____________
16) Describe what each of the four quantum numbers represent:
Principle - ______________________________________________________
____________________________________________________________
Angular Momentum -_____________________________________________
____________________________________________________________
Magnetic - _____________________________________________________
____________________________________________________________
Spin - _________________________________________________________
____________________________________________________________
Naming:
17) Phosphorus trichloride: ________________
18) Manganese (V) fluoride: ________________
19) Sulfur hexafluoride: ________________
20) Dinitrogen monoxide: ________________
21) Sodium iodite: ________________________
Chapter 4 & 5 ( 15) | P a g e

Name: _______________________
Period: _____ Date: ____________
________________________ 22) Selenium dibromide:
23) Aluminum acetate:
24) NO
2
:
25) CBr
4
:
26) ZnSO
3
:
27) SO
3
:
28) OCl
2
:
29) SiF
4
:
30) Au
2
O:
31) P
4
O
10
:
________________________
_________________________
_________________________
_________________________
_________________________
_________________________
_________________________
_________________________
_________________________
32) UF
6
:
33) CSe
2
:
_________________________
___________________________
34) How many atoms are present in 72 grams of MgCl
2
?
35) How many moles are present in 8.20 x 10 4 cg of N
2
O
5
?
Atoms: __________
Moles: __________
Chapter 4 & 5 ( 16) | P a g e