Name: _____________________________________________________________________________ Period: ____ Date: ________________________
Unit 7: Bonding Test Review Sheet
Periodic Trends:
1. Define:
a) Ionization energy
b) Electronegativity
2. Atomic radius INCREASES or DECREASES as you go down a group, because:
Atomic radius INCREASES or DECREASES as you go left to right across a period, because:
Electronegativity INCREASES or DECREASES as you go down a group, because:
Electronegativity INCREASES or DECREASES as you go left to right across a period, because:
Ionization energy INCREASES or DECREASES as you go down a group, because:
Ionization energy INCREASES or DECREASES as you go left to right across a period, because:
3. On the periodic table below, draw labeled arrows to show the direction of increasing atomic radius, electronegativity, and ionization
energy.
4. Group 1 elements
GAIN or LOSE ____
electron(s) to form an
ion with a _______ charge.
Group 2 elements GAIN or LOSE ____ electron(s) to form an ion with a _______ charge.
Group 6 elements GAIN or LOSE ____ electron(s) to form an ion with a _______ charge.
Group 7 elements GAIN or LOSE ____ electron(s) to form an ion with a _______ charge.
Shorthand Electron Configuration:
5. Write the shorthand electron configuration for the following:
Mg ________________________________________________________________
Fe ________________________________________________________________
Br- ________________________________________________________________
Al3+________________________________________________________________
Types of Bonds:
6. Ionic bonds:
a) Electrons are _________________________________________, and atoms in the bond are attracted to each other because
b) Are formed between a ___________________________ and a _______________________________.
c) Are formed between two atoms that have a electronegativity difference of close to 0, between 0.4-2, or >2
7. Non-polar covalent bonds:
a) Electrons are ______________________________________________________.
b) Are formed between a ___________________________ and a _______________________________.
c) Are formed between two atoms that have a electronegativity difference of close to 0, between 0.4-2, or >2
8. Polar covalent bonds:
a) Electrons are ______________________________________________________.
b) Are formed between a ___________________________ and a _______________________________.
c) Are formed between two atoms that have a electronegativity difference of close to 0, between 0.4-2, or >2
9. Use the table of electronegativities provided to classify the
following bonds as ionic, nonpolar covalent, or polar covalent.
a) H-F
______________________
b) C-O
______________________
c) C-H
______________________
d) K-Cl
______________________
e) MgBr2
______________________
Lewis Structures
10. Draw lewis structures for the following neutral atoms:
K
Ar
N
11. Draw lewis structures for the following ions:
K+
Ca2+
Cl-
12. Draw lewis structures for the following ionic compounds:
Kl
MgCl2
LiBr
13. Draw lewis structures for the following covalent compounds:
CH4
H-F
H2CO
14. Draw lewis structures for the following polyatomic ions:
SO32-
HCO3-
NH4+
15. A line in a Lewis Structure represents ____ electrons.
16. Define “lone pair”:
17. What is the total valence electron count for the following:
CO2 : ______________
H3O+ : ______________
18. Draw the resonance structure for the ion: NO3-
VSEPR
19. Define and describe how VSEPR theory defines the shape of a molecule:
20. Draw the lewis structures for the molecules below, then classify their shape by using the table of shapes.
CF4
CO2
NH3
Shape:
Shape:
Shape:
21. Use VSEPR to explain why water has a bent shape as opposed to linear. Draw a picture to support your answer.
Polar molecules:
22. What is the difference between a polar molecule and a nonpolar molecule?
23. Draw a lewis structure of a water molecule. Make sure you draw the molecule with the correct shape (from #21 above).
Label where the molecule is partially negative (�-) and partially positive (�+).
24. Add three (3) more water molecules to your diagram above, and draw in hydrogen bonds by using dotted lines.
25. Draw in the dipole moment as a net vector of charge (⤉) on your water molecule above.
26. Describe how a molecule’s polarity affects its:
a) Solubility in water
b) Intermolecular forces/surface tension
c) Melting and boiling points