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Ch. 7-8 Review Sheet

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1. What are the properties of IONIC substances?

These substances:-Solid Hard and brittle (like salt) at room temp-Conduct electricity when dissolved in water -High boiling/melting points

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2. What are the properties of COVALENT substances?

These substances:-MOST are liquids/gases at room temp-Do not conduct electricity when dissolved in

water -Most can not dissolve in water-Low boiling/melting points

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3. What’s the difference between ionic BONDING and covalent BONDING?

Ionic CovalentTransfer electrons Shared electrons

Metal/nonmetals Nonmetals

Has a charge No charge

Single bonds only Can have double/triple bonds

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4. Why do atoms form bonds?

Atoms are trying to fill their valence orbit with a stable octet of electrons- in the case of hydrogen it’s a duet

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5. What are diatomic molecules? Name 7 of them.

Diatomic molecules are molecules that are made up of 2 identical atoms to become a molecule.H2, N2, O2, F2, Cl2, Br2, I2

KNOW THESE!!!~!!!

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6. How many electrons are involved in covalent bonding?____

2 shared electrons or a pair of electrons

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7. What is bond dissociation energy?

The energy needed to separate a covalent bond

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8. What properties determine bond strength?

C-C longer and weakerO=O not so long and strongerN=N short and strong

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9. Provide the Lewis structure, the VSEPR shape and determine the polarity for the following

Lewis Structure

VSEPR shape IMF

SO3

CI4

SeO2

HF

Trig planar DD

Dispersion

HB

DD

Tetrahedral

Bent

Iinear

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10. What are the 10 prefixes to molecular compound naming?

Mono- 1Di- 2Tri- 3Tetra- 4Penta- 5Hexa- 6Hepta- 7Octa- 8Non-9 Deca- 10

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11. What is the difference between a nonpolar covalent bond and a polar covalent bond?

Provide an example.Nonpolar covalent bond is where the electrons are shared equally between the atoms. Ex: Cl-Cl

Polar covalent bond is where the electrons are not shared equally between the atoms. Ex: H-Cl

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12. Can a molecule have polar covalent bonds and be nonpolar? Explain your answer.

Yes, they can.

BUT it does have polar bonds

Overall– Nonpolar molecule

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13. Match the following- answers can be used more than once or have multiple answers.1. Induced dispersion 2. Dipole-dipole 3. Hydrogen bonding a. H-H _____ e. nonpolar covalent____b. H-F _____ f. polar covalent____ c. C-Cl____ g. attraction to nucleus & electrons ___d. O-O ____ h. attraction to adjacent atoms___

1321

12 or 3

11, 2, 3

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Name or FormulaIonic or

Covalent ANSWER

Li2O

Nitrogen dibromide

SBr6

Aluminum phosphide

Boron sulfide

SO2

CN2

Potassium nitride

Chlorine trifluoride

Nitrogen disulfide

Magnesium phosphide

Ionic Lithium oxide

Covalent NBr2

Covalent Sulfur hexabromide

Ionic AlPIonic B2S3

Covalent Sulfur dioxideCovalent Carbon dinitride

Ionic K3NCovalent ClF3

Covalent NS2Ionic Mg3P2

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I Can

• Describe covalent bonding. • Provide the names or formulas for molecules. • Draw Lewis dot structures of molecules. • Use Lewis dot structures and VSPER theory to

determine the shape of a molecule. • Predict the intermolecular forces between

molecules by using molecular shapes.

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To Know List- Ch. 3-9

• Look at your reading notes from Ch. 9– 9.1- Covalent bonds

• Why bonds form?• Diatomic Molecules- Name them.• Lewis structures- bonding verse lone pairs• Double/Triple bonds• Bond length verse bond strength

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To Know List- Ch. 3-9

• Look at your reading notes from Ch. 9 (75%)– 9.2 and 9.5 – Naming and Molecular structure

• Binary molecules- what are they?• Naming molecules- Prefixes and rules for mono• 3 Exceptions to the octet rule• Know the 8 basic shapes of Molecules• Electronegativity and polarity relationship• Non polar molecules vs Polar molecules

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To Know List- Ch. 3-9 Test• Concentration of MOSTLY Ch. 9 (75%)

– Ionic Bonding- Ch. 8• Ionic Bonding• Naming/Formula of ionic substances• Properties of Ionic bonds

– Periodic trends- Ch. 6– Energy levels-light, E-dot/valence-Ch. 5– Particles- Protons, Electrons Neutrons-Ch. 4– Physical chemical properties/changes-Ch. 3

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