Topics to Expect:

Periodic Table:

s, p, d, f blocks

Metal, Metalloid, Non –metal, etc.

Electron Configuration: Orbitals and SubLevels

Electron Configuration: Atomic #, mass, core notation

Periodic Trends, Family names

Bonding: covalent, ionic, Lewis dot diagrams

Bonding: nonpolar covalent, polar covalent,

Bonding : molecular shapes, intermolecular forces

Solutions: solubility curves

Acid and Bases and pH

Atomic Structure and Electron Configuration

• Location of electrons in s, p, d, f orbitals.• Shape and number of s and p orbitals.• Number of electrons each orbital each sublevel and

each level can hold.• Location of s, p, d, f blocks on periodic table.• Lewis dot diagrams.• Formation of complete octets by transfer of / sharing

of electrons.

Electron Configuration & Periodic Table

• Atomic Number• Electrons, Protons and Neutrons• Core notation using chemical symbol of preceding

noble gas• Trends for physical and chemical properties• Atomic radii, ionization energy, electronegativity

Bonding

• Ionic versus covalent• Valence electrons and dot diagrams• Lewis structures: shared pairs and lone pairs

Molecular Shapes and Polarity

• Recognize drawings of ball and stick models• Use VSEPR• Recognize dipole as electrons being pulled towards the

higher electronegative element, causing a partial negative charge on that atom and a partial positive charge on the lower electronegative atom

• Dispersion, dipole-dipole, hydrogen bonding: types of intermolecular forces in covalent compounds

Solutions

• Solubility Curves and Vocabulary

Acids, Bases and pH•Self Ionization of Water and pH

What is the maximum number of electrons that can by held in an “s”

sublevel?

• A. 1• B. 2• C. 6• D. 8

B

What is the maximum # of e- that can by held in a “p” sublevel?

• A. 1• B. 2• C. 6• D. 8

C

What is the total number of sublevel for n=2?

• A. 1• B. 2• C. 6• D. 8

B

For an element whose electron configuration is [Ne]3s23p3, how many dots would the Lewis dot

diagram have?

• A. 3• B. 5• C. 8• D. 13

B

How many dots does the Lewis dot diagram for chlorine have?

• A. 3• B. 5• C. 7• D. 8

C

A positive lithium ion is formed when a neutral lithium atom:

• A. gains one proton• B. gains one electron• C. loses one proton• D. loses one electron

D

When a potassium atom becomes an ion, it:

• A. gains one proton• B. gains one electron• C. loses one proton• D. loses one electron

D

When a calcium atom becomes an ion, it:

• A. gains two protons• B. gains two electrons• C. loses two protons• D. loses two electrons

D

Use the periodic table to locate K; what block is it in?

• a. s-block• b. p-block• c. d-block• d. f-block

A

What does [Ar]4s1 represent?

• a. the full electron configuration of K• b. the abbreviated electron configuration for K• c. the full mass designation for K• d. the block designation for K

B

What does Ar represent in [Ar]4s1?

• a. the block of the periodic table• b. the highest orbital filled• c. the chemical symbol of the preceding noble

gas• d. the chemical symbol of the element

C

What kind of bond is predicted to form between B and H if their

electronegativities are 2.0 and 2.2 respectively?

• a. nonpolar covalent • b. polar covalent• c. ionic• d. intermolecular

A

A bond is nonpolar covalent if the difference in electronegativities between the two atoms is:

• A. 2.1 or more• B. between 0.5 and 2.1• C. less than 0.4• D. less than zero

C

Which of the following bonds would be considered completely nonpolar?

• A. H-N• B. O-O• C. O-C• D. F-Cl

B

For the diatomic molecule Cl2, how many electron(s) do the

chlorines share ?

• A. 1• B. 2• C. 7• D. 8

B

How many pairs of shared and unshared electrons does the Lewis

dot structure for water have?

• A. 4, 0• B. 3, 1• C. 2, 2• D. 4, 4

C

In a double bond between two atoms, the number of shared

electrons is:

• A. 2• B. 4• C. 6• D. 8

B

In the compound ammonia, NH3:

• A. Each hydrogen has a partial negative charge• B. The nitrogen has a full positive charge• C. The N-H bond is ionic• D. The Lewis structure will have one unshared

pair of electrons D

What kind of compound would form between nonmetallic atoms and non

metallic atoms?

• A. Nonpolar covalent• B. Polar covalent• C. Ionic• D. Covalent

D

What kind of compound would form between polyatomic ions and

metallic ions?

• A. Nonpolar covalent• B. Polar covalent• C. Ionic• D. Covalent

C

What kind of compound would form between metallic ions and

nonmetallic ions?

• A. Nonpolar covalent• B. Polar covalent• C. Ionic• D. Covalent

C

What kind of compound would form between potassium and bromine?:

• A. Nonpolar covalent• B. Polar covalent• C. Ionic• D. Macromolecular covalent

C

Predict the physical state of the compound formed between

magnesium and oxygen:

• A. Probably a gas• B. Probably a liquid• C. Probably a solid• D. Impossible to determine from the given data

C

The physical state of nearly all ionic compounds at the temperature of

boiling water is:

• A. Solid• B. liquid• C. Gas• D. Different for each ionic compound

A

Ionic Compounds are generally:

• A. Conductors of electricity in the solid state• B. Gases at room temperature• C. Formed when a metal transfers its valence

electron to a nonmetal• D. Electrically charged

C

How does a covalent bond differ from an ionic bond?

• A. Ionic: transfer of e-; covalent: sharing of e-

• B. Ionic: involves 2 e-; covalent: involves 4 e-

• C. Ionic: btw metals; covalent btw nonmetals• D: Ionic: usually acids; covalent: usually bases

A

Which theory is used to account for the shape of molecules?

• A. theory of relativity• B. thermodynamic theory• C. kinetic theory• D. VSEPR theory

D

Which of the following does a ball and stick model reveal about

chemical bonds?

• A. their arrangement in space• B. their presence and type• C. both A and B• D. neither A or B

C

What shape does an ammonia , NH3, molecule have?

• A. pyramidal• B. trigonal planar• C. tetrahedral• D. bent

A

What shape does a water molecule have?

• A. pyramidal• B. trigonal planar• C. tetrahedral• D. bent

A

In a molecule of carbon dioxide, what kind of bonds connect the

carbon atom to the 2 oxygen atoms?

• A. two single bonds• B. one single and one double bond• C. one double and one triple bond• D. two double bonds

D

What shape is a carbon dioxide molecule?

• A. linear• B. bent• C. trigonal planar• D. pyramidal

A

What shape is a methane molecule?

• A. tetrahedral• B. bent• C. trigonal planar• D. pyramidal

A

What is the bond angle of a molecule of ammonia , NH3?

• A. 107o

• B. 109.5o

• C. 120o

• D. 180o

A

What is the bond angle of a molecule of carbon dioxide?

• A. 107o

• B. 109.5o

• C. 120o

• D. 180o

D

What is the bond angle of a molecule of methane?

• A. 107o

• B. 109.5o

• C. 120o

• D. 180o

B

What is the bond angle of a molecule of water?

• A. 90o

• B. 105o

• C. 107o

• D 109.5o

B

Which of the following properties would you expect to find in a small

nonpolar molecule?

• A. Gas at room temperature• B. Solid at room temperature• C. Very high melting point• D Very high boiling point

A

In a pyramidal molecule, how many unshared pairs of valence electrons

does the central atom have?

• A. None• B. One• C. Two• D. Three

B

In a tetrahedral molecule, how many unshared pairs of valence electrons does the central atom

have?

• A. None• B. One• C. Two• D. Three

A

In polar bonds electrons are:

• A. Shared unequally• B. Shared equally• C. Completely transfered• D. Not shared at all

A

Dipoles are:

• A. Nonpolar bonds• B. Polar bonds• C. Nonpolar molecules• D. Polar molecules

D

What determines the polarity of a bond?

• A. Electronegativity difference only• B. Molecular shape only• C. Both A and B• D. Neither A and B

A

What determines the polarity of a molecule?

• A. Electronegativity difference only• B. Molecular shape only• C. Both A and B• D. Neither A and B

C

How are the electrons shared in a bond between carbon & oxygen?

• A. They are shared equally• B. Carbon attracts them more• C. Oxygen attracts them more• D. Electrons are completely transferred

C

All solutions have the following properties except that the:

• A. Dissolved particles are very small• B. Particles in a solution are evenly distributed• C. Solution particles do not settle out• D. Final physical state of a solution is a liquid

D

Which of the following statements applies to the dissolved solute

particles in a solution?

• A. They can be seen with the unaided eye• B. They will be in the same phase as the

solvent• C. They will settle out when left standing• D. There is always less solute than solvent

D

Which two substances are miscible in all proportions?

• A. Water and sugar• B. Water and mineral oil• C. Water and gasoline• D. Water and ethanol

D

An alloy is an example of a:

• A. Gaseous mixture• B. Liquid solution• C. Solid solution• D. Solid mixture

C

All of the following are solutions except:

• A. Ocean water• B. 14K gold bracelet• C. antifreeze• D. A concrete building block

D

Solutions with water as the solvent are called:

• A. Liquids• B. Miscible solutions• C. Aqueous solutions• D. Electrolytes

C

Molarity is expressed as:

• A. Moles of solvent / Liters of solute• B. Moles of solute / Liters of solvent• C. Moles of solute / Liters of solution• D. Moles of solute / moles of solution

C

A solution that contains as much solute as can possibly be dissolved under existing conditions is said to

be:

• A. saturated• B. supersaturated• C. soluble• D. concentrated

A

Which of the following is NOT an important factor influencing

solubility?

• A. Chemical nature of solute• B. Temperature• C. Chemical nature of solvent• D. Volume of solution

D

Common nonpolar solvents include all of the following except:

• A. Salt water• B. Carbon tetrachloride• C. Hexane• D. Vegetable oil

A

Ionic solids best dissolve in liquid solvents that are:

• A. polar• B. nonpolar• C. viscous• D. transparent

A

Which of the following’s solubility is most affected by pressure?

• A. Ionic solids• B. Supersaturated solutions• C. Gases• D. Alloys

C

Why can water dissolve NaCl, whereas hexane cannot?

• A. Hexane is attracted to the sodium, but not to the chlorine

• B. As a polar solvent, water is attracted to both anions and cations

• C. Both water and salt are inorganic, while hexane is organic

• D. Water can form hydrogen bonds with NaCl

B

The rate at which a solid can be dissolved in a liquid solvent can be

increased by:

• A. Lowering the temperature of the solvent• B. Grinding the solute into smaller pieces• C. Increasing the air pressure on the liquid• D. Lowering the temperature of the solute

B

To identify the strongest acid, compare the Ka and:

• A. The highest Ka value is the strongest acid

• B. The lowest Ka value is the strongest acid

• C. The Ka closest to pH 7 is the strongest acid

• D. The Ka closest to pH 0 is the strongest acid

A

Substances that change color when added to acids or bases are called:

• A. indicators• B. electrolytes• C. insulaotrs• D. capacitators

A

The ionic compound formed in acid-base neutralization reactions is:

• A. water• B. a salt• C. hydride• D. hydroxide

B

A substance that can act as either an acid or a base is described as:

• A. neutral• B. ambidextrous• C. conjugate• D. amphoteric

D

Which of the following is least able to donate a proton?

• A. HF• B. H2O

• C. HCO3-

• D. F-

D

Which of the following could be a conjugate acid-base pair?

• A. strong acid –strong base• B. weak acid - weak base• C. strong acid – weak base• D. need more information

C

The Ka for HCN is 6.2x 10-2. What is the conjugate base for HCN in the following equation? HCN + H2O

H3O+ + CN-

• A. H2O, weak

• B. H2O, strong

• C. CN-, weak• D. CN-, strong

D

The acid dissociation constant measures an acid’s:

• A. concentration• B. strength• C. number of protons• D. degree of sourness

B

Which 1M solution, hydrofluoric acid or formic acid, would have the

greater H3O+ concentration?

• A. the acid with more hydrogen atoms• B. the acid with the higher Ka

• C. the acid with the higher molar mass• D. neither

B

HNO3 reacts with magnesium metal to give off the gas:

• A. oxygen• B. nitrogen• C. hydrogen• D. no gas is given off

C

HNO3 turns litmus paper:

• A. blue• B. red• C. no color change• D. green

B

What is the pH of 0.00100M HCl?

• A. 3• B. 2• C. 1.3• D. 4

A

What affect does increasing the pH have on the hydronium ion

concentration?

• A. Doubles it• B. Halves it• C. Increases by power of 1 (10 times more)• D. Decreases by power of 1 (10 times less)

D

What is the pH of an acid if the hydronium ion concentration is

2 x 10-4 M?

• A. 2• B. 3.7• C. 4.3• D. 4.7

B

Determine the pH of a 0.00100M NaOH solution.

• A. 3• B. 4• C. 11• D. 14

C

Pure water contains which of the following species?

• A. H2O molecules

• B. H3O+ ions

• C. OH- ions• D. all of these

D

Determine the hydroxide ion concentration of a solution with a

pH of 13.

• A. 1.0 x 10-13

• B. 13• C. 1• D. 1.0 x 10-1

D

The definition of pH is:

• A. –log[H3O+]

• B. the percent of hydronium ions• C. the parts per million of hydronium ions• D. log[OH-]

A

Two common ways to measure pH are:

• A. with indicators and thermometers• B. with indicators and a pH meter• C. by taste and color• D. by electric conductivity and by temperature

B

The equivalence point of a strong acid-strong base titration curve is:

• A. at a pH of 7• B. at the steepest part of the curve• C. when the solution is neutral• D. all of the above

B

If phenolphtalein is used as an indicator in a titration of a strong acid with a strong base, at what point will the solution turn pink?

• A. before the equivalent point• B. at the equivalence point• C. after the equivalence point• D. need more information

B

Chemistry Final Exam Good Luck!

– ESSENTIALLY CUMMULATIVE

• Units 4-6• Review past

assessments• Complete the review

package.