Chemistry Final Exam Review and Practice Chapters Covered ESSENTIALLY CUMMULATIVE List of Chapters: Ch: 6, 7, 8, 9, 10, 13, 14, 15, 16, 19, 20
Topics to Expect: Periodic Table: s, p, d, f blocks Metal, Metalloid, Non metal, etc. Periodic Trends, Family names Electron Configuration: Orbitals and SubLevels Bonding: covalent, ionic, Lewis dot diagrams Electron Configuration: Atomic #, mass, core notation Bonding: nonpolar covalent, polar covalent, Bonding : molecular shapes, intermolecular forces Solutions: solubility curves Acid and Bases and ph
Atomic Sturcture 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 versuscovalent 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
What is the maximum number of electrons that can by held in an s sublevel? B. 2
What is the maximum # of e - that can by held in a p sublevel? A. 1 B. 2 C. 6 D. 8
What is the maximum # of e - that can by held in a p sublevel? C. 6
What is the total number of sublevel for n=2? A. 1 B. 2 C. 6 D. 8
What is the total number of sublevel for n=2? B. 2
For an element whose electron configuration is [Ne]3s 2 3p 3, how many dots would the Lewis dot diagram have? A. 3 B. 5 C. 8 D. 13
For an element whose electron configuration is [Ne]3s 2 3p 3, how many dots would the Lewis dot diagram have? B. 5
How many dots does the Lewis dot diagram for chlorine have? A. 3 B. 5 C. 7 D. 8
How many dots does the Lewis dot diagram for chlorine have? C. 7
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
A positive lithium ion is formed when a neutral lithium atom: D. loses one electron
When a potassium atom becomes an ion, it: A. gains one proton B. gains one electron C. loses one proton D. loses one electron
When a potassium atom becomes an ion, it: D. loses one electron
When a calcium atom becomes an ion, it: A. gains two protons B. gains two electrons C. loses two protons D. loses two electrons
When a calcium atom becomes an ion, it: D. loses two electrons
Use the periodic table to locate K; what block is it in? a. s-block b. p-block c. d-block d. f-block
Use the periodic table to locate K; what block is it in? a. s-block
What does [Ar]4s 1 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
What does [Ar]4s 1 represent? b. the abbreviated electron configuration for K
What does Ar represent in [Ar]4s 1? 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
What does Ar represent in [Ar]4s 1? c. the chemical symbol of the preceding noble gas
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
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
A bond is nonpolar covalent if the difference in electronegativities between A. 2.1 or more the two atoms is: B. between 0.5 and 2.1 C. less than 0.4 D. less than zero
A bond is nonpolar covalent if the difference in electronegativities between the two atoms is: C. less than 0.4
Which of the following bonds would be considered completely nonpolar? A. H-N B. O-O C. O-C D. F-Cl
Which of the following bonds would be considered completely nonpolar? B. O-O
For the diatomic molecule Cl 2, how many electron(s) does each chlorine share with the other A. 1 B. 2 C. 7 D. 8 chlorine?
For the diatomic molecule Cl 2, how many electron(s) does each chlorine share with the other A. 1 chlorine?
How many pairs of shared and unshared electrons does the Lewis dot structure for water A. 4, 0 B. 3, 1 C. 2, 2 D. 4, 4 have?
How many pairs of shared and unshared electrons does the Lewis dot structure for water have? C. 2, 2
In a double bond between two atoms, the number of shared electrons is: A. 2 B. 4 C. 6 D. 8
In a double bond between two atoms, the number of shared electrons is: B. 4
In the compound ammonia, NH 3 : 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
In the compound ammonia, NH 3 : D. The Lewis structure will have one unshared pair of electrons
What kind of compound would form between nonmetallic atoms and non metallic atoms? A. Nonpolar covalent B. Polar covalent C. Ionic D. Covalent
What kind of compound would form between nonmetallic atoms and non metallic atoms? D. Covalent
What kind of compound would form between polyatomic ions and metallic ions? A. Nonpolar covalent B. Polar covalent C. Ionic D. Covalent
What kind of compound would form between polyatomic ions and metallic ions? C. Ionic
What kind of compound would form between metallic ions and nonmetallic ions? A. Nonpolar covalent B. Polar covalent C. Ionic D. Covalent
What kind of compound would form between metallic ions and nonmetallic ions? C. Ionic
What kind of compound would form between potassium and bromine?: A. Nonpolar covalent B. Polar covalent C. Ionic D. Macromolecular covalent
What kind of compound would form between potassium and bromine?: C. Ionic
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
Predict the physical state of the compound formed between magnesium and oxygen: C. Probably a solid
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
The physical state of nearly all ionic compounds at the temperature of boiling water is: A. Solid
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
Ionic Compounds are generally: C. Formed when a metal transfers its valence electron to a nonmetal
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
How does a covalent bond differ from an ionic bond? A. Ionic: transfer of e - ; covalent: sharing of e -
Which theory is used to account for the shape of molecules? A. theory of relativity B. thermodynamic theory C. kinetic theory D. VSEPR theory
Which theory is used to account for the shape of molecules? D. VSEPR theory
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
Which of the following does a ball and stick model reveal about chemical bonds? C. both A and B
What shape does an ammonia, NH 3, molecule have? A. pyramidal B. trigonal planar C. tetrahedral D. bent
What shape does an ammonia, NH 3, molecule have? A. pyramidal
What shape does a water molecule have? A. pyramidal B. trigonal planar C. tetrahedral D. bent
What shape does a water molecule have? D. bent
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
In a molecule of carbon dioxide, what kind of bonds connect the carbon atom to the 2 oxygen atoms? D. two double bonds
What shape is a carbon dioxide molecule? A. linear B. bent C. trigonal planar D. pyramidal
What shape is a carbon dioxide molecule? A. linear
What shape is a methane molecule? A. tetrahedral B. bent C. trigonal planar D. pyramidal
What shape is a methane molecule? A. tetrahedral
What is the bond angle of a molecule of ammonia, NH 3? A. 107 o B. 109.5 o C. 120 o D. 180 o
What is the bond angle of a molecule of ammonia, NH 3? A. 107 o (<109.5 o )
What is the bond angle of a molecule of carbon dioxide? A. 107 o B. 109.5 o C. 120 o D. 180 o
What is the bond angle of a molecule of carbon dioxide? D. 180 o
What is the bond angle of a molecule of methane? A. 107 o B. 109.5 o C. 120 o D. 180 o
What is the bond angle of a molecule of methane? B. 109.5 o
What is the bond angle of a molecule of water? A. 90 o B. 105 o C. 107 o D 109.5 o
What is the bond angle of a molecule of water? B. 105 o
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
Which of the following properties would you expect to find in a small nonpolar molecule? A. Gas at room temperature
In a pyramidal molecule, how many unshared pairs of valence electrons does the central atom have? A. None B. One C. Two D. Three
In a pyramidal molecule, how many unshared pairs of valence electrons does the central atom have? B. One
In a tetrahedral molecule, how many unshared pairs of valence electrons does the central atom have? A. None B. One C. Two D. Three
In a tetrahedral molecule, how many unshared pairs of valence electrons does the central atom have? A. None
In polar bonds electrons are: A. Shared unequally B. Shared equally C. Completely transfered D. Not shared at all
In polar bonds electrons are: A. Shared unequally
Dipoles are: A. Nonpolar bonds B. Polar bonds C. Nonpolar molecules D. Polar molecules
B. Polar bonds Dipoles are:
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
What determines the polarity of a bond? A. Electronegativity difference only
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
What determines the polarity of a molecule? C. Both A and B
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
How are the electrons shared in a bond between carbon & oxygen? C. Oxygen attracts them more
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
All solutions have the following properties except that the: D. Final physical state of a solution is a liquid
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
Which of the following statements applies to the dissolved solute particles in a solution? B. They will be in the same phase as the solvent
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
Which two substances are miscible in all proportions? D. Water and ethanol
An alloy is an example of a: A. Gaseous mixture B. Liquid solution C. Solid solution D. Solid mixture
An alloy is an example of a: C. Solid solution
All of the following are solutions except: A. Ocean water B. 14K gold bracelet C. antifreeze D. A concrete building block
All of the following are solutions except: D. A concrete building block
Solutions with water as the solvent are called: A. Liquids B. Miscible solutions C. Aqueous solutions D. Electrolytes
Solutions with water as the solvent are called: C. Aqueous solutions
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
Molarity is expressed as: C. Moles of solute / Liters of solution
A solution that contains as much solute as can possibly be dissolved under existing A. saturated conditions is said to be: B. supersaturated C. soluble D. concentrated
A solution that contains as much solute as can possibly be dissolved under existing A. saturated conditions is said to be:
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
Which of the following is NOT an important factor influencing solubility? D. Volume of solution
Common nonpolar solvents include all of the following except: A. Salt water B. Carbon tetrachloride C. Hexane D. Vegetable oil
Common nonpolar solvents include all of the following except: A. Salt water
Ionic solids best dissolve in liquid solvents that are: A. polar B. nonpolar C. viscous D. transparent
Ionic solids best dissolve in liquid solvents that are: A. polar
Which of the following s solubility is most affected by pressure? A. Ionic solids B. Supersaturated solutions C. Gases D. Alloys
Which of the following s solubility is most affected by pressure? C. Gases
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
Why can water dissolve NaCl, whereas hexane cannot? B. As a polar solvent, water is attracted to both anions and cations
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
The rate at which a solid can be dissolved in a liquid solvent can be increased by: B. Grinding the solute into smaller pieces
To identify the strongest acid, compare the K a and: A. The highest K a value is the strongest acid B. The lowest K a value is the strongest acid C. The K a closest to ph 7 is the strongest acid D. The K a closest to ph 0 is the strongest acid
To identify the strongest acid, compare the K a and: A. The highest K a value is the strongest acid
Substances that change color when added to acids or bases are called: A. indicators B. electrolytes C. insulaotrs D. capacitators
Substances that change color when added to acids or bases are called: A. indicators
The ionic compound formed in acid-base neutralization reactions is: A. water B. a salt C. hydride D. hydroxide
The ionic compound formed in acid-base neutralization reactions is: B. a salt
A substance that can act as either an acid or a base is described as: A. neutral B. ambidextrous C. conjugate D. amphoteric
A substance that can act as either an acid or a base is described as: D. amphoteric
Which of the following is least able to donate a proton? A. HF B. H 2 O C. HCO - 3 D. F -
Which of the following is least able to donate a proton? D. F -
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
Which of the following could be a conjugate acid-base pair? C. strong acid weak base
The K a for HCN is 6.2x 10-2. What is the conjugate base for HCN in the following equation? HCN + H 2 O H 3 O + + CN - A. H 2 O, weak B. H 2 O, strong C. CN -, weak D. CN -, strong
The K a for HCN is 6.2x 10-2. What is the conjugate base for HCN in the following equation? HCN + H 2 O H 3 O + + CN - D. CN -, strong
The acid dissociation constant measures an acid s: A. concentration B. strength C. number of protons D. degree of sourness
The acid dissociation constant measures an acid s: B. strength
Which 1M solution, hydrofluoric acid or formic acid, would have the greater H 3 O + concentration? A. the acid with more hydrogen atoms B. the acid with the higher K a C. the acid with the higher molar mass D. neither
Which 1M solution, hydrofluoric acid or formic acid, would have the greater H 3 O + concentration? B. the acid with the higher K a
HNO 3 reacts with magnesium metal to give off the gas: A. oxygen B. nitrogen C. hydrogen D. no gas is given off
HNO 3 reacts with magnesium metal to give off the gas: C. hydrogen
HNO 3 turns litmus paper: A. blue B. red C. no color change D. green
B. red HNO 3 turns litmus paper:
What is the ph of 0.00100M HCl? A. 3 B. 2 C. 1.3 D. 4
What is the ph of 0.00100M HCl? A. 3
What affect does increasing the ph have on the hydronium ion concentration? A. Doubles it B. Halves it C. Increases by power of 2 (10 times more) D. Decreases by power of 2 (10 times less)
What affect does increasing the ph have on the hydronium ion concentration? D. Decreases by power of 2 (10 times less)
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
What is the ph of an acid if the hydronium ion concentration is 2 x 10-4 M? B. 3.7
Determine the ph of a 0.00100M NaOH solution. A. 3 B. 4 C. 11 D. 14
Determine the ph of a 0.00100M NaOH solution. C. 11
Pure water contains which of the following species? A. H 2 O molecules B. H 3 O + ions C. OH - ions D. all of these
Pure water contains which of the following species? D. all of these
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
Determine the hydroxide ion concentration of a solution with a ph of 13. D. 1.0 x 10-1
The definition of ph is: A. log[h 3 O + ] B. the percent of hydronium ions C. the parts per million of hydronium ions D. log[oh - ]
The definition of ph is: A. log[h 3 O + ]
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
Two common ways to measure ph are: B. with indicators and a ph meter
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
The equivalence point of a strong acid-strong base titration curve is: D. all of the above
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
If phenolphtalein is used as an indicator in a titration of an acid with a base, at what point will the solution turn pink? C. after the equivalence point
Chemistry Final Exam Good Luck! ESSENTIALLY CUMMULATIVE List of Chapters: Ch: 6, 7, 8, 9, 10, 11, 13, 14, 15, 16, 19, 20 Read CHAPTER SUMMARIES Complete the review package.