Which of the following elements requires the least amount ...s3.amazonaws.com/prealliance_oneclass_sample/kKr72yrwKa.pdf · he particle that has the smallest mass is? Select one:

he particle that has the smallest mass is?

Select one: a. Atom b. Neutron c. Electron d. Proton

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Which particle always has a negative charge?

Select one: a. Neutron b. Atom c. Proton d. Electron

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Which of the following elements requires the least amount of

energy to remove an electron to form an ion?

Select one: a. Ca b. K c. Na d. Mg e. Fr

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According to the Lewis model of the atom, the number of bonding electrons in a nitrogen atom is?

Select one: a. 1 b. 2

c. 5 d. 3 e. 7

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The mass number refers to

Select one: a. The number of protons in the nucleus of an atom b. The total number of protons and electrons in the nucleus of an atom c. The number of neutrons in atom d. The number of electrons in an atom e. The total number of protons and neutrons of an atom

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Atoms of the same element which have the same number of protons but a different number of neutrons are known as

Select one: a. Neutral atoms b. Molecule c. A chemical family d. Ions e. Isotopes

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2412Mg2+ contains (note, 24 should be directly over top of the 12)

Select one: a. 12 protons, 12 neutrons and 14 electrons b. 12 protons, 12 neutrons and 10 electrons c. 12 protons, 12 neutrons and 12 electrons d. 12 protons, 10 neutrons and 10 electrons e. 24 protons, 12 neutrons and 2 electrons

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In which pair of elements is the element with the smaller electron affinity listed first? Select one: a. Helium, neon b. Sodium, magnesium c. Fluorine, oxygen d. Beryllium, lithium

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Which of the following statements about atomic structure is TRUE?

Select one: a. The number of protons, neutrons and electrons are always equal in a neutral atom. b. The number of neutrons and electrons are always equal in a neutral atom. c. The number of protons and neutrons are always equal in a neutral atom. d. The number of protons and electrons are always equal in a neutral atom.

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Which of the following is the most important factor in determining the chemical properties of an element?

Select one: a. The number of valence electrons b. The total number of neutrons c. The total number of electrons in its atoms d. The total number of protons in the nucleus

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How many molecules are in 1 mole of Na2O?

Select one: a. 1 b. 2

c. 3 d. 1.8x10^24 e. 6.02x10^23

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1mL is equal to how many grams?

Select one: a. 2 b. 5 c. 1 d. 3 e. 4

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3mg is equivalent to how many micrograms (µg)?

Select one: a. 0.000003 b. 0.0003 c. 3000 d. 0.003 e. 300

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What is the difference between an ionic and covalent bond in terms of electrons.

Select one: a. Ionic electrons are only lost, covalent electrons are only gained b. Ionic electrons are shared, covalent electrons are transferred c. Ionic electrons are transferred, covalent electrons are shared d. Ionic electrons are only gained, covalent electrons are only lost

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Determine the following for COCl2

·The type of bond(s) (ionic, polar covalent, non-polar covalent) present.

·If polar covalent indicate the ∆EN associated with each bond.

· If polar covalent indicate the correct partial charge associated with each element of each bond.Use Lewis structure to demonstrate the electron configuration and partial charge distribution.

·Determine the potential molecular geometry. (remember VSEPR).

Select one: a. Non-Polar covalent. Carbon central with single covalent bond to each of the two chlorides (∆EN = 0) and double covalent to the oxygen (∆EN = 0). Molecular geometry linear. b. Polar covalent. Carbon central with double covalent bond to each of the two chlorides (∆EN = 0.61) and double covalent to the oxygen (∆EN = 0.89). Carbon partial negative charge, both chloride and oxygen a negative partial charge. Molecular geometry bent. c. Polar covalent. Carbon central with single covalent bond to each of the two chlorides (∆EN = 0.61) and double covalent to the oxygen (∆EN = 0.89). Carbon partial positive charge, both chloride and oxygen a negative partial charge. Molecular geometry trigonal planar. d. Ionic bond. Carbon central with single covalent bond to each of the two chlorides (∆EN = 0.61) and double covalent to the oxygen (∆EN = 0.89). Carbon partial positive charge, both chloride and oxygen a negative partial charge. Molecular geometry tetrahedral. e. Non -Polar covalent. Carbon central with single covalent bond to each of the two chlorides (∆EN = 0.89) and double covalent to the oxygen (∆EN = 0.61). Carbon partial negative charge, both chloride and oxygen a positive partial charge. Molecular geometry trigonal bipyramidal.

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Write the equation and predict the products of the following

combination.Remember to balance if necessary.

Potassium iodide plus bromine gas

Select one: a. KI + Br -> KBr + I b. 2KI2 + 2B3 -> K2I + 3B2 c. 2KI + Br2 -> 2KBr + I2 d. K2I3 + 4Br -> 2KBr2 + 3I

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Balance the following chemical equations and identity the type of reaction demonstrated.

Mg(NO3)2 + K3PO4-> Mg3(PO4)2 + KNO3

Select one: a. Mg(NO3)2 + 3K3PO4 -> Mg3(PO4)2 + 9KNO3; combustion b. 6Mg(NO3)2 + 4K3PO4 -> 2Mg3(PO4)2 + 4KNO3; synthesis c. 3Mg(NO3)2 + 2K3PO4 -> Mg3(PO4)2 + 6KNO3; double displacement d. 12Mg(NO3)2 + K3PO4 -> 4Mg3(PO4)2 + 3KNO3; single displacement e. 2Mg(NO3)2 + K3PO4 -> Mg3(PO4)2 + 3KNO3; decomposition

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If situated close enough together a hydrogen bond may form between which of the following. A hydrogen bond is an example of what type of attraction?

Select one: a. Nδ- and Hδ-, dipole-dipole b. Oδ+ and Hδ+, ion-dipole c. Oδ- and Hδ+, ion-dipole d. Nδ- and Hδ+, dipole-dipole

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Electrons found in which of the following orbitals have the highest energy?

Select one: a. 2p b. 4p c. 3d d. 1s e. 3s

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What volume of 0.27mol/L solution can be made using 15.2g of sodium hydroxide?

Select one: a. 4.5L b. 0.27L c. 1.4L d. 15.2L e. 2.3L

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400mL of 3M NaOH needs to be diluted to 2M. What volume of diluting solution should be added to the initial volume?

Select one: a. 400mL b. 800mL c. 600mL d. 200mL e. 100mL

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Maganese(III) fluoride can be formed by the reaction of manganese(II) iodide with fluorine gas. If 1.23g of manganese(II) iodide reacts with 25g of fluorine gas what mass of manganese(III)fluoride is expected? Which reactant is in excess and how much of it remains at the end of the reaction?

Select one: a. 0.38g, fluoride gas, 25g b. 1.23g, manganese(III) fluoride, 1g c. 0.5g, manganese(III) fluoride, 0.5g d. 0.45g, fluoride gas, 24g

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37.82mL of sodium hydroxide solution is needed to neutralize 15mL of 0.250mol/L of hydrofluoric acid. What is the concentration of sodium hydroxide?

Select one: a. 0.0992mol/L b. 9.92mol/L c. 2.3mol/L d. 0.045mol/L e. 0.0333mol/L

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An unknown gas is composed of 80% carbon and 20% hydrogen. A 4.60g sample occupies a volume of 2.50L at 1.50atm and 25.0οC. What is the molecular formula of the gas?

Select one: a. C4H10 b. CH2 c. C2H6 d. C3H8 e. CH

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The name 3-ethyl-2,2-dimethyl-3-heptene tells you what about its structure. (Draw)

Select one: a. 6 carbon root with a double bond at the 3rd carbon, three ethyl side chains and 2 methyl side chains. b. 6 carbon root with 3 double bonds, three ethyl side chains and four methyl side chains c. 7 carbon root with a triple bond at the 2nd carbon, one ethyl side chain at carbon 3 and one methyl side chain at carbon 2 d. 7 carbon root with a double bond at the third carbon, one ethyl side chain at carbon 3, and two methy side chains off of carbon 2 e. 2 carbon root with two methyl side chains and three heptene side chains.

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Name the following functional groups. NH2, COOH, COO-, OH

Select one: a. Amine, carboxyl, ester, alcohol b. Ammonia, carboxyl, carboxyl negative, hydroxyl c. Nitrogen, carbonoester, carbon, alcohol d. Nitrogen, carbon, carbon, oxygen e. Amine, carbonoester, ester, hydroxyl

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A reaction combining a carboxylic acid and an alcohol results in a compound containing a or an______________? What type of reaction is this?

Select one: a. Ketone, condensation b. Amide, combustion c. Carboxyl-alcohol, hydrolysis

d. Aldehyde, hydrolysis e. Ester, condensation

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Propanol contains which functional group? (determine based on the name, you do not need to know the structure)

Select one: a. Alcohol b. Aldehyde c. Carboxyl d. Ketone e. Ether

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Name the reaction: Disaccharide + H2O -> Monosaccharide + Monosaccharide.

Select one: a. Condensation b. Combustion c. Oxidation d. Reduction e. Hydrolysis

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Lipids are soluble in.

Select one: a. Lipids are not soluble b. Aqueous solutions c. Water d. Polar solutions e. Non-polar solutions

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Monosaccharide, disaccharide, and polysaccharide are respectively composed of.

Select one: a. One sodium, two sodium, many sodium b. One sugar, two sugar, many sugars c. One ether, two ether, many ether d. One alcohol, two alcohol, many alcohols e. One aldehyde, two aldehyde, many aldehydes

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Aluminum readily reacts with chlorine gas to produce aluminum chloride. This is an exothermic reaction.

2Al(s) + 3Cl(g)-> 2AlCl3(s) ∆Hrxn = -1408KJ

What is the enthalpy change when 1.0kg of Al reacts completely with excess Cl2?

Select one: a. -26093KJ b. +3001KJ c. +32KJ d. +400KJ e. -1278KJ

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Over an interval of 1second (s) the mass of Mg(s), in the reaction below, changes by -0.011g. What is the corresponding rate of consumption of HCl(aq) in mol/second (mol/s).

Mg(s) + 2HCl -> MgCl2(aq) +H2(g)

Select one: a. +9 x 10^-4mol/s b. +4.5 x 10^-4mol/s c. -4.5 x 10^-4 mol/s d. -9 x 10^-4mol/s

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Which of the following affect the rate of reaction?

Select one: a. Surface area b. Reactant concentration c. Temperature d. All options e. A catalyst

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Carbon monoxide reacts with nitrogen dioxide to form carbon dioxide and nitric oxide. The activation energy of the forward reaction (Ea(fwd)) is 134KJ and the ∆Hrxn is -226KJ. What is the activation energy of the reverse reaction (Ea(rev))? (It may be helpful to draw a potential energy diagram).

Select one: a. 92KJ b. 226KJ c. 360KJ d. -134KJ e. -92KJ

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A 500mL beaker is equally divided by a membrane

permeable only to NaCl. Side A contains 250mL of 1x10-6M

of NaCl. Side B contains 250mL 1x10-12M of NaCl. In which

direction will the NaCl diffuse?

Select one: a. No diffusion will occur it is already at equilibrium b. Diffuse side A to side B c. Diffuse side B to side A

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The following reaction increases the proportion of hydrogen gas.

CO(g) + H2O(g) ↔ H2(g) + CO2(g) At 700K the equilibrium constant is 8.3. You start with 1.0mol of CO(g) and 1.0mol of H2O(g) in a 5.0L container. What amount of H2(g) and CO(g) will be present in the container when the gases are at equilibrium, at 700K?

Select one: a. H2(g) 0.04mol, CO(g) 0.96mol b. H2(g) 0.25mol, CO(g) 0.75mol c. H2(g) 1mol, CO(g) 1mol d. H2(g) 0.75mol, CO(g) 0.25mol e. H2(g) 0.96mol, CO(g) 0.04mol

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At 500οC the value of Kc (equilibrium constant) is 0.40. The concentration of gases present at this temperature are as follows: N2(g) 0.10mol/L, H2(g) 0.30mol/L, and NH3(g)

0.20mol/L. Is this mixture at equilibrium? If not, what is Qc and in which direction will the reaction go to reach equilibrium?

N2(g) + 3H2(g) ↔ 2NH3(g)

Select one: a. Reaction at equilibrium b. Reaction not at equilibrium, Qc 5, reaction proceeds to the left c. Reaction not at equilibrium, Qc 0.35, reaction proceeds to the right d. Reaction not at equilibrium, Qc 0.2, reaction proceeds to the right e. Reaction not at equilibrium, Qc 14.8, reaction proceeds to the left

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Lemon juice is pH2 and blood pH8. Which is more acidic and how many times greater is the [H+]?

Select one: a. Lemon juice acidic, blood basic, 1 000 000 times greater b. Lemon juice basic, blood acidic, 60 times greater c. Lemon juice acidic, blood basic, 6 times greater d. Lemon juice basic, blood acidic, 1000 times greater e. Lemon juice acidic, blood basic, 600 times greater

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A 0.10mol/L solution of propanoic acid (CH3CH2COOH) is pH 2.96. Calculate the Ka(acid dissociation constant) and the percent dissociation for this acid.

CH3CH2COOH(aq) + H2O(l) ↔ CH3CH2COO- + H3O+(aq)

Select one: a. Ka 6.3 x10^-8, percent dissociation 10% b. Ka 1.3 x10^5, percent dissociation 3.4% c. Ka 5.2 x10^-4, percent dissociation 25% d. Ka 1.2 x10^-5, percent dissociation 1.1% e. Ka 1.7 x10^-9, percent dissociation 0.5%

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REDOX reaction refers to an oxidation-reduction reaction. During the reduction component electrons are

______________. During the oxidation component electrons are _______________.

Select one: a. Gained (reduction) and Lost (oxidation) b. Moved to a lower energy level (reduction), moved to a higher energy level (oxidation) c. Moved to a higher energy level (reduction), moved to a lower energy level (oxidation) d. Lost (reduction) and gained (oxidation)

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Comments regarding the chemistry self-assessment test. ◦ Did you find this test to be useful? ◦ Did you discover areas of strength or weakness? ◦ Do you have plans to review chemistry material based on what you discovered

through completing the self assessment? ◦ Any other comments

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Yes, it refreshed my memory about chemistry and I remembered alot. I discovered that I have to re-learn alot of the basic

chemistry skills that were taught to me in grade 12.

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How long ago did you complete grade 12 chemistry or an equivalent course (e.g. Chem 1500)?

(This question provides us will valuable information regarding the students composing our class and will aid with future lecture and course development. All information is confidential, but you do not need to answer if you do not feel comfortable doing so. Thank you) Select one: a. Less than 6 months ago. b. 6months to 1 year ago c. 2 years ago d. 3-4 years ago e. 5 or more years ago.

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Where did you complete Grade 12 chemistry or an equivalent course? (This question provides us will valuable information regarding the students composing our class and will aid with future lecture and course development. All information is confidential, but you do not need to answer if you do not feel comfortable doing so. Thank you) Select one: a. Greater Toronto Region (GTA) b. Southern Ontario (not including the GTA) c. Central or Northern Ontario d. Quebec or Eastern Canada e. Prairie or Western Provinces f. United States of America (USA) g. International (not including the USA)

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Which of the following elements requires the least amount ...s3.amazonaws.com/prealliance_oneclass_sample/kKr72yrwKa.pdf · he particle that has the smallest mass is? Select one: