Honors Chemistry: Spring Exam Review SheetName:

True or False: Decide whether the following statements are either true or false. If the statement is false, change the underlined word or phrase to make the statement true.

TRUE1) The density of a silver bar stays the sameeven as the mass of the bar increases..

Density is an intensive property. It does not depend on the amount present.

FALSE2) The number 6.023 x 1023 contains 4 significant figures.

When decimal is present, start on left and count all digits starting with first nonzero number.

TRUE3) Mass is an example of an extensive property.

It depends on the amount present.

FALSE4) TheCRITICAL POINTof a substance is the temperature above which the liquid state of a substance can longer be formed.

The triple point is the temperature and pressure where all 3 states of matter are present in an equilibrium.

FALSE5) The decomposition of H2O to form elemental hydrogen and oxygen is an example of a CHEMICAL change.

Two new substances are formed.

TRUE6) A solution is a homogeneous mixture of two or more substances.

FALSE7) The change of CO2 (s) to CO2 (l) is known as MELTING.

Deposition is when a gas turns directly into a solid.

FALSE8) The OIL DROP EXPERIMENTwas used to the discovery of the charge of an electron.

The gold foil experiment led to the discovery of the nucleus.

TRUE9) The addition of an electron to an elementresults in the formation of ananion.

TRUE10) Anelectron was the first subatomic particle to be discovered.

It was discovered by JJ Thomson using a cathode ray tube.

FALSE11) Analpha particle is a high-speed electron.

A beta particle is a high speed electron.

FALSE12) Isotopes of an atom have the same number of protons, but a different number ofNEUTRON.

Ions (cation or anion) have different number of electrons

TRUE13) Oxygen is one of the seven diatomic elements.

FALSE14) Atoms of the same element must have the same ATOMIC number.

The atomic number gives the number of protons in an atom, which defines the identity of an atom.

TRUE15) Sulfur is an atom that has six valence electrons.

TRUE16) Chlorine is classified as ahalogen.

FALSE17) A cathode ray is a beam of ELECTRONS.

The ray bends towards the positive electrode when passed through charged plates.

TRUE18) Elements in the periodic table are sequentially arranged in order of increasing atomic number.

FALSE19) An example of THE LAW OF DEFINITE PROPORTIONS is that water always consists of 89% oxygen and 11% hydrogen by mass.

The law of conservation of mass states that mass is neither created nor destroyed during a process.

FALSE20) TheEXPERIMENTAL yield of a product is the experimental mass obtained from a specified reaction.

The theoretical yield is the maximum amount of product that is possible based on calculations.

FALSE21) Spectator ions DO NOT APPEARin a net-ionic equation.

Only ions involved in the chemical reaction appear in the net ionic equation.

FALSE22) Sucrose (C12H22O11) will dissociate completely when dissolved in water.

Sugar (C12H22O11) is a molecular compound which do not dissociate when dissolved in water.

TRUE23) Nitric acid is a strong acid.

Along with HCl, HBr, HI, HClO4, and H2SO4

FALSE24) The explosion of a hydrogen bomb is accompanied by the release of heat; thus it is an EXOTHERMIC process.

ANY process gives off heat is considered to be exothermic.

FALSE25) Green electromagnetic radiation with a wavelength of 500 nm has an energy that is INVERSELY proportional to its wavelength.

The energy is directly proportional with the frequency ( E = h ).

TRUE26) According to Heisenberg’s uncertainty principle, it is not possible to measure simultaneously and accurately the position and momentum of an electron at the same time.

FALSE27) Theground-state electron configuration for carbon is 1s22s22p2

Carbon has 4 valence electrons on the 2nd energy level.

FALSE28) According to the HUND’S RULE, electrons must enter degenerate orbits successively with the same spin.

Pauli’s states that no two electrons can have the same quantum number.

FALES29) The atomic radius of fluorine is SMALLER than that of nitrogen.

Radius of atoms decrease from left to right across a period

TRUE30) Noble gases tend to be inert because their valence shell of electrons is filled.

They have full s and p sublevels, so they don’t need to gain, lose, or share electrons

FALSE31) The first ionization energy of nitrogen is LARGER than that of carbon.

Ionization energies increase from left to right across a period

FALSE32) The Lewis structure for N2 includes a TRIPLE bond.

Must draw the Lewis structure (10 total electrons to distribute).

FALSE33) The bond that forms between atoms of Ca and O in the compound CaO is IONIC.

Bond between a metal and a nonmetal.

FALSE34) When the activation energy of a reaction is greater than the energy released when the bonds of the products are form, the process is said to be ENDOTHERMIC.

The amount of energy put in is greater than the amount of energy given off.

FALSE35) The compound H2COhas an AX3E2 base structure.

PCl3 has 26 valence electrons to distribute. The 3 peripheral atoms require 24 electrons, so there must be a lone pair.

FALSE36) The molecular geometry of NH3 is tetrahedral.

It has an AX4E base structure.

TRUE37) ICl is a polar molecule where I2 is not.

FALSE38) The formula C2H4O can be considered an empirical formula.

Empirical formulas must be reduced to simplest ratio

FALSE39) To be classified as a combustion reaction, OXYGEN must be one of the reactants.

All combustion reactions have oxygen as a reactant. Common combustion reactions involve hydrocarbons.

TRUE40) A solution is saturated when the maximum amount of solute is dissolved into a given amount of solvent.

FALSE41) Standard temperature and pressure (STP) for a gas is 0˚C AND 1atm.

Standard temperature of a gas is 0C or 273 K.

TRUE42) According to Graham’s law, you should expect NH3 (g) to effuse faster through a tiny hole than CO2 (g) at 25˚C.

Lighter gases will effuse faster than heavier gases at the same temperature.

FALSE43) According to the kinetic theory of gases, gases have THE SAME average kinetic energies at the same temperature.

According to the kinetic molecular theory, all gases have the same average kinetic energy at the same temperature.

FALSE44) You would expect a gas at LOW pressures to behave like an ideal gas.

Gases act most ideally at low pressures and high temperatures.

FALSE45) The vapor pressure of a liquid will INCREASE as the temperature of the liquid increases.

The rate of evaporation increases, so there will be more gas particles present.

TRUE46) The boiling point of a liquid is the temperature at which the vapor pressure of water equals the atmospheric pressure.

The NORMAL boiling point of a substance occurs at 760 mm Hg or 1 atm

FALSE47) H2Ois predicted to have a HIGHER normal boiling point that H2S.

H2O exhibits hydrogen bonding while H2S will have dipole-dipole forces (H is not bonded to N, O, or F).

TRUE48) Thepolarizability of CCl4 should belargerthan that of CH4.

Polarizability depends on the total number of electrons present in a compound or atom.

TRUE49) A reaction with the general format AB + C--CB +A is a single replacement reaction.

FALSE50) omit this question

TRUE 51) When the [H+] is greater than the [OH-] in a solution, the pH of the solution will be less than seven.

TRUE 52) A substance that changes the activation energy of a reaction and is not permanently changed in the process is

called a catalyst

FALSE53) Hydrochloric acid can be classified as a polyprotic acid. It is monprotic

FALSE54) The freezing point of a pure substance is higher than a solution made of the substance. lower

FALSE55) The pH of a 0.25 M acetic acid solution can be found by the calculation: pH = -log[0.25]

Multiple Choice: Choose the best answer to each question.

56)When a solid substance undergoes a physical change to a liquid, which of the following is always true?

  1. A new substance is formed.d. It vaporizes.
  2. Heat is given off.e. It melts
  3. A gas is given off.

57)An empty container weighs 15.230 g. When filled with water (density = 1.00 g/ml), it weighs 35.920 g. When filled with an unknown liquid to the same mark as it was filled with water, it weighs 36.261 g. What is the density of the unknown liquid?

  1. 1.02 g/mld. 1.20 g/m3
  2. 1.02 g/m3e. none of the above.
  3. 1.20 g/ml

58)Which of the following is not an intensive property of a compound?

  1. chemical formulad. mass
  2. densitye. elemental composition.
  3. melting point temperature

59)A pure solid is heated and it decomposes into two substances, one a liquid and the other a gas. One can conclude with certainty that:

  1. The two products are elements.d. the liquid is a compound and the gas is an element.
  2. One of the two product is an elemente. Both products are compounds.
  3. The original solid is not an element.

60)Which of the following was not one of Dalton’s postulates for his Atomic theory?

  1. Matter is made up of small indestructible spheres called atoms.
  2. Atoms have a positive dense core that is surrounded by electrons.
  3. Atoms combined in small whole-number ratios to form elements.
  4. An atom can neither be created nor destroyed during a chemical or physical process
  5. They are all postulates of Dalton’s atomic theory.

61)The development of modern atomic theory took a leap forward with the proof that an atom is mostly empty space. Which of the following experiments was responsible for this proof?

  1. Millikan’s oil drop experiment.d. Separation of gases by gas chromatography
  2. Cathode-ray deflection in a magnetic fielde. The Wilson cloud chamber
  3. The bombardment of gold foil with alpha particles

62)What do these elements have in common: Na, K, and Cs?

  1. Metallic(5) Alkali metals
  2. Nonmetallic(6) Alkaline-earth metals
  3. Form cations(7) Halogens
  4. Form anions

a. 1 and 3b. 2 and 4c. 1, 4, and 7d. 1, 3, and 5e. 2, 4, and 6

63)What is the percentage mass of Al in aluminum oxide (Al2O3)?

  1. 26.46%d. 47.08%
  2. 20.93%e. 53.21%
  3. 52.92%

64)What is the mass of 4.25 x 1020 molecules of H2O?

  1. 0.127 gd. 142 g
  2. 0.0127 ge. 4.25 x 1020 g
  3. 1420 g

65)What is the coefficient in front of BF3 when the following equation is balanced?

BF3 + NaBH4 → NaBF4 + B2H6

  1. 1d. 4
  2. 2e. 5
  3. 3

66)Give the following information:

AgBr (s) + ½ Cl2 (g) → AgCl (s) + ½ Br2 (l) ΔH = -27.6 kJ

Which of the following statements concerning the reaction are true: (1) heat is released; (2) heat is absorbed; (3) the reaction is exothermic; (4) the reaction is endothermic?

  1. 1 and 3d. 2 and 3
  2. 2and 4e. 1 and 4
  3. 1 only

67)0.50 mol of ammonium nitrate is added to a 50.0 ml of water in a thermally insulated reaction vessel. Both are initially 20.0˚C. After stirring the temperature of the solution is found to be less than 10.0˚C. Which statement best explains the temperature change? (Temp goes down, which means the process is endothermic)

  1. Heat is evolved from the system to the surroundings.
  2. Heat is absorbed by the surroundings from the system.
  3. Heat is absorbed by ammonium nitrate when it dissolves and becomes hydrated.
  4. Heat is evolved by ammonium nitrate when it dissolves and becomes hydrated.
  5. The heat energy of the hydrated ions is lass than the ions in solid ammonium nitrate.

68)What is the energy of a photon that has a frequency of 9.00 x 1011 1/s?

  1. 1.66 x 10-45 Jd. 5.00 x 10-22 J
  2. 5.97 x 10-22 Je. 3.32 x 10-45 J
  3. 4.99 x 10-27 J

69)According to Bohr’s model of the atom, emission of electromagnetic radiation by heated atoms in a vacuum is directly due to which of the following?

  1. Photons absorbed by the atom
  2. Particle emission from the nucleus
  3. Momentum possessed by electrons
  4. Electrons being excited from a lower to higher energy level
  5. Electrons falling back from an excited state to their ground state.

70)Which of the following quantum numbers for an electron is not permissible?

  1. n = 5, l = 2, ml = 0d. n = 1, l = 0, ml = 0
  2. n = 3, l = 2, ml = 3e. n = 2, l = 1, ml = -1
  3. n = 4, l = 3, ml = -2

71)How many electrons are there in the outer energy level of arsenic?

  1. 3d. 6
  2. 4e. 7
  3. 5

72)Which elements have the lowest ionization energies?

  1. Those on the right side of the periodic tabled. Halogens
  2. Nonmetale. Both (a) and (b)
  3. Those on the left side of the periodic table

73)Why doesn’t sodium ordinarily occur in the 2+ ion state?

  1. low electron affinityd. small density
  2. high second ionization energye. large electronegativity
  3. large atomic radius

74)Based on its position on the periodic table, which atom has the largest atomic radius?

  1. Lid. Rb
  2. Nae. Cs
  3. K

75)Which element is considered a transition metal?

  1. Nad. Cu
  2. Cae. Al
  3. Cl

76)Which of the following is an exception to the general ionization energy trend?

  1. Nad. Ar
  2. Cae. P
  3. B

77)Which of the following is the largest in size?

  1. Cl-d. I+
  2. Cle. I-
  3. Na+

78)What is the electron configuration for Se-2?

  1. [He]2s22p4d. [Ar]4s23d104p6
  2. [He]2s22p6e. [Ne]3s23p2
  3. [Ar]4s23d104p4

79)What is the correct order of increasing radii for the isoelectronic series Rb+, Sr+2, Se-2, Br-?

  1. Rb+ < Sr+2 < Se-2 < Br-d. Sr+2 < Rb+< Br- < Se-2
  2. Br- < Se-2 < Sr+2Rb+e. None of the above
  3. Se-2 < Br-Rb+ < Sr+2

80)Which of the following compounds contains a double bond in its Lewis dot structure?

  1. N2d. NH4+
  2. SO2e. SO4-2
  3. Cl2

81)Which of the following possess π electrons?

  1. CH2Cl2d. (a) and (b)
  2. OCN-e. (b) and (c)
  3. N2O

82)In which of the following would you expect the central atom to use sp3d2 hybridization?

  1. PF5d. SiO2
  2. BrF5e. SO3
  3. CO2

83)A 15.0 L gas sample is heated from 29˚C to 67˚C at constant pressure conditions. Under these conditions, which of the following statements is correct?

  1. The number of moles of gas increases.d. The volume decreases.
  2. The number of moles of gas decreases.e. None of the above is correct.
  3. The volume increases.

84)A sample of CO2 (g) occupies 3.0 L at 35˚C at 1.0 atm. What is the new volume if the temperature and pressure are changed to 48˚C and 1.5 atm?

  1. 3.0 Ld. 4.3 L
  2. 1.9 Le. 2.1 L
  3. 4.7 L

85)Which of the following substances should have the highest melting point?

  1. Krd. CHCl3
  2. SO3e. H2O
  3. Ca(NO3)2

86)Which substance should exhibit hydrogen bonding in the liquid phase?

  1. SF4d. HBr
  2. CH3CH3e. CH3CH2NH2
  3. NaH

87)To an equilibrium mixture of 2 SO2 (g) + O2 (g)  2 SO3 (g), some helium, an inert gas, is added at constant volume. The addition of He causes the total pressure to double. Which of the following is true?

a.The concentrations of all three gases are unchanged.d. [SO3] increases.

b.The number of moles of SO3 increases.e. [SO2] increases.

c.The number of moles of O2 increases.

88)For a certain diprotic acid,H2X, Ka1 = 1 x 10−2 and Ka2 = 1 x 10−6. When the salt NaHX is dissolved in water, what is true about the pH of the resulting solution?

  1. pH < 7c. pH = 7
  2. pH > 7d. the pH can’t be determined

89)In general, as temperature goes up, the rate of a chemical reaction

  1. goes up if the reaction is exothermic
  2. goes up if the reaction is endothermic
  3. goes up regardless of whether the reaction is endothermic or exothermic.
  4. stays the sameregardless of whether the reaction is endothermic or exothermic.
  5. stays the same if the reaction is first order

90)A Bronsted/Lowry acid is defined as a substance that

  1. increases [H+] when placed in waterc. acts as a proton acceptor
  2. decreases [H+] when placed in waterd. acts as a proton donor

91)Which of the following is the conjugate base of acetic acid?

  1. C2H3O2-d. OH-
  2. H2C2H3O2+e. HC2H3O2+

c.H3O+

Free Response: Answer each of the following questions completely.

  1. Determine the correct number of significant digits in the following numbers.
  1. 0.00067 ml2d. 49600.0 g6
  2. 210.0 m4e. 200 rattlesnakesinfinite
  3. 0.040 L2
  1. Make the following temperature conversions.
  1. -70º F to ºC–56.7Cb. 480ºC to K753 Kc. 15ºF to K264 K
  1. What is Dalton’s atomic theory? Which postulates are no longer true? Why?
  1. All matter is composed of tiny, indivisible particles called atoms.
  2. All atoms of a given element have identical properties that different from those of other elements.
  3. Atoms cannot be created, destroyed, or transformed into atoms of another element during a chemical reaction.
  4. Compounds are formed when atoms of different elements combined with one another in small whole-number ratios.

Postulates I and II are no longer true. Postulate I is false, because of the existence of subatomic particles (protons, neutrons, and electrons). Postulate II is false, because not all atoms of the same elements are identical due to isotopes (a different number of neutrons) and ions (a different number of electrons).

  1. A 37Cl- atom of chlorine contains how many protons, electrons, and neutrons?

protons = 17, neutrons = 20, and electrons = 18

  1. Name the following compounds.
  1. CaSO4Calcium sulfatee. H2SO4 (aq)Sulfuric acid
  2. PF5 Phosphorus pentafluoridef. NaClO3Sodium chlorate
  3. KBr Potassium bromideg. Cu(CN)2Copper (II) cyanide
  4. Na2SSodium sulfide

Write the formula for the following compounds.

  1. Tin (IV) chlorideSnCl4e. calcium phosphateCa3(PO4)2
  2. Chromium (III) hydroxideCr(OH)3f. osmium tetraoxideOsO4
  3. Cesium cyanideCsCNg. sulfurous acidH2SO3
  4. Dinitrogen trioxideN2O3h. Hydroselenic acidH2Se
  1. Balance the following reactions, and then write the net ionic equation for each.
  1. AgNO3 (aq)+ CaCl2 (aq) → AgCl (s) + Ca(NO3)2 (aq)

2 AgNO3 (aq) + CaCl2 (aq)  2 AgCl (s) + Ca(NO3)2 (aq)

NET: Ag+ (aq) + Cl- (aq)  AgCl (s)

  1. VO (s) + Fe2O3 (s) → FeO (s) + V2O5 (s)

2 VO (s) + 3 Fe2O3 (s)  6 FeO (s) + V2O5 (s)

NET: Same as above.

  1. Na (s) + H2O (l) → NaOH (aq) + H2 (g)

2 Na (s) + 2 H2O (l)  2 NaOH (aq) + H2 (g)

NET: 2 Na (s) + 2 H2O (l)  2 Na+ (aq) + 2 OH- (aq) + H2 (g)

  1. NH4NO3 (s) → N2O (g) + H2O (l)

NH4NO3 (s)  N2O (g) + 2 H2O (l)

NET: Same as above.

  1. MnO2 (s) + HCl (aq) → Cl2 (g) + MnCl2 (aq) + H2O (l)

MnO2 (s) + 4 HCl (aq)  Cl2 (g) + MnCl2 (aq) + 2 H2O (l)

NET: MnO2 (s) + 4 H+ (aq) + 2 Cl- (aq)  Cl2 (g) + Mn+2 (aq) + 2 H2O (l)

  1. Write the balanced chemical equations for the following reactions, and determine the type of reaction.
  1. Aqueous silver (I) nitrate reacts with aqueous copper (II) chloride to form insoluble silver (I) chloride and aqueous copper (II) nitrate.

2 AgNO3 (aq) + CuCl2 (aq)  2 AgCl (s) + Cu(NO3)2 (aq); Double displacement.

  1. Aluminum metal reacts with oxygen gas to form solid aluminum oxide.

4 Al (s) + 3 O2 (g)  2 Al2O3 (s); Synthesis

  1. Aqueous barium chloride reacts with aqueous potassium sulfate to form solid barium sulfate and aqueous potassium chloride.

BaCl2 (aq) + K2SO4 (aq)  BaSO4 (s) + 2 KCl (aq); Double displacement.

  1. Solid potassium chlorate decomposes to solid potassium chloride and oxygen gas.

2 KClO3 (s)  2 KCl (s) + 3 O2 (g); Decomposition.

  1. Ethylene, C2H4, is used to make plastic polyethylene. How many moles of ethylene are there in 5.50 g?

0.196 mol C2H4(molar mass = 28.06 g/mol)

  1. How many atoms of oxygen are found in a 19.25 g sample of gallium nitrate?

4.08 x 1023(Ga(NO3)3)(molar mass = 255.74 g/mol)(9 mol O / 1 molGa(NO3)3)

  1. Cholesterol is made up of 83.87% C, 11.99% H, and 4.14% O. It has a molar mass of 386.64 g/mol. What is the molecular formula of cholesterol?

The molecular formula for cholesterol is C27H46O(Remember, use mole ratios to find empirical formula, then molar mass / empirical mass to find ratio for molecular formula)

  1. Given the following balanced reaction:

5 H2C2O4 + 2 KMnO4→ 4 H2O + 10 CO2 + 2 MnO2 + 2 KOH

  1. How many grams of CO2 are formed when 10.05 g of H2C2O4 and 26.72 g of KMnO4 are mixed together?

9.82 g CO2 (H2C2O is the limiting reagent) USE Stoichiometry!

  1. If the reaction produced 36.5 g of KOH, how many grams of H2O were also formed?

23.4 g H2O is formed.

  1. Determine the following for a sucrose solution.
  1. The number of moles of sucrose in 200.0 ml of a 0.345 M solution.

0.0690 moles sucrose(remember to convert volume to liters)

  1. The molarity of a solution containing 10.0 g of sucrose in enough water to make a 500.0 ml solution.

0.0584 M (sucrose is C12H22O11; molarity is moles solute / liter solution)

  1. Using the solubility rules, determine if the following compounds would be soluble or insoluble in water to a large extent.
  1. PbBr2 ISe. ZnSIS
  2. CsClSf. Ag2SO4IS
  3. Cu(C2H3O2)2Sg. Na2OS
  4. Mn(OH)2Sh.Ca3(PO4)2IS
  1. 10.30 ml of 0.150 M HCl is reacted with 11.25 ml of 0.1355 M NaOH. What is the limiting reactant?

NaOH is the limiting reactant. (Remember to start with a balanced equation, and then USE Stoichiometry.)

  1. What is the molarity of a solution of HC2H3O2 if 50.00 ml of the HC2H3O2 is reacted completelywith 25.86 ml of 0.1201 M NaOH?

0.0621 M HC2H3O2 (Again. Balanced equation, then stoichiometry!)

  1. Calculate the energy of a photon with a wavelength of 420 nm.

The energy of the wavelength is 4.73 x 10-19 J (c = λ ν; E = h ν) Must convert nm to m

  1. Calculate the wavelength of a photon of light that is given off when an electron in a hydrogen atom drops from the 4th energy level to the 2nd energy level.

The wavelength is 4.86 x 10-7 m or 486 nm. (E = RH(1/n2lo – 1/n2hi); c = λν)

  1. List three properties that distinguish metals from nonmetals.

Metals are shiny, ductile, malleable, and conduct electricity. Nonmetals are dull, brittle, and do not conduct electricity.

  1. For the following compounds, I) drawing the Lewis dot structure, II) determine the molecular geometry, III) Determine the hydridization of the central atom (sp3, ect.), and IV) Determine the polarity.

NOTE: unfortunately I can’t put the lewis dot structures on this sheet. See me if you are having problems.

  1. CS2 linear;sp; nonpolare. SO3Trigonal planar; sp2; nonpolar
  2. ICl linear; N/A; polarf. TeCl4See-saw; sp3d; polar
  3. ClF3T-shaped; sp3d; polarg. PF5Trigonalbipyramid sp3d;nonpolar.
  4. SF6 Octahedral; sp3d2; nonpolar
  1. A mixture of 2.00 g of O2 (g) and 3.25 g SO2 (g) will exert what pressure on the inside of a 2.00 L container at 27˚C?

The pressure on the container is 1.39 atm. ( Ptot = ntot R T / V)