Chemistry and Chemistry Honors

Review Packet for Semester I Examination

Hint: Definitions of terms can and will be used in the construction of multiple choice and matching test questions

Chapter 1: Introduction to Chemistry

Be able to define the following terms:

MatterScientific law

Scientific methodChemistry

ObservationHypothesis

Theory

Responding variable (aka dependent variable)

Manipulated variable (aka independent variable)

You should be able to

1. Explain the difference between a hypothesis and a theory?

2. Describe the five steps of the scientific method.

3. Explain what you should do when you perform an experiment and get unexpected results

4. Explain the difference between a theory and a scientific law?

Chapter 13: States of Matter

Be able to define the following terms:

Kinetic energyBoiling point Critical Temperature

Kinetic theoryMelting pointCritical Pressure

Gas pressureAllotropes

VaporizationSublimation

EvaporationPhase diagram

Vapor pressureTriple point

Normal boiling point

You should be able to provide detailed answers to the following questions

Consider the following graph when answering questions 1 through 3


  1. What is thecritical temperature andcriticalpressure at the triple point?
  2. At what temperature and pressure will all three phases coexist? What is this point called?
  3. If you have a bottle of compound X at a pressure of 50 atm and temperature of 100C, what will happen if you raise the temperature to 600C?
  4. What phases are in equilibrium at a substances boiling point? At its melting point?
  5. What is the relationship between the rate of evaporation and the rate of condensation of a substance in a closed container that has constant vapor pressure?
  1. 6. Which particles in a liquid are the first to boil?
  2. What condition must exist for a liquid to boil?
  3. Why does the boiling point of a liquid vary with atmospheric pressure?
  4. Explain how evaporation lowers the temperature of a liquid. (think about the liquid’s kinetic energy)
  5. Is it easier to boil water at the top or bottom of a mountain? EXPLAIN.
  6. Is it possible to boil water at 105C instead of 100C? If so, how?
  7. Describe absolute temperature. What is the temperature in Celsius and Kelvin?
  8. Convert the following pressures: SHOW WORK FOR FULL CREDIT! (1 atm = 760 torr = 101.3 kPa = 760 mmHg)
  9. 0.95 atm  ? kPa
  10. 45 mm Hg ? Atm
  11. 7.563 Torr  ? mm Hg
  12. 0.003 kPa  ? Torr
  13. 3.2 atm  ? Torr
  14. 84.2 kPa  ? mmHg
  15. How does the gas pressure at sea level compare to the gas pressure in the mountains?

Chapter 4: Atomic Structure

Be able to define the following terms:

AtomAtomic numberGroup

ElectronsMass number

ProtonsIsotopes

NeutronsAtomic mass

NucleusPeriod

You should be able to

  1. Determine the number of neutrons, mass number, protons, and electrons from the information given
  2. Apply notation to designate isotopes
  3. Calculate atomic mass
  4. Explain why two isotopes can have different mass numbers, but must have the same number of protons.

Sample Questions

  1. The sum of the protons and neutrons in an atom equals the

a. atomic numberc. atomic mass.

b. number of electrons.d. mass number.

  1. Which of these statements is false?
  2. Electrons have a negative charge.
  3. Electrons hav a mass of 1 amu.
  4. The nucleus of an atom is positively charged.
  5. The neutron is found in the nucleus of an atom.
  1. How do the isotopes hydrogen-2 and hydrogen-3 differ?
  2. Hydrogen-3 has one more electron that hydrogen-2.
  3. Hydrogen-3 has two neutrons.
  4. Hydrogen-2 has three protons.
  5. Hydrogen-w has no protons.
  1. Which of these statement s is NOT true?
  2. atoms of the same elements can have different masses.
  3. The nucleus of an atoms has a positive charge.
  4. Atoms of isotopes of an element have different numbers of protons.
  5. Atoms are mostly empty space.
  1. An atom of an element with an atomic number 48 and a mass number 120 contains
  2. 48 protons, 48 electrons, and 72 neutrons.
  3. 72 protons, 48 electrons, and 48 neutrons.
  4. 120 protons, 48 electrons, and 72 neutrons.
  5. 72 protons, 72 electrons, and 48 neutrons
  1. Dalton theorized that atoms are indivisible and that all atoms of an element are identical. Scientists now know that
  2. Dalton’s theories are completely correct.
  3. atoms of an element can have different numbers of protons.
  4. atoms are all divisible.
  5. all atoms of an element are not identical but they all have the same mass.
  1. Which of the following is NOT a part of Dalton’s atomic theory?
  2. All elements are composed of atoms.
  3. Atoms of the same element are alike.
  4. Atoms are always in motion.
  5. Atoms that combine do so in simple whole-number ratios.
  1. If E is the symbol for an element which two of the following symbols represent isotopes of the same element?

1. 2. 3. 4.

  1. a. 1 and 2c. 1 and 4
  2. b. 3 and 4d. 2 and 3

9. Complete this table:

Element Name / Atomic Number / Mass Number / Number of Protons / Number of Neutrons / Number of Electrons
9 / 10
14 / 7
21 / 20
13 / 27
56 / 26

10. The element X contains three naturally occurring isotopes: X-36, X-38, and X-40. The relative abundance and atomic masses are

IsotopeRelative abundanceAtomic mass

X-360.337%35.978 amu

X-380.063%37.963 amu

X-4099.600%39.962 amu

The atomic mass of element X is

a. 41.25 amub. 4,125 amuc. 39.96 amud. 3, 996 amu

Chapter 25: Nuclear Chemistry

Be able to define the following terms:

Half-lifeRadioactivity

FissionRadiation

FusionRadioisotopes

Transmutation

Alpha particle

Beta particle

Gamma ray

You should be able to

  1. Balance an equation where beta or alpha decay has occurred
  2. Explain the difference between fusion and fission reactions
  3. Calculate the amount of time that has passed in the decay of a given isotope when given the fraction remaining, and the length of the half-life
  4. Identify the penetrating ability of alpha particles, beta particles and gamma rays.
  5. NOTE: Honors Chemistry only: Be able to use the formula time passed = (ln fraction remaining/-0.693) * length of half-life to determine the fraction of radioactive isotope remaining

Sample Questions

  1. Polonium is a naturally radioactive element decaying with the loss of an alpha particle.
  1. The half-life of a radioactive nuclide is the time it takes for
  2. 25% of the atoms to undergo radioactive decay.
  3. all the atoms to become nonradioactive.
  4. 50% of the atoms to undergo decay.
  5. none of the above
  1. Beta particles are
  2. electrons.
  3. protons.
  4. neutrons.
  5. helium nuclei.
  1. Thorium-234 undergoes beta decay. What is the other product of the decay?
  1. Gamma rays can penetrate
  2. paper
  3. wood
  4. skin
  5. all of the above
  1. Cesium-131 has a half-life of 30 years. How much of a 16 gram sample of cesium-131 will remain after 90 years?
  2. 0 gramsb. 8 gramsc. 4 gramsd. 2 grams
  1. A radioactive isotope has a half-life of 10.0 days. What fraction of the original sample is left after 30.0 days?
  2. 1/2b. ¼c. 1/8d. 1/16

Chapter 5: Electrons in Atoms

Be able to define the following terms:

Atomic orbitalPhoton

Energy levels

Ground state

Excited state

You should be able to explain the following in detail

  1. What was Dalton’s theory of atomic structure.
  2. What was J.J. Thomson’s contribution to our current knowledge of atomic structure? Why was his model called the plum pudding model?
  3. What was Ernest Rutherford’s contribution to our current knowledge of atomic structure?
  4. What was Neils Bohr’s contribution to our current understanding of atomic structures?
  5. Draw diagrams of Dalton’s, Thomson’s, Rutherford’s Bohr’s models of the atoms and the electron cloud model.
  6. Write the electron configuration for the following elements: Na, Ge, I, Hf
  7. Draw electron diagrams for the following elements: P, Nb, Ga
  8. 8. Chemistry Honors students only: Write the electron configuration for the Ca2+ion. Draw the orbital diagram for the O2-ion.

Chapter 6: The Periodic Table

Be able to define the following terms:

Alkali metalsElectronegativityMetalsTransition metal

Alkaline earth metalsHalogensNoble gases

AnionIonNonmetals

Atomic radiusIonization energyPeriodic law

CationMetalloidsRepresentative elements

You should be able to

  1. Explain the following period trends: electronegativity, ionization energy, atomic radius (size) as you go from left to right across a period and down a group
  2. Diagram these trends on a periodic table
  3. Locate the transition metals, metalloids, lanthanides, actinides, noble gases, alkali metals, nonmetals and alkaline earth metals found on the periodic table
  1. Identify the group that consists of the most reactive metals and most reactive nonmetals
  2. Define the octet rule and explain how it affects the periodic trends?
  3. Compare and contrast metals and non-metals.

Sample Questions

  1. In which of the following sequences are elements place in order of increasing ionization energy?
  2. Mg > Na > Cl > P > Si
  3. Na > Mg > Si > P > Cl
  4. Cl > P > Si > Mg > Na
  5. Si > P > Cl > Mg > Na
  1. In which of the following sequences are elements placed in order of increasing electronegativity?
  2. Mg > Na > Cl > P > Si
  3. Na > Mg > Si > P > Cl
  4. Cl > P > Si > Mg > Na
  5. Si > P > Cl > Mg > Na
  1. In which of the following sequences are elements placed in order of decreasing atomic radius?
  2. Mg > Na > Cl > P > Si
  3. Na > Mg > Si > P > Cl
  4. Cl > P > Si > Mg > Na
  5. Si > P > Cl > Mg > Na

For questions 4-6, Given the following elements Ba, Ra, Ca, Sr, Mg, Be

  1. In which of the follow sequences are the elements placed in order of increasing electronegativity?
  2. Ra < Ba < Sr < Ca < Mg < Be
  3. Ra > Ba> Sr > Ca > Mg > Be
  4. Be < Mg < Ca < Sr < Ba < Ra
  5. Be > Mg > Ca > Sr > Ba > Ra
  1. In which of the follow sequences are the elements placed in order of increasing atomic radius?
  2. Ra < Ba < Sr < Ca < Mg < Be
  3. Ra > Ba> Sr > Ca > Mg > Be
  4. Be < Mg < Ca < Sr < Ba < Ra
  5. Be > Mg > Ca > Sr > Ba > Ra
  1. In which of the follow sequences are the elements placed in order of increasing ionization energy?
  2. Ra < Ba < Sr < Ca < Mg < Be
  3. Ra > Ba> Sr > Ca > Mg > Be
  4. Be < Mg < Ca < Sr < Ba < Ra
  5. Be > Mg > Ca > Sr > Ba > Ra
  1. What element is a halogen in the 4th period?
  2. Fb. Clc. IBr
  1. Where are the alkali metals found on the periodic table?
  2. Group 1b. Group 2c. group 17 (7A)d. Group 18 (8A)
  1. What noble gas is the smallest?
  2. Heb. Nec. Ard. Xe
  1. How are the elements arranged on the periodic table?
  2. Increasing atomic mass
  3. Increasing atomic number
  4. Increasing size
  5. Increasing ionization energy
  1. Which of the following is a characteristic of nonmetals?

a. lusterb. malleablec. ductiled. brittle

  1. Which of these metals isn’t a transition metal?

a. aluminumb. ironc. silverd. zirconium

  1. Which element in each pair has atoms with a larger atomic radius?
  2. sodium, lithium
  3. strontium, magnesium
  4. carbon, germanium
  5. selenium, oxygen
  1. Which particle has the larger radius in each atom/ion pair?

a. Na, Na+c. I I-

b. S, S2-d. Al, Al3+

Chapter 7: Ionic and Metallic Bonding

Be able to define the following terms:

AlloysIonic BondsValence electrons

Chemical formulaIonic compounds

Electron dot structureMetallic bonds

Formula unitOctet rule

You should be able to

  1. Identify the type of compound (ionic or covalent) based on the elements in the compound
  2. Identify the characteristics of ionic compounds
  3. Draw electron dot diagrams for elements 1 through 20
  4. Explain what is meant by “sea of electrons” when referring to metallic bonds.
  5. Explain the octet rule

Sample questions:

  1. Which of the following pairs of elements will form an ionic compound?
  2. sulfur and oxygenc. sodium and calcium
  3. sodium and sulfurd. oxygen and chlorine
  4. Which of the following is NOT a characteristic of ionic compounds
  5. they have high melting points
  6. they are brittle
  7. they conduct electricity when melted or dissolved in water
  8. they consist of metals and nonmetals
  9. Which of the following ions is formed by phosphorus
  10. P1+b. P3+c. P1-d. P3-
  11. Which of the following formulas is correct?
  12. KS2b. CaOc. Al3N3d. Mg3N2

Chapter 8: Covalent Bonding

Be able to define the following terms

Covalent bondPolyatomic ion

Diatomic moleculeMolecular formula

Molecular compound

You should be able to

  1. draw Lewis structures for covalent compounds (i.e. molecules) similar to those completed in class: Examples CH3OH, CCl4, HCN, NH3,
  1. Honors Chemistry students only: you should be able to identify the electron and molecular geometries using Lewis structures
  2. Compare and contrast the properties of ionic and covalent compounds:

Sample:

Which of the following is NOT a characteristic of a covalent compound?

a. low melting point

b. brittle

c. conduct electricity when melted or dissolved in water

d. all of the above are characteristics of covalent compounds

Chapter 9: Chemical Names and Formulas

You should be able to

  1. Name covalent and ionic compounds based on their chemical formulas
  2. Write the chemical formula of an ionic or covalent compound based on the name of the compoun

Sample Questions

  1. The formula for the compound formed from ammonium and sulfate ions is
  2. NH4SO4b. (NH4)2SO4c. NH4(SO4)2d. (NH4)3SO4
  1. The correct name for CU2O is
  2. copper oxide.b. copper (I) oxide.c. copper (II) oxide.d. dicopper monoxide.
  1. The name of the compound PI3 is
  2. phosphorus (III) iodide.c. phosphorus triiodide.
  3. b. monophosphorus triiodide.d. phosphorus iodide.
  1. The formula for the compound diphosphorus pentaoxide is
  2. P2O5.b. PO4O5.c. P5O2.d. none of the above
  1. The name of the compound K3P is
  2. potassium (III) phosphide.c. potassium phosphide.
  3. tripotassium monophosphide.d. potassium triphosphide.

Chapter 11: Chemical Reactions

Be able to define the following terms:

Catalyst

Chemical equations

Single replacement reaction

Double replacement reaction

Combination (Synthesis) reactions

Decomposition reaction

Combustion reaction

You should be able to

  1. Classify a reaction as combination, single replacement, double replacement, combustion or decomposition
  2. Balance equations.

Sample Questions

Use the following key to classify the reactions in questions 1 through 5

Key:

  1. Combination (synthesis) reaction
  2. Decomposition reaction
  3. Single replacement reaction
  4. Double replacement reaction
  5. Combustion reaction
  1. 2NaNO3(s)  2NaNO3(s) + O2(g)
  2. ib. iic. iiid. ive. v
  1. O2(g) + 2Mg  2MgO
  2. ib. iic. iiid. ive. v
  1. H2SO4(aq) + 2KOH(aq)  K2SO4(aq) + 2H2O(l)
  2. ib. iic. iiid. ive. v
  1. 2C6H14(g) + 19O2(g)  12CO2(g) + 14H2O(l)
  2. ib. iic. iiid. ive. v
  1. Pb(s) + 2AgNO3(aq)  Pb(NO3)2(aq) + 2Ag(s)
  2. ib. iic. iiid. ive. v

Balance the following equations in questions 6 through 10:

  1. _____Al2O3 + _____H2SO4 _____Al2(SO4)3 + _____H2O
  1. _____H2S + _____O2 _____2SO2 + ____H2O
  1. _____Br2 + _____KI  _____I2 + _____KBr
  1. _____Al + _____O2 _____Al2O3
  1. _____C3H8 + _____O2 _____CO2 + _____H2O