CHEMISTRY HONORS
LEOCE Study Guide
CHEMISTRY AND SCIENTIFIC MEASUREMENT
BENCHMARK: N.1.1-1.2, N.1.6, N.3.1, N.3.3, N.3.4
TEXTBOOK: Glencoe, Chemistry: Matter and Change, Chapters 1-3
ESSENTIAL QUESTION: How is measurement applied to science? How do we classify matter?
KEY VOCABULARY: density, significant figures, scientific notation, dimensional analysis, compound,
element, mixtures, homogeneous, heterogeneous
STUDENT TASKS:
1. Be able to classify matter.
2. Be able to interpret data.
3. Be able to use correct significant figures
4. Be able to convert units.
SAMPLE QUESTION:
1. After performing a density lab in which the student places an irregularly shaped object in a
cylinder, the student records the following data.
Volume and Mass Data
Mass of sample
Volume of water
Volume of water + sample
20.46 g
40.0 mL
43.0 mL
What is the density based on the data above? Round your answer to the correct number of
significant figures.
Ⓐ .478 g/mL
Ⓒ .147 g/mL
Ⓑ 6.82 g/mL
Ⓓ 2.10 g/m
2. How many significant figures are in the measurement of the mass of the sample?
Ⓐ 1
Ⓒ 3
Ⓑ 2
Ⓓ 4
ATOMIC STRUCTURE
BENCHMARK: SC.912.P.8.4
TEXTBOOK: Glencoe, Chemistry: Matter and Change, Chapters 4, 5
ESSENTIAL QUESTION: How are the electrons arranged?
KEY VOCABULARY: valence electrons, electron configuration, orbital, sublevels, unpaired electrons,
Aufbau diagram, isotopes
STUDENT TASKS:
1. Identify maximum number of electrons in a sublevel.
2. Identify unpaired valence electrons in an atom and shared pairs in a molecule.
3. Identify valence electrons in a family or group.
4. Write electron configuration of a neutral atom for elements 1-36.
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CHEMISTRY HONORS
LEOCE Study Guide
5. Be able to identify an electron configuration in an Aufbau diagram.
6. Be able to identify the number of protons, neutrons, and electrons in a given atom, isotope, or
ion.
7. Distinguish between the isotopes of elements.
SAMPLE QUESTION:
1. What are the maximum number of electrons that can fill the p-sublevel?
Ⓐ 2
Ⓒ 6
Ⓑ 4
Ⓓ 8
2. How many neutrons would be contained in an atom of the isotope uranium – 238 (23892 U)
Ⓐ 238 neutrons
Ⓒ 52 neutrons
Ⓑ 92 neutrons
Ⓓ 146 neutrons
PERIODIC TABLE
BENCHMARK: SC.912.P.8.5
TEXTBOOK: Glencoe, Chemistry: Matter and Change, Chapter 6
ESSENTIAL QUESTION: What are the fundamental trends in the periodic table?
KEY VOCABULARY: electronegativity, ionization energy, atomic radius, reactivity, family/group, period,
valence electrons, halogens, alkali metal, alkaline earth metals
STUDENT TASKS:
1. Place elements in order of atomic size.
2. Describe the trend for electronegativity.
3. Place elements in order of ionization energy.
4. Compare the characteristics of elements within the same family/group.
SAMPLE QUESTION:
1. Which of the following atoms has the highest electronegativity?
Ⓐ Na
Ⓒ P
Ⓑ F
Ⓓ Rb
2.Which of the following elements has the largest atomic radius?
Ⓐ O
Ⓒ Se
Ⓑ S
Ⓓ Te
IONIC COMPOUNDS
BENCHMARK: SC.912.P.8.7
TEXTBOOK: Glencoe, Chemistry: Chapter 7
ESSENTIAL QUESTION: What are ionic compounds?
KEY VOCABULARY: ionic bonding, anion, cation, ionic bond, polyatomic ions
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CHEMISTRY HONORS
LEOCE Study Guide
STUDENT TASKS:
1. Differentiate between anion and cation.
2. Define an ionic compound.
3. Write formulas or names for ionic compounds.
SAMPLE QUESTION:
1. What is the formula for Calcium acetate?
Ⓐ CaC2H302
Ⓑ Ca(C2H302)2
Ⓒ Ca2C2H302
Ⓓ CaC204
2. What is the formula for copper (II) chloride?
Ⓐ CuCl
Ⓒ Cu2 Cl2
Ⓑ CuCl2
Ⓓ Cu2Cl
COVALENT MOLECULES
BENCHMARK: SC.912.P.8.7
TEXTBOOK: Glencoe, Chemistry: Chapter 8
ESSENTIAL QUESTION: How are shapes and interactions between molecules explained? What is a
covalent bond?
KEY VOCABULARY: linear, tetrahedral, pyramidal, bent, trigonal planar, bond angles, polar and
nonpolar molecule, Octet Rule, shared pairs, unshared pairs, VSEPR Theory, covalent bond, Lewis dot
diagram, Lewis structure
STUDENT TASKS:
1. Identify covalently bonded molecules.
2. Identify the molecular shape, bond angle, and polarity.
3. Write formulas or names for covalent molecules and acids
4. Identify a correct Lewis structure for a molecule.
SAMPLE QUESTION:
1. What is the molecular shape of H2O and is it polar or nonpolar?
2.
In accordance with the octet rule, what is the total number of shared pairs of electrons in the
BMO of an oxygen molecule?
Ⓐ 1
Ⓒ 3
Ⓑ 2
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Ⓓ 4
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CHEMISTRY HONORS
LEOCE Study Guide
CHEMICAL REACTIONS
BENCHMARK: SC.912.P.8.8
TEXTBOOK: Glencoe, Chemistry: Chapter 9
ESSENTIAL QUESTION: How do chemical changes occur when substances interact?
KEY VOCABULARY: products, reactants, coefficients, combination/synthesis, decomposition, single
replacement, double replacement, combustion, Law of Conservation of Matter, precipitate
STUDENT TASKS:
1. Identify 5 types of chemical reactions.
2. Be able to complete and balance chemical reactions.
3. Understand Law of Conservation of Matter.
4. Identify the precipitate(s) and aqueous solution (aq) in a double replacement reaction.
SAMPLE QUESTION:
1. Complete and balance the following reaction.
___NaOH(aq) + ___CuCl2
___NaCl + ________
3.
Ⓐ CuOH:
1,1,1,1
Ⓑ CuOH:
2,1,2,1
Ⓒ Cu(OH)2:
2,1,2,1
Ⓓ Cu(OH)2:
1,1,1,1
In the complete combustion reaction of methane, CH 4, what is the coefficient in front of the
oxygen, O2?
Ⓐ 1
Ⓒ 3
Ⓑ 2
Ⓓ 4
MOLAR CALCULATIONS
BENCHMARK: SC.912.P.8.9
TEXTBOOK: Glencoe, Chemistry: Chapters 10, 11
ESSENTIAL QUESTION: How is stoichiometry used to calculate chemical quantities from balanced
chemical equations?
KEY VOCABULARY: representative particles, empirical formula, molecular formula, standard
temperature and pressure (STP), percent composition, limiting reagent, excess reagent, mole,
stoichiometry, mole ratio, molar mass, skeleton equation
STUDENT TASKS:
1. Perform mole conversions.
2. Calculate percent composition.
3. Perform mass to mass, mass to volume, volume to volume, moles to mass stoichiometric
calculations.
4. Solve for the limiting reactant.
5. Compare and identify empirical and molecular formula.
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CHEMISTRY HONORS
LEOCE Study Guide
SAMPLE QUESTION:
1. When 15.0 g of Copper (II) sulfate reacts with powered aluminum according to the reaction
below, how many grams of Cu could be collected from this reaction?
3CuSO4 (aq) + 2Al (s)
Ⓐ 23.5 g Cu
Al2(SO4)3 (aq) + 3Cu (s)
Ⓒ 52.9 g Cu
Ⓑ 5.97 g Cu
2.
Ⓓ 31.5 g Cu
What is the number of representative particles in 0.50 moles of O 2?
Ⓐ 1.2 x 1024 atoms
Ⓒ 3.0 x 1023 atoms
Ⓑ 1.2 x 1024 molecules
Ⓓ 3.0 x 1023 molecules
STATES OF MATTER AND INTERMOLECULAR FORCES
BENCHMARK: SC.912.P.8.1, P.8.6, P.10.5
TEXTBOOK: Glencoe, Chemistry: Chapter 12
ESSENTIAL QUESTION: How do changes in the kinetic energy of particles affect the state of
substances?
KEY VOCABULARY: solid, liquid, gas, vaporization, condensation, melting point, boiling point,
sublimation, triple point, London dispersion force, hydrogen bonding, dipole – dipole, critical point
STUDENT TASKS:
1. Identify phase changes and interpret a phase diagram as shown above (page 429).
2. Identify the strengths of the intermolecular forces.
SAMPLE QUESTION:
1. What are the forces of attraction in a nonpolar molecular substance?
Ⓐ dipole – dipo
Ⓒ London dispersion
Ⓑ ionic bond
Ⓓ hydrogen bonding
2
What state of matter is the substance in section A?
3.
What phase change occurs as a substance transitions from A directly to C?
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CHEMISTRY HONORS
LEOCE Study Guide
GASES
BENCHMARK: SC.912.P.12.10
TEXTBOOK: Glencoe, Chemistry: Chapter 13
ESSENTIAL QUESTION: What are the properties of an ideal gas?
KEY VOCABULARY: ideal gas law, quantitative, real gas, combined gas law
STUDENT TASKS:
1. Perform calculations using the combined gas law and ideal gas law.
2. Know the assumptions and deviations of the ideal gas law.
3. Understand the relationship between temperature, volume, and pressure of gas.
SAMPLE QUESTION:
1. What is the mass of 4.0L of oxygen gas (O2) at 4.0 ATM and 25°C?
Ⓐ 10.0g O2
Ⓑ 15.2g O2
Ⓒ 20.9g O2
Ⓓ 25.4g O2
2.
According to the reaction below, how many liters of waters are produced from 10.0 L of O 2 ?
2H2 (g) + O2 (g)
Ⓐ 10.0 L
Ⓑ 20.0 L
2H2O (g)
Ⓒ 22.4 L
Ⓓ 40.0 L
REACTION RATES
BENCHMARK: SC.912.P.12.12
TEXTBOOK: Glencoe, Chemistry, Chapter 16 Section 2
ESSENTIAL QUESTION: What factors affect the rate of reaction?
KEY VOCABULARY: catalyst, concentration, rate of reaction, particle size, temperature
STUDENT TASKS:
1. Identify the factors that affect the rate of reaction.
2. Describe the role of a catalyst in the rate of reaction.
3. Understand the relationship between temperature and frequency of collision.
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CHEMISTRY HONORS
LEOCE Study Guide
SAMPLE QUESTION:
1. Solid magnesium is reacted with hydrochloric acid, (HCL). Which choice below would react
the fastest?
Ⓐ Magnesium ribbon in 1M HCl
Ⓑ Magnesium ribbon in 2M HCl
Ⓒ Magnesium powder in 1M HCl
Ⓓ Magnesium powder in 2M HCl
2.
Which of the following is a characteristic of a catalyst?
Ⓐ increase the pressure of the reaction
Ⓒ slows down the rate
Ⓑ is consumed in the reaction
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Ⓓ lowers the activation energy
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