First Semester Review Worksheet

  1. Determine the number of significant figures in each of the numbers below
  2. 1000
  3. 4.567
  4. 2030
  5. 0.0240
  6. 0.02677
  7. 200.00
  8. 4.65 x 104
  9. 100.300
  1. Convert the following units using dimensional analysis and report the answer in the correct number of significant figures:
  2. 2.50 cm = ? m
  3. 34.5 km = ? mm
  4. 700 g = ? kg
  1. How many protons, neutrons and electrons in each element?
  2. Plutonium-242
  3. Nitrogen-14
  4. Zinc-65
  5. Barium-137
  6. Tin-119
  1. Determine the charge of the following elements when they ionize:
  2. Strontium
  3. Nitrogen
  4. Iodine
  5. Beryllium
  6. Oxygen
  1. Name the following compounds:
  2. Ba(NO3)2
  3. CaSO3
  4. Ni(OH)2
  5. CuS
  6. Na2CrO4
  1. Write the formula for the following compounds:
  2. Magnesium carbonate
  3. Cobalt (III) acetate
  4. Carbon tetrachloride
  5. Silver (I) phosphate
  1. Explain the difference between mass number and atomic number.
  1. Determine the molar mass for the compounds in Q#6?
  1. How many moles would you have if you began with 7.50 grams of each one of the compounds in Q#6? How many formula units would be represented for each?
  1. Determine the percent composition of each element in the compoundsfromQ#6.
  1. Solid Aluminum burns in gaseous bromine producing aluminum bromide.
  2. Write the chemical equation for this reaction
  3. If you have 6.0g of Al, how much aluminum bromide would you produce?
  4. Determine the percent yield if you actually produce 2.03g of aluminum bromide.
  1. Explain the relationships among observation, hypothesis, experiment, theory and law, with respect to the scientific method.
  1. Using the scientific method, design a controlled experiment to determine how the water content of food influences how well it heats in a microwave oven.
  1. Give five examples of each, heterogeneous mixtures and homogeneous mixtures.
  1. Explain the difference between an element and a compound.
  1. Explain the difference between chemical and physical properties. Give an example of each.
  1. What is the sum of 2.7g + 2.47g expressed in the correct number of sig figs?
  1. What is the volume of an object with a mass of 6.00x102gand a density of 2.03g/cm3?
  1. The density of water is 1.0g/mL. What is the density of water in pounds/gallon? (1 quart = 9.46x10-1L; 1 g = 2.20x10-3lb.)
  1. Gold has sold for $500/ounce. Considering that there are 16 ounces (or 454 grams) in a pound, how many milligrams of gold could you buy for one cent?
  1. In what way are two isotopes of the same element different? Explain why isotopes of the same element have the same chemical behavior.
  1. There are four naturally occurring isotopes of the element chromium. Calculate the average atomic mass of chromium if the relative abundance of each isotope is:

50Cr = 4.31%52Cr = 83.76%53Cr = 9.55%54Cr = 2.38%

  1. Find the number of moles of argon in 481g of argon.
  1. What is the percent by mass of hydrogen in aspirin, C9H8O4?
  1. Balance the following equations:
  2. (NH4)2CO3 + NaOH → Na2CO3 + NH3 + H2O
  3. Na3PO4 + ZnSO4 → Na2SO4 + Zn3(PO4)2
  1. How many grams of CO are needed to react with an excess of Fe2O3 to produce 591 g Fe? Fe2O3(s) + 3CO(g) → 3CO2(g) + 2Fe(s)

VOCABULARY

Chemical Property

Chemical Reaction

Compound

Element

Gas

Heterogeneous Mixture

Homogeneous Mixture

Law of Conservation of Mass

Liquid

Matter

Mixture

Phase

Physical Change

Physical Property

Solid
Solution

Substance

Vapor

Alkali Metal

Alkaline Earth Metal

Atom

Atomic Mass

Atomic Mass Unit

Atomic Number

Cathode Ray

Dalton’s Atomic Theory

Electron

Period

Group or Family

Halogen

Isotope

Mass Number

Metal

Metalloid

Neutron

Noble Gas

Nonmetal

Nucleus

Period Law

Period Table

Transition Metal

Molecule

Molecular Compound

Ions

Cation

Anion

Ionic Compound

Chemical Formula

Molecular Formula

Formula Unit

Law of Definite Proportions

Monatomic Ions

Polyatomic Ions

Mole

Avogadro’s number

Representative particles

Gram Atomic Mass

Gram Molecular Mass

Gram Formula Mass

Molar mass

Standard Temperature and Pressure (STP)

Molar Volume

Percent Composition

Molecular Formula

Chemical Equation

Skeleton Equation

Catalyst

Coefficients

Balanced equation

Stoichiometry

Theoretical Yield

Actual Yield

Percent Yield

Percent Error

Mole Ratio

Things you Should Know and be able to do!

  • Summarize Dalton’s Atomic theory, know which are incorrect and which are still held as true
  • Describe the size of an atom
  • Know about the various models of the atom and their authors: Bohr, Rutherford, Thomson, Chadwick, Goldstein, and Schrodinger.
  • List the differences between the sub-atomic particles of an atom
  • Describe the structure of the atom, where are the protons, neutrons and electrons?
  • What is the atomic number?
  • Use the atomic number and the mass number to determine the number of p+, n°, e-
  • What is an isotope, how are they different?
  • Calculate the average atomic mass.
  • Identify the position and name of groups in the periodic table.
  • List the properties of metals and nonmetals.
  • Who are the authors of the periodic table and how did they each arrange the periodic table?
  • Describe periodic law and how this helps arrange the periodic table of elements.
  • Which concept is attributed to de Broglie? Heisenberg?
  • Know the periodic trends in radii, ionization energy, electron affinity and electronegativity.
  • What is matter?
  • What are the three states of matter and how do they differ?
  • What is the difference between a chemical change and a physical change, be able to give an example.
  • Categorize a sample of matter as a substance or mixture.
  • Distinguish between mixtures:homogeneous or heterogeneous
  • What is the difference between an element and a compound?
  • What is the law of conservation of mass?
  • Determine the number of significant figures when solving a mathematical problem
  • What’s the difference between accuracy and precision?
  • Convert a number to scientific notation
  • Solve conversions problems using Dimensional analysis
  • How do you solve for density?
  • What are the two methods for determining density?
  • Distinguish between ionic and molecular compounds.
  • Determine a molecules VSEPR shape using Lewis electron dot structures.
  • What is the octet rule?
  • Define cation & anion, relate them to metal and nonmetal
  • Write Electron Configurations
  • Know about the location of electrons in levels, sublevels, and orbitals.
  • Know the contributions of Puali, Hund, and Aufbau to the electron configuration of an element.
  • Distinguish among chemical formulas, molecular formulas, and formula units
  • Use the periodic table to determine the charge on an ion
  • Name and write formulas of molecular compounds
  • Name and write formulas for ionic compounds
  • List the properties of molecular and ionic compounds.
  • Know the difference between covalent and ionic bonding, polar and nonpolar bonding, and the different types of intermolecular attractions.
  • Interpret chemical equations
  • List indicators of a chemical reaction.
  • Perform Mole-Mole Calculations
  • Perform g to gram Calculations
  • Calculate percent yield and percent error of a reaction
  • Distinguish between theoretical and actual yield
  • Know how frequency and wavelength relate to one another.
  • What are Planck’s constant and the speed of light?
  • What are valence electrons and where are they located?
  • What is meant by the wave/particle duality of motion?
  • Know the polyatomic ions.
  • What is the difference between a theory, hypothesis, and law?
  • What is a mole and why was it needed in chemistry?
  • What is one mole equal to?
  • Calculate the molar mass of a compound
  • Convert between moles & mass
  • What is a mole of gas equal to at STP? What is STP?
  • Convert units using the metric system
  • Calculate the percent composition of an element in a compound
  • Balance chemical equations.
  • Write a balanced equation when given a word equation.

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