Name:

Semester Review Packet

Directions: Answer the following questions below. Show all work for full credit, label all units, put all calculation answers in correct scientific notation and significant figures and BOX all answers.

Chapter 1 & 2

  1. What is the difference between a scientific theory and a scientific law?
  1. Explain in detail each step of the scientific method.
  1. What is the difference between a solution and a mixture? Give an example of each.
  1. What is the difference between a compound and an element? Give an example of each.
  1. Explain the difference between matter, mass and a substance. Give an example of each.
  1. Identify each of the following as a chemical change or physical change.
  1. growing grass______
  2. sugar dissolving in water______
  3. crushing a rock______
  4. boiling water______
  5. cooking a steak______
  1. Define the law of conservation of mass.
  1. Give the number of significant figures in each of the following numbers:
  1. 2.01______
  2. 3.10000______
  3. .0031______
  4. 3.000000______
  5. 201______
  1. Three different people weigh a standard mass of 2.00 g on the same balance. Each person obtains a reading of 7.23 g. These results imply that the balanced that was used was:
  1. accurate
  2. precise
  3. accurate and precise
  4. neither accurate nor precise
  1. The diameter of a carbon atom is .0000000000154 m. What is this number in scientific notation as well as the number of significant figures? ______
  1. Classify each measurement as qualitative or quantitative:
  1. The basketball is brown ______

b. The diameter of basketball is 31 centimeters. ______

  1. The basketball is 12 pounds ______
  1. Give the SI unit and symbol for each of the following:
  1. length ______
  2. volume______
  3. mass______
  4. density______
  5. pressure______
  6. time______
  7. amount of a substance______
  1. Explain the difference between mass and weight.
  1. What is the temperature 25° C expressed in Kelvin.
  1. The copper penny has a mass of 3.1 g and a volume of .35 cm3. What is the density of copper?

Answer: ______

Chapter 3:

Show all work for full credit, use dimensional analysis, label all units and all answers must show proper scientific notation and significant figures.

Make sure you know the International System of Units, Prefixes and Conversion factors!

  1. What is the mass of a bone that has a volume of 80.0 cm3 and a density of 1.5 g/cm3?

Answer: ______

  1. Convert 50.1 cm to km:Answer: ______
  1. Convert 0.45 ng to mg:Answer: ______
  1. Convert 10.5 ml to L:Answer: ______

Chapter 4:

  1. What are the parts of Dalton's Atomic Theory?
  1. How did the following people contribute to the development of the atomic theory?
  1. Goldstein
  1. Chadwick
  1. Thompson

d. Rutherford

3. How was a cathode ray tube used to discover the subatomic particles in question #2?

  1. An atom is identified as platinum -95.
  1. What is the number 195 called? ______
  2. Write the symbol for this atom using subscripts to show the mass number and atomic number. ______
  1. Complete the following table:

Atomic Number / Mass Number / Number of Protons / Number of Neutrons / Number of Electrons
5
15
11
  1. Name two ways that the isotopes of an element are different and two ways that they are similar.
  1. What is the difference between mass number and atomic mass?

Chapter 5:

  1. The region around the nucleus where the electron is likely to be moving is called a/an ______.
  1. The probability of finding an electron within a certain volume of space surrounding the nucleus can be portrayed as a ______.
  1. In the quantum mechanical model, the cloud shapes are called ______.
  1. Which scientist developed the quantum mechanical model of the atom? ______
  1. How many orbitals are in the following sublevels?
  1. 3d sublevel ______b. 2p sublevel ______c. 4f sublevel ______
  1. How many unpaired electrons are there in a phosphorus atom? ______
  1. How many paired electrons are there in a Oxygen atom? ______
  1. What is it meant by 4p5? ______
  1. What is the maximum number of electrons allowed in one atomic orbital? ______
  1. Draw the orbital diagrams for the following elements:
  1. P: ______
  1. Write the complete electron configuration for the following elements:
  1. Ag: ______
  1. How many electrons are in the highest occupied energy level of these atoms?

a. Strontium ______b. Magnesium ______c. Gallium ______

  1. What is the maximum number of electrons that can go into each of the following sublevels?

a. 2s ______b. 4p ______c. 5f ______d. 3d ______

  1. Write the noble gas electron configuration and orbital diagrams for the following elements:
  1. Rn: ______

______

  1. Y+3: ______

______

  1. U: ______

______

  1. Write the electron configuration and orbital diagrams for the following elements:
  1. Ca: ______

______

  1. Ar: ______

______

  1. Cl-: ______

______

  1. Arrange the following electromagnetic radiations in order of decreasing wavelengths.

a. green lightb. infrared radiation from a heat lampc. ultraviolet light from the sun

d. dental X-rayse. the signal from a short-wave radio station

Answer: ______

  1. List the colors of the visible spectrum in order of increasing wavelengths.

Answer: ______

Use the following information for problems #18-20. A mercury lamp emits radiation with a wavelength of 6.15 x 107 m and has a velocity of 2.5 x 108 m/s.

  1. What is the energy of this light?
  1. What is the mass of the photon of light?
  1. In what region of the electromagnetic spectrum is this radiation?______
  1. A quanta of light is called a/an: ______.
  1. Electrons that are ejected by metals when light shines on them are called ______.
  1. The energy state higher than the ground state is known as the ______.
  1. Who developed the Uncertainty Principle? ______
  1. In complete sentences, explain what is the Uncertainty Principle?

Chapter 6 Review

  1. For the elements whose outermost electron configurations are given below, tell the period and group to which each belongs:

SymbolElement NamePeriodGroup

  1. 6s1
  2. 5s25p4
  3. 3s23p2
  1. Arrange the following elements in order of decreasing ionization energy (highest  lowest).
  2. Ca, Ba, Be, Sr ______
  3. Cl, Si, P, Ar ______
  4. Cs, Li, K ______
  5. Tell whether each of the following elements is an inner transition metal, noble gas, alkali metal, alkaline earth metal, halogen, or transition metal.
  6. K ______
  7. Cl ______
  8. Gd ______
  9. Circle the element of the following pairs that has the higher electronegativity:

a. Na, Mgb. Rb, Ic. Cl, Br

  1. Circle the element of the following pairs that has the larger atomic radius?
  1. Cl, Cl-
  2. Mg, Mg2+
  1. Explain why fluorine has a smaller atomic radius than both oxygen and chlorine.
  1. What where the contributions of each of the following scientists to the development of the periodic table?
  1. Mendeleev
  1. Moseley
Chapter 7:
  1. Complete the following table:

Dot Structure of atom / Dot Structure of ion / Formula of ion / Type of ion (cation or anion)
Rn
F
O
H
  1. Draw the formation of the ionic compound for the following. Include (a) electron dot structure for both elements, (b) arrows illustrating the loss or gain of electron(s), (c) the charge of both elements, (d) label reactants as metal or nonmetal, and (e) write the formula for the compound and the name.

Aluminum and oxygen

Chemical Formula:Chemical Name:

  1. What is metallic bonding? What properties of metals are explained by metallic bonding?
  1. Why are substances made up of ionic compounds called “formula units” instead of molecules?
  1. When you put an ionic compound, like sodium chloride into water, what happens to the compound?

If you then apply a power source, such as a battery and insert electrons into the solution, where do the sodium atoms go? (See diagram on page 198).

Chapter 8:

  1. What is a polar bond?
  1. Draw electron dot structures for the following. The drawing should show the correct geometry. Label the electronegativity of each atom. Draw arrows to show the polarity of the bond, if it is polar.

HCN

Molecule Name:

Molecule Geometry:

Polar or Non polar:

Intermolecular Forces:

CO2

Molecule Name:

Molecule Geometry:

Polar or Non polar:

Intermolecular Forces

NH3
Molecule Name:
Molecule Geometry:
Polar or Nonpolar
Intermolecular Forces
SCl2
Molecule Name:
Molecule Geometry:
Polar or Nonpolar
Intermolecular Forces

3. Rank the following from strongest intermolecular attractive force to weakest:

___ dipole interactions___ dispersion forces___ hydrogen bonding

Chapter 9:

  1. What is difference between a cation and an anion.

How is each formed?

  1. Which groups of elements on the periodic table are cations and which group of elements are anions? List the charges of each group.
  1. Complete the following table. Write the chemical name and the chemical formula for the compounds formed.
  1. Complete this table:

Symbol of Element / Change in electrons / Formula of ion / Name of ion
Be
  1. Give the chemical name or write the chemical formula for the following Binary Molecular Compounds or Acids:
  1. SF6______
  2. N2O5______
  3. P4O10______
  4. Phosphorus Heptachloride______
  5. Acetic Acid______
  6. H2SO4______
  7. CaCl2______
  8. FeO______
  9. Chromium(III) oxide______
  10. Hydrosulfuric acid______
  11. MnO2

Chapter 10:

Answer all questions in the space provided. Show all work for full credit, label all units and put all answers in scientific notation and significant figures.

  1. What is the number of moles in 452 g of Krypton?Answer: ______
  1. How many molecules are there in 1.43g of glucose, C6H12O6?Answer: ______
  1. Calculate the number of atoms in 5.78 mol of sucrose, C12H22O11.Answer: ______
  1. Calculate the volume, in liters, of 3.24 x 1022 molecules of CO2 at STP.Answer: ______
  1. What is the percent of hydrogen, in grams, in aspirin, C9H8O4?Answer: ______

Chapter 25 Review

  1. Distinguish between alpha particles, beta particles, and gamma rays. Indicate how the atomic number and atomic mass number change when each type of radiation is emitted.
  1. Complete the following nuclear reactions
  2. 14N + ____  14C + 1H
  3. 55Mn + 2H  ______+ 2 1n (neutron)
  4. 222Rn 218Po + ______
  1. Who discovered radioactivity?
  1. Why do radioactive isotopes emit radiation?
  1. What particle is emitted in alpha radiation?
  1. What type of radiation is the most penetrating?
  1. Above which atomic number are the transuranium elements?
  1. What is nuclear fission and name two applications for fission.
  1. What is nuclear fusion. Where does it occur naturally?

Note: This is a cumulative final; therefore you are responsible for every lecture, lab, and anything else that has been taught since the first day of school. Remember this is just a review guide it is impossible to put everything that has been taught on this review worksheet.