Name: ______Date: ______Period: ______

Chemistry Student Learning Objective Review Part 1

Unit 1: Measurements and Calculations (Chapter 1 and 3)

  1. Give the number of significant digits in each of the following measurements:

a)1278.50 / b)0.00730 / c)90027.00
d)8.002 / e)670 / f)0.0053567
g)43.050 / h)120000 / i)0.147
  1. Round the following numbers to the designated # of significant figures

Original Number / Round to 5 sig. figs. / Round to 4 sig. figs. / Round to 2 Sig. figs.
a)4.5361946
b)125000
c)0.0009548947
d)876493
  1. Perform the following calculations and round the answer to the correct number of significant figures.

a)23.4 x 14 = / b)105.15 + 273 =
c)7.895 + 3.4 = / d)0.25 ÷ 0.0005 =
e)7.895 ÷ 34 = / f)11.14 – 4.273 =
g)0.005 - 0.0007 = / h)0.0945 x 1.47 =

Unit 2: Matter & Changes Chapter 2

  1. Define and give an example of the following classification of matter

Classification / Define / Example
a)Pure Substance
b)Element
c)Compound
d)Mixture
e)Homogeneous Mixture
f)Heterogeneous Mixture
  1. Using the diagram to the right label phases present at each point in the diagram

a)______

b)______

c)______

d)______

e)______

  1. Describe the changes in potential and kinetic energy at each point above.

a)PE______, KE______d) PE______, KE______

b)PE______, KE______e) PE______, KE______

c)PE______, KE______f) PE______, KE______

  1. Give the name of the phase change described and state if it is endothermic or exothermic

Transition / Name / Endothermic/Exothermic
a)Gas to liquid
b)Liquid to gas
c)Solid to liquid
d)Liquid to solid
e)Gas to solid
f)Solid to gas
  1. Identify the following as chemical or physical changes/properties

  1. table salt
  2. gold
  3. the air in DHS
  4. carbon
  5. Kool-aid
  6. fruit salad
  7. city air
/
  1. Salad dressing
  2. hydrogen chloride (HCl)
  3. beach sand
  4. water from water fountain
  5. Lucky charms cereal
  6. pure water
  7. sodium
/
  1. wood
  2. blood
  3. milk
  4. oily water
  5. soil (dirt)
  6. oxygen
  7. glucose

  1. boiling water
  2. burning gasoline
  3. cooking an egg
  4. ironing a shirt
  5. evaporating alcohol
  6. rusting iron
  7. water evaporates.
/
  1. Ripping paper
  2. Steel turns red when heated
  3. fermenting orange juice
  4. Ar is very nonreactive.
  5. rocks are ground to sand.
  6. digesting a pizza
  7. an ice melting in a drink
/
  1. decomposing meat
  2. evaporating water
  3. sulfur is burned.
  4. titanium is an inert metal.
  5. Na is a soft, shiny metal.
  6. ice melts at 0°C
  7. silverware tarnishes.

Unit 3: Atomic History and Atomic Structure Chapter 4

  1. How has the model of the atom changed over time [1st model to current model]
  1. Describe the charge, relative size and location of subatomic particles

Particle / Charge / Size / Location
a)Proton
b)Neutron
c)Electron
  1. Flame lab: Describe why did the compounds emitted light when placed in a flame [use terms: excited state and ground state]
  1. What ion (charge and number) does the following element from to achieve stable electron configuration

Element / Ion / Element / Ion
a)Gallium / b)Calcium
c)Cesium / d)Iodine
e)Sulfur / f)Phosphorous
g)Potassium / h)Chlorine
  1. Determine the number of protons, neutrons, and electrons for the following elements/isotopes

Element / Protons / Neutrons / electrons
Magnesium
Hydrogen-2
Sulfur
Uranium-235
Cobalt
Carbon-14
Rubidium-87
  1. Determine the average atomic mass for the elements listed below. Show ALL work

a)A sample of iodine has 80% I-127, 17% I-126, and 3 % I-126

b)

c)Uranium is used in nuclear reactors and is a rare element on earth. Uranium has three common isotopes. If the abundance of 234U is 0.01%, the abundance of 235U is 0.71%, and the abundance of 238U is 99.28%, what is the average atomic mass of uranium?