Final Exam Review Questions 2006

Final Exam Review Questions 2009 p. 1

Name___________________________

What is the formula for density? _________

What is the density of water? ___________

What is the formula for the volume of a rectangular shaped object? __________

What is the formula for the volume of a cylinder?_____________

Draw and label the metric steps

0.0506 hg = ________ dg Which is larger 5.61 daL or 205 dL _________

How much larger is a dg compared to a mg? ____________

If an object has a known density of 45g/ml, what will the volume be if a sample of the object has a mass of 25 grams? ______________

How would you find the volume of an odd shaped object?

What is the rule for reading an instrument such as a ruler that has calibration lines?

How do you read the volume of a liquid in a graduated cylinder?

What is the formula for percent error?

If the theoretical density is 5.6 g/ml but your measurement reads 4.9 g/ml, what is the percent error for your work?

Explain the Atlantic-Pacific rule for determining significant figures.

How many significant figures in each number? 5005 0.450 50.50

p. 2

(6.3 x 10-3) x ( .04 x 105) = __________ (round to the correct # of sig fig)

All acids must have _________and __________

Acids have a pH range of ________to _______. A weak acid would have a pH of _____

All bases contain _________and ________

Red litmus is used to test for _________

Name a strong (dangerous) acid ____________Name a weak acid ___________

Name the two acids found in acid rain __________and _____________

What is the formula for stomach acid? _____________ Battery acid? ________

_____________________

Name 5 physical properties of water.

Define chemical properties.

Compare physical change to chemical change.

Give an example of physical change.

Give an example of chemical change.

Define the Law of conservation of matter.

Define homogeneous mixture and give an example.

Define heterogeneous mixture and give an example.

Draw a gravity filter.

Will it separate a homogeneous or heterogeneous mixture.

p. 3

Give an example for a homogeneous mixture and a heterogeneous mixture that can be separated by distillation.

What physical property does distillation depend on?

A mixture of dyes can be separated by using ________________ which takes advantage of the

_____________ and ___________ of each dye.

List the following solution particles in order of size from largest to smallest.

Ion, suspension, colloid.

How could you prove the presence of ions in a solution?

Which particles will not pass through filter paper?

Which particles can be seen when in solution?

Which type of particles are detected with a Tyndall test?

_________________________

Atomic number tells you the number of ____________and ______________for an atom.

If you round off atomic mass, you know have __________ __________ which is the total of _______ and _________

Family # for A groups tells you the number of ______________

The row or period tells you the number of ________ _________that the atom has.

Isotopes of an element have the same # of ___________and __________ but have different number of __________

Ca-40 40 is called the _____ ________ and tells us the number of _________and _______

Draw a Bohr model of Ca 40

p. 4

Metals will form _________ions by ________electrons.

Nonmetals will form _________ions by _________electrons.

The roman numeral after the name of metal tells us ____________

Write the symbol for an alpha particle.____________

Write the symbol for a beta particle. __________

Write the reaction for the alpha decay of U-240

Write the beta decay reaction for Th 235

Define half life.

If an element has a half life of 5 days, how much will be left undecayed after 20 days if you start with 100 grams?

____________________________

Write the electron configuration for an atom of Mg

Write the electron configuration for an atom of Cobalt.

Give examples of each of the following:

Period 2 alkaline _________Solid halogen __________

Liquid transition _________Radioactive alkali _________

Man made with lowest atomic mass________

Period 3 metalloid ________

p. 5

Which is larger: atom of Mg atom of sulfur

atom of Mg ion of Mg

atom of S atom of Cl

Which has larger ionization energy Mg or S

Mg or Ca

Has lowest electronegativity Mg or S

Mg or Ca

Name the following compounds:

FeCl3CaOP2O5

Na OHMg SO4Pb(NO3)2

Write correct formulas for the following:

Copper (II) sulfateCopper (I) oxide

Magnesium carbonateSodium bromide

Write correct formulas and balance the equations: (review material for chapter 9) also identify the type of reaction

Methane (CH4) + oxygen carbon dioxide + water

Sodium carbonate decomposes into sodium oxide and carbon dioxide

Hydrochloric acid + calcium hydroxide calcium chloride + water

Sodium + Fluorine sodium fluoride

Write the dissociation reaction for Potassium phosphate when it dissolves in water.

Calculate the formula weight of calcium phosphate.

p. 6

What is the percent of oxygen in Iron (III) acetate?

4.5 moles of lithium oxide = ________grams

8 x 1023 atoms of argon = __________grams

2.3 Liters of sulfur dioxide = __________grams

47 grams of carbon dioxide = _________molecules

p. 7

Write the electron configuration for an ion of bromine

Write the electron configuration for an atom of iron which has lost 2 electrons

Write the orbital notation model for an atom of chromium

Write the Lewis model for an atom of phosphorus

Write the Lewis model for an ion of nitrogen

Write the Lewis model for an ion of calcium