IPC for Freshmen – Spring 2015

Final Exam Test Review

Unit 5: Properties of Matter

1)What is matter?

2)What 2 categories can matter be separated into?

3)What is a mixture?

4)What is a homogeneous mixture?

5)What is a heterogeneous mixture?

6)Describe the following mixtures as either homogenous or heterogeneous:

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a)Orange juice with pulp:

b)Milk:

c)Italian salad dressing:

d)Paper:

e)Fruit salad

f)A bag of skittles:

g)Hershey’s chocolate bar:

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7)What is a substance?

8)What is an element?

9)What is a compound?

10)Describe the following substances as an element or a compound?

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a)Water (H2O):

b)Oxygen gas (O2):

c)Table salt (NaCl):

d)Gold (Au)

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11)What are the 3 main states of matter? Give an example of each.

12)For each of the three states of matter, describe how their particles behave and how their volume changes when placed into another container:

a)Solid:

b)Liquid:

c)Gas:

13)What is plasma?

14)Where can plasma be found naturally on earth?

15)Where is plasma located in the universe?

16)What happens to the states of matter as you add heat or remove heat?

Use the following diagram to answerquestions 17-21:

The diagram below is a plot of temperature vs. time. It represents the heating of what is initially ice at -10oC at a near constant rate of heat transfer.

17)Does segment 1 represent a solid, liquid or gas?

18)What is occurring during segment 2? What is this phase change called?

19)Does segment 3 represent a solid, liquid or gas?

20)What is occurring during segment 4? What is this phase change called?

21)Does segment 5 represent a solid, liquid or gas?

22)What is mass? What units are used to measure mass?

23)What is volume? What units are used to measure volume?

24)What tool would you use to find the mass of a solid copper cube?

25)Explain how you would find the mass of 20 mL of water.

26)What tool is used to find the volume of a liquid?

27)Explain how you would find the volume of an irregular shaped rock. (What is this method called?)

28)Explain how you would find the volume of a regular shaped object such as a cube of copper.

29)What is density? How do you calculate density?

30)What are the 2 units you can use to write density?

31)What is the density of a gas if 0.196 g occupies a volume of 100 ml?

32)A block of wood 3 cm on each side has a mass of 27 g. What is the density of the block? (Hint, you need to first find the volume of the wood.)

33)An irregularly shaped stone was lowered into a graduated cylinder holding a volume of water equal to 2 ml. The height of the water rose to 7 ml. If the mass of the stone was 25 g, what is its density?

34)Silver has a density of 10.5 grams/cm3 and gold has a density of 19.3 g/cm3. Which would have the greater mass, 5cm3 of silver or 5cm3 of gold?

35)What is the mass of a 50.0 ml of water if the density of water is 1.00 g/ml?

Using the chart below answer questions 36-38

Substance Density(g/cm3)

Gold 19.3
Mercury 13.5
Lead 11.4
Iron 7.87
Aluminum 3.7
Bone 1.7-2.0
Gasoline 0.66-0.69
Air (dry) 0.00119

36)A substance has a mass of 4725g and a volume of 350 cm3. Using the density, identify the substance.

37)A substance has a mass of 171g and a volume of 15 cm3. Using the density, identify the substance.

38)If I cut the substancefrom #37 in half, what is the density now?

39)Which substances will sink when placed in water?

40)What is a fluid? Give 2 examples.

41)Does the mass of a substance increase, decrease, or stay the same as you melt it from a solid to a liquid.

42)Does the volume of a substance increase or decrease as you melt it from a solid to a liquid. Why?

43)Does the density of a substanceincrease or decrease as you melt it from a solid to a liquid. Why?

44)Complete the following sentences:

i)As the volume increases, the density ______.

ii)As the volume decreases, the density ______.

45)Explain how water is different from other substances as it goes from a liquid to a solidin terms of density. Why is this concept important to life as we know it?

46)What property gives you the ability to carry your friends in the swimming pool easier than when you are on land?

47)What is buoyancy?

48)What is Archimedes’ principle?

49)A 3.5 N object is placed in a tank of water. If the water exerts a force of 2.0 N on the object, will the object sink or float?

50)A 3.5 N object is placed in a tank of honey. If the honey exerts a force of 4.0 N on the object, will the object sink or float?

51)Corn syrup has a larger buoyant force than water does. Explain why this is true. (Talk about the molecules and density of each)

52)A cube of silver weighs 1.69 N when suspended in the air from a spring scale. When suspended in molasses, it has a weight of 1.53 N. What is the buoyant force acting on the cube?

53)What is viscosity?

54)Does viscosity increase or decrease when the temperature is increased? Why?

55)Label the following substances as low or high viscosity:

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a)Water:

b)Motor oil:

c)Syrup:

d)Rubbing alcohol:

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Final Exam Test Review

56)Liquid A has a flow rate of 2.0 cm/s. Liquid B has a flow rate of 5.0 cm/s. Liquid C has a flow rate of 1.0 cm/s (all at room temperature) Flow rate is the volume of liquid that flows in one second.

a)Which of these is the least viscous (has the lowest viscosity)?

b)If you were to heat these liquids to 50 degrees, would you expect the flow rate of each to change? If so, how would it change?

57)Asphalt is the black, sticky material that binds gravel in the pavement that covers streets and highways. Why are most streets pavedduring the summer months?

Unit 6: Atomic structure, ions, isotopes, and the periodic table

1)What is an atom?

2)What are the 3 subatomic particles found in an atom? Describe their location and their charge.

3)What are the energy levels of an atom? How do electrons fill these orbitals?

4)What does the atomic number of an element represent?

5)How can you determine the number of electrons in a neutral atom?

6)What is the mass number of an atom? How do you calculate the mass of an atom?

7)Complete the following chart:

Element name / Element symbol / Atomic number / Atomic mass / Number of protons / Number of neutrons / Number of electrons
Lithium
Silver
Uranium
Oxygen
Sodium
Copper

8)What is an ion?

9)Why do atoms form ions?

10)Complete the following chart:

11)How can you use the periodic table to help determine the charge of a particular element’s ion?

12)What is an isotope?

13)What is the difference between the atomic mass and the mass number of an atom?

14)Complete the following chart:

15)Draw the Lewis dot diagrams for the following atoms:

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a)Calcium

b)Carbon

c)Potassium

d)Helium

e)Argon

f)Oxygen

g)Aluminum

h)Phosphorus

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16)On the periodic table of elements, what are columns called? Why do elements in the same column have similar properties?

17)On the periodic table of elements, what are rows called? What do elements in the same row have in common?

18)What are three properties of metals?

19)What are three properties of non-metals?

20)Where are metals located on a periodic table? Where are non-metals located?

21)Which family of elements is called the alkali earth metals?

22)Which family of elements is known as the halogens?

23)Which family of elements is known as the noble gases?

24)Why are the noble gases inert (don’t react)?

25)Where are the transition metals located on the periodic table of elements?

26)What is the term given to the elements touching the zig-zag lane separating metals from non-metals? Why are they called this (think about their properties)?

Unit 7: Compounds, Chemical Bonding, Counting atoms, Biomolecules, Food labels, Reactions:

  1. What is a chemical change? Give two examples.
  1. What is a compound? How is a compound formed?
  1. What type of energy is stored in a chemical bond?
  1. Why do atoms form bonds? (hint: they want to be happy)
  2. What is an ionic bond?
  3. Between what elements will an ionic bond typically form? Metals and nonmetals? Two metals? Two nonmetals?
  4. For the following elements, show their charges and write their chemical formulas:
  5. Sodium and oxygen: Na: O: Formula: .
  6. Magnesium and sulfur: Mg: S: Formula: .
  7. Lithium and chlorine: Li: Cl: Formula: .
  8. Beryllium and fluorine: Be: F: Formula: .
  9. Calcium and oxygen: Ca: O: Formula: .
  10. What is a covalent bond?
  1. What type of bond is formed between the following elements?
  2. Calcium and sulfur?
  3. Nitrogen and oxygen?
  4. Sodium and fluorine?
  5. Carbon and phosphorus?
  6. Hydrogen and chlorine?
  7. Which electrons are used to determine the valence of an atom? How do you determine the valence of an atom?
  1. How many valence electrons do the following atoms have and what is their valence?
  2. Helium: valence electrons = valence = .
  3. Carbon: valence electrons = valence = .
  4. Oxygen: valence electrons = valence = .
  5. Hydrogen: valence electrons = valence = .
  6. Phosphorus: valence electrons = valence = .
  7. Fluorine: valence electrons = valence = .
  8. How many electrons are shared in a single covalent bond?
  9. How many electrons are shared in a double covalent bond?
  10. How many electrons are shared in a triple covalent bond?
  11. Draw the electron-dot diagram/formula to show the covalent bonds between the following elements:
  12. N2
  1. CO2
  1. Cl2
  1. H2O
  1. For the following formulas, list the elements and number of atoms of each and the total number of atoms in the compound:
  2. Be(OH)2
  1. Li2NO3
  1. 3Na(SO4)2
  1. What is a chemical reaction?
  1. What are the four main types of chemical reactions?
  1. For the following chemical reactions, label the type of chemical reaction:
  2. NaCl(aq) + AgNO3(aq)  NaNO3(aq) + AgCl(s):
  3. 2 H2O  2 H2+ O2:
  4. Zn + 2 HCl  ZnCl2+ H2:
  5. 8 Fe + S8 8 FeS:
  1. What is a polymer? What is a monomer?
  1. What are the four major groups of biomolecules?
  1. What are the monomers for each group?
  1. Draw the basic structure for each group.
  1. Give two examples and two functions of each group.

Look at the food labels and answer the following questions:

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IPC for Freshmen – Spring 2015

Final Exam Test Review

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IPC for Freshmen – Spring 2015

Final Exam Test Review

  1. What is the serving size?
  2. How many servings are in the package?
  3. How many calories per serving?
  4. How much fat is there?
  5. How much sugar is there?
  6. How much starch is there?
  7. How much protein is there?
  8. If a person was to eat the entire container, what percentage of their fat daily value would they consume?

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  1. How many calories per serving?
  2. How much starch is there per serving?
  3. Would this be considered high, medium or low in fat?
  4. Would this be considered high, medium or low in protein?
  5. Would this product be good for an athlete? Why or why not?
  1. Would this product be bad for a person trying to lose weight? Why or why not?
  1. Would this product be bad for a diabetic? Why or why not

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