Chemistry: Progress Assessment 2 Review Sheet CHAPTER 1: MATTER Study of matter and the changes it undergoes
1. Define CHEMISTRY: ___________________...
Use one of the states of matter to complete each statement. (Words will be used more than once.)
Solid
Gas
Liquid
Plasma
solid 3. A _______________ has definite volume and definite shape. plasma 4. ________________ is a state of matter found in outer space. liquid 5. ________________ have definite volume and no definite shape. plasma 6. ________________ has particles smaller than gas. gas 7. ________________ has the most energy of the 3 states of matter found on earth. It has no definite volume, and no definite shape.
Use the word bank below to describe each.
Evaporation
Condensation Melting
Freezing Sublimation
8. When a solid changes to a liquid:
melting ____________________
9. When a liquid changes to a solid:
freezing ____________________
10. When a liquid changes a gas:
evaporation ___________________
11. When a gas changes a liquid:
condensation ____________________
sublimation 12. When a solid changes to a gas: ____________________ sublimation 13. When a gas changes to a solid: ____________________ 1|Page
Chemistry: Progress Assessment 2 Review Sheet
14. Use an arrow to indicate in which direction the following processes occur. (Ex. A B, or B A) C -> D Evaporation = ___________________
B -> A Freezing = _____________________ A -> B Melting = _____________________ D -> C
Condensation = __________________
50 degrees 15. What is the boiling point of the substance above? _______ 0 degrees What is the freeing point? _______
Celsius
Celsius
gas 16. At 75°C, in which state of matter would this substance be? ________ solid At 15 °C ? ___________ At 45 °C ? ___________ liquid and
gas
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Chemistry: Progress Assessment 2 Review Sheet 17. Fill in the Matter Flow Diagram below.
ixture
ubstance
lement C H
ompound H2O NaCl
omogeneous
eterogeneous
salt and water
salad
brass
sand and water
Use the Word Bank below to fill in the blanks. (Not all the words are used)
mixtures compound substances
homogeneous elements compounds
heterogeneous matter element
atoms
mass
solutions
atoms 18. All matter consists of tiny particles called_______________. substances and _______________. mixtures 19. Matter is divided into 2 categories: _______________ elements 20. Substances can be broken down into 2 categories: _______________ and _______________. compounds element 21. An _____________ is made up of only one type of atom. 22. Two or more different atoms combined chemically are called a _______________. compound
mixture 23. A _______________ is made up of 2 or more substances physically combined.
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Chemistry: Progress Assessment 2 Review Sheet homogeneous 24. A mixture that is uniform throughout the sample is said to be _______________. solutions These types of mixtures are known as _______________. 25. A mixture that has uneven distribution of 2 or more substances is called heterogeneous _____________________. 26. Fill in the following table. A. Determine if the following examples are Substances or Mixtures. B. If it’s a substance, indicate if it’s a compound or an element. C. If it’s a mixture, indicate if it’s homogenous or heterogeneous. Type of Matter Substance or Mixture? (Element or Compound) or (Homogeneous or Heterogeneous?) Ex 1: water Substance Compound Ex 2: sand & water Iron Sugar water Carbon dioxide Vegetable soup
Mixture
Heterogenous
substance
element
mixture
homogeneous
substance
compound
mixture
heterogeneous
27. Physical Changes only change the a____________________ of a substance, not it’s ppearance identity! 28. Chemical Changes results in ___________________________. a new substance List the 4 ways to show a chemical reaction takes place:
color/ odor change a)__________________________ bubbles (gas) b) __________________________ precipitate (solid formed c) __________________________
when combining 2 solutions)
energy gained (endothermic d) __________________________
-cold) or energy lost (Exothermic - hot)
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Chemistry: Progress Assessment 2 Review Sheet 29. Fill in the following chart. Physical or Chemical Change? Cutting paper
P C
Burning paper Freezing water
P
Dissolving salt in water
P
Combining an acid & base to form water and salt Rusting metal
C C
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Chemistry: Progress Assessment 2 Review Sheet CHAPTER 2: SI UNITS & MEASUREMENTS 1. Put the following steps of the scientific Method in the proper order:
4 Observe and record data. _____ 3 Test the hypothesis with an experiment. _____ 1 Identify the problem. _____ 2 Make a hypothesis. _____ _____ 5 Arrive at a conclusion. 2. Fill in the following metric prefixes.
giga mega kilo
hecto deca
deci
centi milli micro nano
Use the Factor-Label Method to convert each of the following measurements. Show work and use appropriate labels.
3) 2.56 kilograms to grams
2.56 kg X 1000 g =
2560 g
1 kg 4) 17 millimeters to centimeters
17 mm x 1 cm = 1.7 cm 10 mm
5) 125 pounds to kilograms (2.2 pounds = 1 kilogram)
125 lb x 1 kg = 11.4 kg 2.2 lb 6|Page
Chemistry: Progress Assessment 2 Review Sheet DENSITY Write the formula to determine density, volume, and mass below. Density =
mass
Mass =
volume
density x volumeVolume = mass density
Determine the value of the missing measurement. SHOW YOUR WORK! USE UNITS!
7.5 g/cm3 6. mass = 75 g; volume = 10 cm3; density = _____________
26.7 cm3 7. mass = 400 g; density = 15 g/cm3 ; Volume = ____________
125 g 8. volume = 25 cm3; density = 5 g/cm3 ; Mass = ___________
1.0 g/cm3
9. What is the density of water? ________ sink (Substances with a higher density will __________, and a lower density will ___________.) float
Substance
Density (g/cm3)
Sink or Float?
10. Mercury
13. 55
sink ____________
11. Salt
1.2
sink ____________
12. Soap
0.8
float ____________
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Chemistry: Progress Assessment 2 Review Sheet Chapter 3: Atoms and Isotopes 1. Label the nucleus, neutrons, protons, and electrons.
electrons
nucleus
protons neutrons
2. Fill in the following chart: Element
Chemical Atomic # Symbol Number Protons
Barium
Ba
chromium
Cr
Silver
Ag
56 24 47
# Electrons
# Neutrons
Mass Number
56
56
81
137
24
24
28
52
47
47
61
108
3. Calculate the average atomic mass.
Isotope Nitrogen-14 Nitrogen-15
Relative Abundance
Atomic Mass
99.63%
14.003
0.37%
15.000
(.9963)x(14.003) + (0.0037)x(15.000) =
14.01 amu 8|Page
Chemistry: Progress Assessment 2 Review Sheet Ch 4 Nuclear Chemistry 1. Band of stability. (read a graph, identify elements that are stable and not stable)
Ca Cl
Use the graph above to identify the following elements as stable or not stable: 35 17
50 20
stable
Cl
Ca
18 neutrons
radioactive (Not stable)
30 neutrons
2. Identify alpha and beta particles. Alpha
Beta
He
e
3. Write nuclear equations that show alpha decay:
238 92
U
→
4 2
234 He
+
Th 90
4. Write a nuclear equation that shows beta decay: 207 82
Pb
→
0 -1
e
+
207
Bi
208 9|Page
Chemistry: Progress Assessment 2 Review Sheet Ch 5 Electrons and Energy Levels energy level (shell) 1. Electrons orbit the nucleus in an ________________________. -
2 2. The first energy level holds ________e .
-
8 3. The second energy level holds ________e . 18 4. The third energy level holds ________e . -
5.
Complete the Table below with the correct information:
Chemistry: Progress Assessment 2 Review Sheet Ch 6 Ions and Ionic Compounds 1. Draw a Bohr Model for the element Sulfur
6 a) How many valence electrons? __________ b) Lose or gain electrons to become stable? _________ gain
S
2 c) How many? __________ anion d) Anion or Cation? __________ d) Charge of ion? __________ -2
8 electrons in their valence shell to 2. The Octet Rule states that atoms want ______ become stable. 3. What are the 3 types of chemical bonds? a. M_____________ etallic
onic b. I______________ c. C______________ ovalent
4. What will Nitrogen do to become stable? d. Gain 3 electrons b. Lose 3 electrons
c. Gain 3 protons
5. Atoms that gain or lose electrons and become charged particle are called ions ___________.
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Chemistry: Progress Assessment 2 Review Sheet 6. Atoms that lose electrons have a (positive / negative) charge and are called (cations / anions). (Metals / Nonmetals) tend to lose electrons to become stable. [circle the correct answers of the pairs]
7. Atoms that gain electrons have a (positive / negative) charge and are called (cations / anions). (Metals / Nonmetals) tend to gain electrons to become stable. [circle the correct answers of the pairs]
8. What happened for Ca+2 to have a charge of +2? a) lost 2 electrons b) gained 2 electrons c) gained 2 protons
9. Complete the following table: Element
Sodium Oxygen Chlorine Calcium Phosphorus
Electron Dot Structure
O
Na
Ca
Cl P
Ion
Na+ O -2 Cl +2 Ca -3 P
Gained or lost electrons?
lost gained gained lost gained
How many?
1 2 1 2 3
Cation or Anion?
cation anion anion cation anion
Metal or nonmetal?
metal nonmetal nonmetal metal nonmetal
ransferred 10. Ionic bonds form when electrons are t_________________ from one atom to another. 11. Ionic compounds are often referred to as ____________. a) lattices b) salts c) polar bonds d) oxidation numbers
12. When an ionic compound is placed in water, the ions separate from dissociation each other. This is called _____________________.
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Chemistry: Progress Assessment 2 Review Sheet 13. Word bank: Place the following formulas or chemical names in the appropriate spaces.
NOT ALL COMPOUNDS ARE USED! a.
O3F9
i.
Lead(II) sulfate
b.
CuCl2
j.
Diphosphorus pentoxide
c.
O2F6
k.
Dinitrogen tetroxide
d.
BaCO3
l.
Potassium oxide
e.
CCl4
m.
Aluminum phosphate
f.
MgBr2
n.
Aluminum phosphorus
g.
Mg2Br3
o.
Lead (I) sulfate
h.
BaCO2
c 13. Dioxygen hexafluoride ____ d 14. Barium carbonate ____ e ____15. Carbon tetrachloride b ____16. Copper (II) chloride f ____17. Magnesium bromide i ____18. PbSO4 L ____19. K2O k ____20. N2O4 m ____21. AlPO4 j ____22. P2O5 13 | P a g e