Solid Gas Liquid Plasma

Chemistry: Progress Assessment 2 Review Sheet CHAPTER 1: MATTER Study of matter and the changes it undergoes 1. Define CHEMISTRY: ___________________...
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Chemistry: Progress Assessment 2 Review Sheet CHAPTER 1: MATTER Study of matter and the changes it undergoes

1. Define CHEMISTRY: __________________________________

2. Define MATTER:

has mass and volume

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

2|Page

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.

3|Page

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)

4|Page

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

5|Page

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 ____________

7|Page

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:

Element

Chlorine

nitrogen Potassium

aluminum Barium

titanium

Electron configuration

1s 2

2 2

2

2s

3

No. of valence electrons

6 2 5 2p 3s 3p

1s 2s 2p

1s 2 2s 2 2p 2

2

6

2

6 3s 2 3p 6 4s 1 1

7 5 1 3

1s 2s 2p 3s 3p

2 2 6 2 6 2 10 6 2 10 1s 2s 2p 3s 3p 4s 3d 4p 5s 4d 6s2 2

2

6

2

6

2

2

1 s 2s 2p 3s 3p 4s 3d

2

2 (just count the outer) which is the 2 from 2 4s

10 | P a g e

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 ___________.

11 | P a g e

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 _____________________.

12 | P a g e

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

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