Unit 2

Name: _________________________________ Date: _______ Period: _____

Atoms, Compounds, and the Periodic Table of Elements

Chapter 3: Section 3.1 Properties of Matter 1. Label each drawing with one of these words: solid, liquid, gas.

____gas____

____solid____

___liquid____

2. What is the difference between a gas and a vapor? A gas is gaseous at room temperature, and a vapor is a gaseous state of a substance that is a liquid or solid at room temperature. 3. What is the definition of an amorphous solid? A solid in which particles are not arranged in a regular, repeating pattern that often is formed when molten material cools too quickly to form crystals. 4. What examples of amorphous solids were discussed in class? Glass, LDPE (garbage bags) 5. What two other states of matter were discussed in class? Plasma, and Super Solids (Bose Einstein Condensate)

Section 12.4 Phase Changes In your textbook, read about phase changes. Complete the table by writing the initial and final phases for each phase change and making a check (ü) in the correct energy column.

Phase change Phase Energy Change

initial final Endothermic Exothermic

1. Melting Solid Liquid ü

2. Freezing liquid solid ü

3. Condensation Gas liquid ü

4. Deposition gas solid ü

5. Sublimation Solid gas ü

6. Vaporization Liquid gas ü

Chemistry: Matter and Change Study Guide Copyright © Glencoe/McGraw-Hill, a division of The McGraw-Hill Companies, Inc.

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3 Unit 2 7. For water, what are the following temperatures (in Celcius)?

Freezing point: _0°C_ Melting point: _0°C _ Boiling point: _100°C_ (in Kelvin: 373K)

8. What is the difference in the energy flow of freezing and melting? Melting: energy is absorbed (endothermic), and in freezing energy is released (exothermic).

Section 3.2 Changes in Matter In your textbook, read about physical properties and chemical properties of matter.

Use each of the terms below just once to complete the passage.

chemical density

mass properties

physical substance

Matter is anything with (1) _______ mass _________and volume. A (2) __ substance _____ is a form

of matter with a uniform and unchanging composition. Substances have specific, unchanging (3)

____ properties ____ that can be observed. Substances have both physical and chemical properties.

(4) ______ physical_______ properties can be observed without changing a substance’s chemical

composition. Color, hardness, and (5) _____ density _______ are examples. Other properties

cannot be observed without changing the composition of a substance. These are called (6) _____

chemical____ properties. An example is the tendency of iron to form rust when exposed to air.

In your textbook, read about physical change and chemical change Label each property as either physical or chemical.

_____ physical ____ 7. Chemical formula H2O

_____ chemical ______8. Forms green carbonate when exposed to moist air

____ chemical _____ 9. Remains unchanged when in the presence of nitrogen

____ physical ______10. Colorless

_____ physical ______11. Solid at normal temperatures and pressures

_____ chemical ______12. Ability to combine with another substance

_____ physical ____ 13. Melting point

_____ physical ____ 14. Liquid at normal temperatures and pressures

_____ physical _____15. Boiling point is 100°C

Unit 2

_____ physical ______16. Conducts electricity

_____ physical _____17. Density is !"##$%&'!(

18. What kinds of changes do these words indicate? Write each word under the correct heading. Use each word only once.

boil crumple crush explode burn precipitate formed freeze grind

condense melt oxidize rot corrode rust change in pH vaporize

Physical Change Chemical Change

Boil crush

Condense grind Crumple vaporize

melt freeze

Burn change in pH

Corrode explode precipitate formed rot

rust oxidize

19. What is the pH of pure water?

a) 0 b) 1 c) 7 d) 14

20. Which is the most likely pH for a solution of a weak acid?

a) 1 b) 5 c) 11 d) 14 21. Which pH value indicates the most basic solution?

a) 3 b) 7 c) 8 d) 11

22. List FOUR observations / signs of a chemical change: Any four of the following: bubbles = gas precipitate forms energy released (light) change in odor

change in temperature change in acidity permanent color change

Chemistry: Matter and Change Study Guide Copyright © Glencoe/McGraw-Hill, a division of The McGraw-Hill Companies, Inc.

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3 Unit 2 History of the Universe (State Textbook, Chapter 1)

1. What are the two most abundant elements in the universe? What processes helped form the elements?

Hydrogen (most); helium (2nd). Formed during the Big Bang through fusion.

2. Earth and the other inner planets contain large amounts of elements heavier than carbon. Where did these elements come from?

From the fusion of atoms following a Super Nova (explosion of a star).

Chapter 4: Section 4.2 Defining the Atom 1. In J.J. Thomson’s experiment, the cathode rays are __________.

A) neutrons B) x-rays C) electrons D) protons 2. Cathode rays are deflected away from a negatively charged plate because __________.

A) they are not particles B) they are positively charged particles C) they are neutral particles D) they are negatively charged particles

3. The gold foil experiment performed in Rutherford's lab __________.

A) confirmed the plum-pudding model of the atom B) led to the discovery of the atomic nucleus C) was the basis for Thomson's model of the atom D) utilized the deflection of beta particles by gold foil

4. Compare and Contrast Thomson and Rutherford’s Atomic Models.

Thomson Both Rutherford

• Usedcathoderays,

electricity,andmagnetstodiscoverELECTRONS

• Nonucleus• Atomisnotsolid–a

positiveforcewithembeddedelectrons.

Atom is divisible – subatomic particles do exist: Electrons!

• Shotalphaparticlesatgoldfoil• Atomhasanucleus• Nucleushasapositivecharge:

PROTONS• Nucleusisdense–hasmass• Mostofatomisemptyspace.• Electronsmovearound

nucleus

Unit 2

Section 4.3 How Atoms Differ Complete the following table of proton, electron, and neutron characteristics.

Particle Symbol Location Relative Charge Relative Mass (amu)

Proton p+ Nucleus Positive 1

neutron no Nucleus Neutral 1

electron e- Outside nucleus Negative 1/1840

In your textbook, read about atomic number. For each statement below, write true or false.

___false (protons)___ 1.The number of neutrons in an atom is referred to as its atomic number.

___true_____ _ 2.The periodic table is arranged by increasing atomic number.

___ false (protons)___3. Atomic number is equal to the number of neutrons in an atom.

____true__________ 4.The number of protons in an atom identifies it as an atom of a particular element.

_false (protons to neutrons)__ 5. Nuclear stability is determined by the ratio of protons to electrons.

Section 6.1 Modern Periodic Table

The Periodic Table Match the definition in Column A with the term in Column B.

Column A Column B

_____f_____ 1. Atom or bonded group of atoms that has a positive or negative charge

______a____ 2. Group 1 elements (except for hydrogen)

______b____ 3. Group 2 elements

______c____ 4. A column in the periodic table

______e____ 5. A row in the periodic table

______d____ 6. Group 17 elements

______g____ 7. Group 18 elements

a. alkali metals

b. alkaline earth metals

c. group

d. halogens

e. period

f. ion

g. noble gases

Chemistry: Matter and Change Study Guide Copyright © Glencoe/McGraw-Hill, a division of The McGraw-Hill Companies, Inc.

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3 Unit 2 Elements of the Periodic Table Use the information in the box on the left taken from the periodic table to complete the table on the right.

Atomic Mass 14.007

Atomic Number 7

Chemical Name Nitrogen

Chemical Symbol N

Answer the following questions (assume all atoms are neutral): 1. Lead has an atomic number of 82. How many protons and electrons does lead have? ___82___

2. Oxygen has 8 electrons. How many protons does oxygen have? ___8________

3. Zinc has 30 protons. What is its atomic number? ________30________

4. Astatine has 85 protons. What is its atomic number? ________85________

5. Rutherfordium has an atomic number of 104. How many protons and electrons does it have?_104__

6. Name the element located in group 7, period 4.___manganese____

7. Nobelium has an atomic number of 102. How many protons and electrons does it have? _102__

Use the periodic table to identify each element described below. 8. atomic number 92 __Uranium____

9. 78 protons ______Platinum_____ 10. 47 protons and 47 electrons _____Silver_____________

11. atomic number 24 ____Chromium_______ 12. 20 protons _________Calcium_________

13. Element in a _________ have similar chemical properties.

a. period b. group / family c. both A and B d. neither A nor B

Unit 2

14. Which of the following elements would you expect to be most similar to carbon? a. nitrogen b. boron c. silicon d. potassium

15. Which of the following elements is in the same group / family as fluorine?

a. silicon b. antimony c. iodine d. arsenic

16. Give the name of the family in which each of the following elements is located:

a. iodine: ___halogen ______

b. krypton: ____noble gas_____

c. barium: ____alkaline earth metal_______

d. francium: ___alkali metal_____

17. On the periodic table above, indicate the element locations and symbols of the two elements occurring naturally as liquids at room temperature (298K).

In the space at the left, write true if the statement is true; if the statement is false, change the italicized word or phrase to make it true.

_____false_______ 18. There are two main classifications of elements. __three (metal, nonmetal, metalloid)____

Br Hg

Chemistry: Matter and Change Study Guide Copyright © Glencoe/McGraw-Hill, a division of The McGraw-Hill Companies, Inc.

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3 Unit 2 _____false_________ 19. More than three-fourths of the elements in the periodic table are nonmetals.

__metals__

______true_______ 20. Group 1 elements (except for hydrogen) are known as the alkali metals. __(no change)__

_____false________ 21. Group 13 elements are the alkaline earth metals. ___2____

____true__________ 22. Group 17 elements are highly reactive nonmetals known as halogens. __(no change)__

____false_________ 23. Group 18 elements are very unreactive elements known as transition metals. __noble gases__

Properties of Metals & Nonmetals For each property, mark (X) if the property is characteristic of most metals or nonmetals.

Property Metal Nonmetal Property Definition / Description

1. Malleable X Bends easy / can be pounded thin

2. Brittle X Breaks easily/crumbles

3. Lustrous X Shiny

4. High melting point X Harder to melt – needs high temp

5. Low boiling point X Vaporizes at low temperature

6. Ductile X Can be pulled into wires

7. Poor conduction of heat X Heat doesn’t flow easily

8. Good conduction of electricity

X Electricity / electrons flow easily

Section 3.4 Elements and Compounds In your textbook, read about elements and compounds. Circle the letter of the choice that best completes the statement or answers the question. 1. A substance that cannot be separated into simpler substances by physical or chemical means is a(n)

a. compound. b. mixture. c. element. d. period.

2. A chemical combination of two or more different elements is a(n) a. solution. b. compound. c. element. d. period.

3. Which of the following is an example of an element? a. water b. air c. sugar d. oxygen

4. Which of the following is an example of a compound? a. gold b. silver c. aspirin d. copper

Unit 2

Label each substance as either an element or a compound. _____ element _______ 5. silicon

_____ compound_____ 6. sodium chloride _____ element _______ 7. francium

_____ element _________ 8.nickel _____ compound _______9.Ice

______ compound ______10. ammonia

What is the chemical formula for this weak base? __NH3____

Match each term in Column A with its example in Column B.

Column A Column B ___d__11. Alloy (mixture)

__a___12. element

__b___13. gas

___c__14. vapor

a. gold

b. methane

c. steam

d. sterling silver (silver and copper)

Laboratory

Identify the following lab equipment:

Mortar & pestle Test tube & holder Tongs Watch glass