EOG PREP Topic:

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EOG PREP

Topic: Chemistry

Questions/Main Idea:

Name: _______________________________________

Period:_______________________________________

Date: _______________________________________

Notes:

Atomic Structure

Matter: Anything that has _____ and takes up _. Matter is made of particles too small to see called ____.

Atom: Make up all matter and are composed of , , and __.

Proton: A _______________ (+) charged particle found in an atom’s nucleus.

Neutron: An ________________ particle in an atom’s nucleus.

Electrons: ________________ charged (-) particles that move around outside the nucleus.

Diagram Li and label the proton, electron and neutron. Use the

Bohr Model.

Atomic number:

What is Arsenic’s atomic number?

The number of ____________ in an atoms nucleus.

Which subatomic particle determines an atom’s identity?(D

12)

How do atoms behave in a liquid, solid and gas? Label (liquid, solid, or gas) and describe the

behavior of molecules in the diagrams to the right.

Pure substance: A sample of matter that has a distinct set of intensive properties that are ____________

in all other samples of that substance.

Element: A substance that _____________ be broken down into simpler substances by ordinary chemical means.

Compound: When two or more elements combine _____ to form a _

substance.

Mixture: A substance made of two or more substances that are ____ in the same place, but not _ combined. In a mixture, each substance its identity and __ be separated out by physical means (sifting, distillation, magnetism, etc.).

Label the items as a either an element, compound or mixture.

Then circle the items that are PURE SUBSTANCES

__ gold _ salt oxygen water _ milk __ soil The Periodic Table

Periodic table: A resource that _____ elements based on and

_ properties. When this occurs, a pattern of properties

appears allowing us to ___________ the properties of neighboring elements.

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Is Calcium more similar to Potassium or Bromine? Why?

Group:

What properties does Group 1(Alkali Metals) have in

common?

Elements in a _ column. They show _ in their chemical &

physical properties.

Period:

Describe 2 patterns that change in a predictable way from left to

right. (D 22-23)

Each _________ row the periodic table. of elements _ in a ________ way moving left to right.

Reactivity:

Which group is the most reactive? Least reactive?

(D 26 – 27)

Describes how likely an element is to form bonds with other elements. Those elements with one valence electron or 7 valence electrons are the ___reactive. Those elements, which have a outer shell of valence electron, are or nonreactive.

Ions:

Calcium is located in Group 2 and Bromine is located in group 17. What type of ion is formed by

each element? Include the charge and number (D 14 & 15)

An ion forms when an atom _ or _ an electron.

Calcium (Ca): _______ How many atoms can Calcium bond with to become stable?

______

Bromine (Br): _______ How many atoms can Bromine bond with to become stable?

______

Metals:

In what region of the periodic table are most metals found? (D

27)

Elements that are good _____ of heat & electricity, shiny, _, malleable, and mostly solids.

Nonmetals:

In what region of the periodic table are most nonmetals found?

(D 29)

Elements whose properties tend to be _______________ of those of metals.

Metalloids:

Name one metalloid.

Explain where metalloids are located on the periodic table. (D

30)

Elements that have properties of both _ and ___.

Measuring Physical and Chemical Changes

Physical change:

Identify a physical change:

Alters the physical properties of a substance changing the _ of the substance.

Chemical change:

Name 4 signs of a chemical change:

Occurs when a substance is ______ into a _ substance with

______________ properties. The change occurs when atoms break bonds, rearrange themselves and create new bonds.

1.

2.

3.

4. Precipitate: A _________ that forms from a chemical reaction of two liquids.

Identify the items as either a

physical or chemical change: ___ burning paper _ freezing or boiling water _ melting sugar ___ rusting iron

_ blowing bubbles _ vinegar & baking soda

Chemical equation: Represent how are _______ in a chemical reaction. In a chemical

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reaction, the TOTAL MASS of the reactants ___________ the TOTAL MASS of the products.

Reactant:

Underline the reactant in the chemical equation to the right:

A substance that takes part in a chemical reaction. It is present _________ the reaction occurs.

4Fe + 3 0

2 →

2FeO

3

Product:

Underline the product in the equation to the right:

A substance formed __________ a chemical reaction.

4Fe + 3 0

2 →

2FeO

3

Law of Conservation of Matter: States that during a chemical reaction, matter cannot be _ or __.

Balanced equation: Shows that no matter how atoms are rearranged during a chemical reaction, the same number of _ must be present and _ the reaction.

Coefficient:

Underline the coefficients in the equation to the right:

Indicates how many MOLECULES take part in a chemical reaction. Found in front of chemical symbol.

4Fe + 3 0

2 →

2FeO

3

Subscript:

Underline the subscripts in the equation to the right:

Indicates the number of ATOMS in a molecule found at the base of a chemical symbol.

4Fe + 3 0

2 →

2FeO

3

EOG Questions

1. Which shows one example of a physical change and one example of a chemical change?

a. boiling water & melting wax c. rusting iron & burning coal (fossil fuel) b. dissolving powder & shredding paper d. freezing water & cooking an egg

2. If the reactants contain 12 carbon atoms with a mass of 144 amu and 4 oxygen atoms with a mass of 64 amu, what must be true of the products?

a. The products must contain a total of 16 atoms.

b. The products must contain 4 carbon atoms and 12 oxygen atoms.

c. The product must consist of carbon to oxygen atoms in a 1:1 ratio.

d. The products must contain 12 carbon atoms and 4 oxygen atoms with a total mass of 208 amu.

4. How does a balanced chemical equation satisfy the Law of Conservation of Mass?

a. During a chemical reaction, the total amount of matter stays the same.

b. During a chemical reaction, matter is destroyed.

c. During a chemical reaction, one or more new substances are formed.

d. During a chemical reaction, the total number of atoms increases 5. Which is the best example of a pure substance?

a. peanuts b. milk c. gold d. air

6. Which statement best explains how elements on the periodic table are organized?

a. increasing atomic number from left to right b. increasing number of neutrons from left to right c. decreasing number of electrons from left to right d. decreasing atomic mass number from left to right

7. An ice cube is put into a heated pan. What will most likely happen to the molecules in the ice as the ice is heated?

a. The molecules will begin to move slower. b. The molecules will begin to move faster.

c. The molecules will begin to increase in density. d. The molecules will begin to condense in the air.

8. Which best explains why the total mass of the product(s) would be less than the total weight of the reactant(s) after a chemical reaction?

a. A physical change occurred. b. Atoms involved in the reaction lost mass.

c. Precipitates were created in the new solution. d. Gases were released to the atmosphere.

9. What happens to water molecules during the boiling process?

a. They move faster and move farther apart as they absorb heat.

b. They move faster and remain close together as they absorb heat.

c. They move more slowly but move farther apart as they lose heat.

d. They move faster and move farther apart as they lose heat.

10. Which pair of elements has the most similar properties?

a. Li and B b. I and Ca c. K and He d. N and P

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11. The table shows properties of several elements:

Properties of Elements at Room Temperature Element

Symbol Conducts Electricity State Reactivity

Ca yes solid Reacts with water; combines with Cl to form CaCl

2

K yes solid Reacts with water; combines with Cl to form KCl

Cu yes solid Does not react with water; combines with Cl to form CuCl or CuCl

2

Cl no gas Reacts with all metals and some nonmetals Ar no gas Does not react with metals or nonmetals

B some solid Does not react with water; combines with Cl to form BCl

³

Element X yes solid Reacts with water; combines with Cl to form XCl

Which element would element X most likely be grouped with on the periodic table?

a. calcium b. chlorine c. copper d. potassium

12. Which statement best describes the chemical properties of the elements across period 5.

a. Non-reactive metals to high reactive non-metals.

b. Highly reactive metals to low reactive metals to highly reactive non-metals to non-reactive non-metals.

c. Reactivity remains constant across period 5.

d. Low reactivity across the metals to highly reactive non-metals.

14. Chlorine has 7 valence electrons, which group would chlorine be located in?

a. group 1 b. group 17 c. group 2 d. group 18

15. Which group of elements are malleable and good conductors (heat & electricity)?

a. Group 1 b. group 3-12 (transition metals) c. group 17 d. group 18

16. What is TRUE about all elements?

a. they are made up of one type of atom & are the building blocks of all matter b. they are made of two or more atoms chemically bonded, but only make up solids c. they are all highly reactive and are only found at high temperatures

d. they are exist for fractions of a second

17. Which equation shows the Law of Conservation of Mass?

a. H

²

+ O

²

 2 H

²

O b. CH

⁴

+ 2O

²

 CO

²

+ H

²

O c. N

2

+ H

2

 NH

3

d. 2NaN

3 

Na + 3N

2

18. Which statement best describes a mixture?

a. Substances can be physically separated because they are not chemically combined.

b. Composed of two or more atoms chemically bonded and exist in a set ratio.

c. Made of only one type of atom.

d. Can be represented with a chemical formula (NH

3

)

EOG Questions KEY

3. Which shows one example of a physical change and one example of a chemical change?

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a. boiling water & melting wax c. rusting iron & burning coal (fossil fuel) b. dissolving powder & shredding paper d. freezing water & cooking an egg 4. If the reactants contain 12 carbon atoms with a mass of 144 amu and 4 oxygen atoms with a mass of 64 amu, what must be

true of the products?

a. The products must contain a total of 16 atoms.

b. The products must contain 4 carbon atoms and 12 oxygen atoms.

c. The product must consist of carbon to oxygen atoms in a 1:1 ratio.

d. The products must contain 12 carbon atoms and 4 oxygen atoms with a total mass of 208 amu.

4. How does a balanced chemical equation satisfy the Law of Conservation of Mass?

a. During a chemical reaction, the total amount of matter stays the same.

b. During a chemical reaction, matter is destroyed.

c. During a chemical reaction, one or more new substances are formed.

d. During a chemical reaction, the total number of atoms increases 5. Which is the best example of a pure substance?

a. peanuts b. milk c. gold d. air

6. Which statement best explains how elements on the periodic table are organized?

a. increasing atomic number from left to right b. increasing number of neutrons from left to right c. decreasing number of electrons from left to right d. decreasing atomic mass number from left to right 7. An ice cube is put into a heated pan. What will most likely happen to the molecules in the ice as the ice is heated?

a. The molecules will begin to move slower. b. The molecules will begin to move faster.

c. The molecules will begin to increase in density. d. The molecules will begin to condense in the air.

8. Which best explains why the total mass of the product(s) would be less than the total weight of the reactant(s) after a chemical reaction?

a. A physical change occurred. b. Atoms involved in the reaction lost mass.

c. Precipitates were created in the new solution. d. Gases were released to the atmosphere.

9. What happens to water molecules during the boiling process?

a. They move faster and move farther apart as they absorb heat.

b. They move faster and remain close together as they absorb heat.

c. They move more slowly but move farther apart as they lose heat.

d. They move faster and move farther apart as they lose heat.

10. Which pair of elements has the most similar properties?

a. Li and B b. I and Ca c. K and He d. N and P

11. The table shows properties of several elements:

Properties of Elements at Room Temperature Element

Symbol Conducts Electricity State Reactivity

Ca yes solid Reacts with water; combines with Cl to form CaCl

2

K yes solid Reacts with water; combines with Cl to form KCl

Cu yes solid Does not react with water; combines with Cl to form CuCl or CuCl

2

Cl no gas Reacts with all metals and some nonmetals Ar no gas Does not react with metals or nonmetals

B some solid Does not react with water; combines with Cl to form BCl

3

Element X yes solid Reacts with water; combines with Cl to form XCl

Which element would element X most likely be grouped with on the periodic table?

a. calcium b. chlorine c. copper d. potassium

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12. Which statement best describes the chemical properties of the elements across period 5.

a. Non-reactive metals to high reactive non-metals.

b. Highly reactive metals to low reactive metals to highly reactive non-metals to non-reactive non-metals.

c. Reactivity remains constant across period 5.

d. Low reactivity across the metals to highly reactive non-metals.

14. Chlorine has 7 valence electrons, which group would chlorine be located in?

a. group 1 b. group 17 c. group 2 d. group 18

15. Which group of elements are malleable and good conductors (heat & electricity)?

a. Group 1 b. group 3-12 (transition metals) c. group 17 d. group 18

16. What is TRUE about all elements?

a. they are made up of one type of atom & are the building blocks of all matter b. they are made of two or more atoms chemically bonded, but only make up solids c. they are all highly reactive and are only found at high temperatures

d. they are exist for fractions of a second

17. Which equation shows the Law of Conservation of Mass?

a. 2 H

2

+ O

2

 2 H

2

O b. CH

4

+ 2O

2

 CO

2

+ H

2

O c. N

2

+ H

2

 NH

3

d. 2NaN

3 

Na + 3N

2

18. Which statement best describes a mixture?

a. Substances can be physically separated because they are not chemically combined.

EOG PREP Topic:

EOG PREP

Topic: Chemistry

Questions/Main Idea:

Name: _______________________________________

Period:_______________________________________

Date: _______________________________________

Notes:

Atomic Structure

Matter: Anything that has _________ and takes up _________. Matter is made of particles too small to see called ________.

Atom: Make up all matter and are composed of ____________, ____________, and ______________.

Proton: A _______________ (+) charged particle found in an atom’s nucleus.

Neutron: An ________________ particle in an atom’s nucleus.

Electrons: ________________ charged (-) particles that move around outside the nucleus.

Diagram Li and label the proton, electron and neutron. Use the

Bohr Model.

Atomic number:

What is Arsenic’s atomic number?

The number of ____________ in an atoms nucleus.

Which subatomic particle determines an atom’s identity?(D

12)

How do atoms behave in a liquid, solid and gas? Label (liquid, solid, or gas) and describe the

behavior of molecules in the diagrams to the right.

Pure substance: A sample of matter that has a distinct set of intensive properties that are ____________

in all other samples of that substance.

Element: A substance that _____________ be broken down into simpler substances by ordinary chemical means.

Compound: When two or more elements combine _______________ to form a ___________

substance.

Mixture: A substance made of two or more substances that are ____________ in the same place, but not _______________ combined. In a mixture, each substance ____________ its identity and ________ be separated out by physical means (sifting, distillation, magnetism, etc.).

Label the items as a either an element, compound or mixture.

Then circle the items that are PURE SUBSTANCES

______ gold _______ salt ______ oxygen ______ water _______ milk ______ soil The Periodic Table

Periodic table: A resource that _________________ elements based on ____________ and

_______________ properties. When this occurs, a ______________ pattern of properties

appears allowing us to ___________ the properties of neighboring elements.

Is Calcium more similar to Potassium or Bromine? Why?

Group:

What properties does Group 1(Alkali Metals) have in

common?

Elements in a _____________ column. They show _____________ in their chemical &

physical properties.

Period:

Describe 2 patterns that change in a predictable way from left to

right. (D 22-23)

Each _________________ row the periodic table. ______________ of elements _______________ in a ________________ way moving left to right.

Reactivity:

Which group is the most reactive? Least reactive?

(D 26 – 27)

Describes how likely an element is to form bonds with other elements. Those elements with one valence electron or 7 valence electrons are the ___________reactive. Those elements, which have a ______ outer shell of ______valence electron, are ________ or nonreactive.

Ions:

Calcium is located in Group 2 and Bromine is located in group 17. What type of ion is formed by

each element? Include the charge and number (D 14 & 15)

An ion forms when an atom _________ or _________ an electron.

Calcium (Ca): _______ How many atoms can Calcium bond with to become stable?

______

Bromine (Br): _______ How many atoms can Bromine bond with to become stable?

______

Metals:

In what region of the periodic table are most metals found? (D

27)

Elements that are good _______________ of heat & electricity, shiny, ___________, malleable, and mostly solids.

Nonmetals:

In what region of the periodic table are most nonmetals found?

(D 29)

Elements whose properties tend to be _______________ of those of metals.

Metalloids:

Name one metalloid.

Explain where metalloids are located on the periodic table. (D

30)

Elements that have properties of both ___________ and _____________.

Measuring Physical and Chemical Changes

Physical change:

Identify a physical change:

Alters the physical properties of a substance ____________ changing the _____________ of the substance.

Chemical change:

Name 4 signs of a chemical change:

Occurs when a substance is ____________ into a _______ substance with

______________ properties. The change occurs when atoms break bonds, rearrange themselves and create new bonds.

1.

2.

Matter: Anything that has _____ and takes up _. Matter is made of particles too small to see called ____.

Atom: Make up all matter and are composed of , , and __.

Compound: When two or more elements combine _____ to form a _

Mixture: A substance made of two or more substances that are ____ in the same place, but not _ combined. In a mixture, each substance its identity and __ be separated out by physical means (sifting, distillation, magnetism, etc.).

__ gold _ salt oxygen water _ milk __ soil The Periodic Table

Periodic table: A resource that _____ elements based on and

_ properties. When this occurs, a pattern of properties

Elements in a _ column. They show _ in their chemical &

Each _________ row the periodic table. of elements _ in a ________ way moving left to right.

Describes how likely an element is to form bonds with other elements. Those elements with one valence electron or 7 valence electrons are the ___reactive. Those elements, which have a outer shell of valence electron, are or nonreactive.

An ion forms when an atom _ or _ an electron.

Elements that are good _____ of heat & electricity, shiny, _, malleable, and mostly solids.

Elements that have properties of both _ and ___.

Alters the physical properties of a substance changing the _ of the substance.

Occurs when a substance is ______ into a _ substance with

physical or chemical change: ___ burning paper _ freezing or boiling water _ melting sugar ___ rusting iron

_ blowing bubbles _ vinegar & baking soda

Chemical equation: Represent how are _______ in a chemical reaction. In a chemical

Law of Conservation of Matter: States that during a chemical reaction, matter cannot be _ or __.

Balanced equation: Shows that no matter how atoms are rearranged during a chemical reaction, the same number of _ must be present and _ the reaction.