Chapter 4 P/C And Energy, Ch 8 Chemical Equations

Question 1

+ symbol meaning?

Answer 1

Plus or added two
placed between substances

Question 2

Arrow to the right

Answer 2

Yields, produces
Points to products

Question 3

(s)

Answer 3

Solid state
Written after a substance

Question 4

(l)

Answer 4

Liquid state
Written after a substance

Question 5

(g)

Answer 5

Gaseous state
Written after a substance

Question 6

(aq)

Answer 6

Aqueous solution
Substance dissolved in water

Question 7

triangle

Answer 7

Heat is added
When written above or below arrow

Question 8

What’s the difference between physical properties and chemical properties

Answer 8

 Physical properties can be observed/determined WITHOUT CHANGING THE IDENTITY of a substance

Chemical properties FORM NEW SUBSTANCES

Question 9

Examples of physical properties

Answer 9

SOLUABILITY
phase change properties, like boiling, freezing or melting point
CONDUCTIVITY

Odor, color, shiny

Question 10

Examples of chemical properties

Answer 10

Flammable,
Decay
Supporting combustion
Ability to rust

Question 11

No two substances have identical, physical and chemical properties

Question 12

What’s the difference between a change and a property?

Answer 12

Properties describe
Shiny measurable prop

Changes are verbs with ING
DISSOLVING, CONDUCTING
CUTTING

Question 13

Are growing a plant and baking physical or chemical changes?

Answer 13

Chemical changes

Question 14

What are the proper proper terms in writing chemical equations?

Answer 14

Reactants (right YIELDS arrow) products

Question 15

What is the law of conservation of mass?

Answer 15

Mass can’t be created or destroyed in any chemical or physical process

Question 16

What is involved in a physical and chemical processes?

Answer 16

Energy

Question 17

Definition of energy

Answer 17

Ability to do work for capacity to cause change

Question 18

Name forms of energy

Answer 18

Foods and fuels

Radiant, light, mechanical, electrical, nuclear, heat, chemical, sound

Question 19

What is kinetic energy

Answer 19

Energy of motion, such as walking down the hall, or rolling a ball

Question 20

Give an example of potential energy

Answer 20

Foods or a spring

Question 21

What is the law of conservation of energy?

Answer 21

Energy cannot be created or destroyed. It can only transform from one form to another,

such as plugging in a appliance in a toaster means, changing, electrical, energy to heat, light, mechanical and sound energy.

Question 22

Official definition of heat

Answer 22

Energy that moves from one place to another due to a difference in temperature

Question 23

Energy always flows from what to what temperature

Answer 23

High to low temperature

Question 24

Test

Question 25

What is specific heat?

Answer 25

Amount of energy needed to change the temperature of 1 g of a specific substance by 1°C

Question 26

What is temperature?

Answer 26

The measure of kinetic energy of the particles in a sample

Question 27

What is thermal energy?

Answer 27

Total kinetic energy and potential energy of all the particles in a sample. This is not warmth but more particles, a swimming pool has more thermal energy than a beaker even if the beaker is boiling and the swimming pool is room temp.

Question 28

What does a low specific heat mean?

Answer 28

A substance does not need to absorb much energy in order to change its temperature. Metal has a lower specific heat. For example, a metal spoon in a pot is warmer than a wooden spoon in the same pot

Question 29

Q = energy in joules or calories

Question 30

C: specific heat

Question 31

TriangleT =  change in temperature

Question 32

When energy is released during a chemical reaction, the process is referred to as what

Answer 32

Exothermic

Question 33

When energy is absorbed during a chemical reaction what is the process called?

Answer 33

Endothermic

Question 34

In this graph is this endothermic or exothermic? How can you tell?

Answer 34

Endothermic because from reactants to products, the endpoint is higher

Question 35

In exothermic reactions such as burning, will the product be higher or lower than the reactant on a graph?

Answer 35

The product will be lower

Question 36

How can energy cause chemical change?

Answer 36

Light causes things to decompose such as hydrogen peroxide

Question 37

What is an example of forms of energy produced by chemical changes?

Answer 37

Gas in a car, sound, heat

Question 38

I got this!

Question 39

Symbols written above the yields arrow in the equation mean what?

Answer 39

It could be a catalyst used to speed up the reaction without being part of the reaction. Or it could be heat or extra info.

Question 40

What’s the term used for numbers that come before an element in a compound?

Answer 40

Coefficients

Question 41

Do we ever change the subscript in a correctly written chemical formula?

Answer 41

NO

Question 42

Is AQ & L the same?

Answer 42

No AQ is dissolved in water/solution, L equals liquid

Question 43

Instead of writing gas or precipice, what is sometimes used?

Answer 43

Gas is upward arrow Precipapte is down arrow

Question 44

When balancing equations, what do we start and end with?

Answer 44

Start with where you have less And with oxygen and hydrogen

Question 45

When balancing equations, how do you reduce?

Answer 45

All or nothing

Question 46

When looking at a chemical reaction, what do we do first

Answer 46

Formulas first, then balance

Question 47

During a chemical reaction what is released/absorbed

Answer 47

Energy Exothermic equals energy released Endothermic equals energy, absorbed

Question 48

If there are kilojoules on the right PRODUCT side This means what?

Answer 48

It is exothermic

Question 49

Is photosynthesis endothermic or exothermic?

Answer 49

Endothermic

Question 50

Where is activation energy on this chart

Answer 50

From the starting line to the top of the hill. This is exothermic as the product is lower than the reaction.

Question 51

Explain the activity series

Answer 51

It’s a list of elements with the most reactive at the top, and the least at the bottom. It means those above have a greater tendency to lose electrons and they force elements lower on the list to accept electrons.  Example if copper is placed in solution of silver nitrate, copper has a greater tendency than silver to lose electrons. Silver is forced to accept electrons and will be reduced from +1 toa 0 oxidation state and copper is oxidized/becomes more positive

Question 52

RS (right arrow) R + S Is an example of what reaction

Answer 52

Decomposition starts with one and makes many Single compound, broken down into two or more simpler products

Question 53

A + B (right arrow) AB Is an example of what kind of reaction?

Answer 53

Synthesis This is ONE thing to the right of the yield arrow Two or more reactants combine to form ONE product Also, referred to as COMBINATION reactions

Question 54

What is the formula for a single replacement?

Answer 54

T + RS (yield arrow) TS + R Or U + RS (right arrow) RU + S if halogen kicking out another halogen

Question 55

The activity series is only used in what kind of reaction

Answer 55

Single replacement

Question 56

What is the formula for a double replacement?

Answer 56

AB + CD (yield arrow) AD + CB Cation listed first  Whatever is written first takes place of the other written first 

Question 57

Do subscripts travel

Answer 57

NO

Question 58

In a double replacement if both are aqueous it is what kind of reaction

Answer 58

No reaction

Question 59

Do we use the activity series for double replacement?

Answer 59

No

Question 60

Combustion reactions always have the same product which is what

Answer 60

CO 2 and’s H2O

Question 61

Formula for single replacement?

Answer 61

T + RS= TS + R The outside ones end up together

Question 62

When hydrogen gets kicked out, it becomes a what?

Answer 62

Diatomic Make sure to note 2 atoms!