MIDTERM (chp1-2)

Question 1

Matter

Answer 1

Anything that occupies space and has mass

Question 2

Mass (3):

Answer 2

• Pertains to the quantity of matter that an object has
• Unaffected by location
• Defined as resistance or acceleration

Question 3

Composition

Answer 3

The simple components that make up a material

Question 4

Structure

Answer 4

Refers to both the composition and arrangement of those simpler substances

Question 5

Extensive properties

Answer 5

Property that depends on the amount of substance present (eg. Mass, volume)

Question 6

Intensive properties

Answer 6

Depends only on the type of matter in a sample and not on the amount.e (eg. Temperature, melting point, density, odour)

Question 7

Physical properties

Answer 7

Properties that can be observed without the substance changing into another substance (eg. Texture, colour, boiling point of liquid)

Question 8

Chemical properties

Answer 8

Properties that matter exhibits as it is undergoing a change in chemical composition, or as it resists a change in chemical composition (eg. Iron rusts/gold doesn’t rust, hydrogen gas reacts with oxygen gas)

Question 9

Homogenous mixture

Answer 9

Mixtures in which the components are evenly blended throughout (eg. A cup of coffee, air around us)

Question 10

Heterogenous mixture

Answer 10

Mixtures in which the components are not evenly blended throughout (eg. Cookie dough with chocolate chips, sand and water)

Question 11

Element

Answer 11

Cannot be broken down into simpler substances and is the fundamental materials of which all matter is composed (eg. Iron, silver, oxygen, gold)

Question 12

Compound

Answer 12

Pure substances composed of more than one element in a fixed ratio (eg. Water is made of two parts hydrogen and one part oxygen)

Question 13

Classification of Matter (3):

Answer 13

• Solid: Non compressible and definite shape/volume
• Liquid: Slightly compressible, indefinite shape and definite volume
• Gas: Readily compressible, indefinite shape/volume, and takes shape and volume of container

Question 14

Melting

Answer 14

Solid to liquid

Question 15

Solidification

Answer 15

Liquid to solid

Question 16

Evaporation

Answer 16

Liquid to gas

Question 17

Condensation

Answer 17

Gas to liquid

Question 18

Sublimation

Answer 18

Solid to gas without going through liquid state

Question 19

Deposition

Answer 19

Gas to solid without going through liquid state

Question 20

Physical change

Answer 20

No change in the chemical composition of the matter (eg. Changes in physical state: ice melts to liquid water, changes in shape and size)

Question 21

Chemical change

Answer 21

Involves a change in chemical composition and will always produce at least one new substance (eg. When wood burns it produces water, carbon dioxide/monoxide

Question 22

Filtration

Answer 22

To separate solid and liquid

Question 23

Distillation

Answer 23

To separate two or more liquids with different boiling points

Question 24

Selective condensation

Answer 24

To separate gases with different condensation temperatures

Question 25

Chromatography

Answer 25

To separate pure liquids or solutions of compounds

Question 26

Potential energy

Answer 26

Energy that is stored

Question 27

Kinetic energy

Answer 27

Energy of motion

Question 28

Kinetic Molecular Theory (KMT)

Answer 28

Used to explain the behavior of matter based on the idea that particles are always in motion and posses both kinetic and potential energy

Question 29

Endothermic process

Answer 29

A change that absorbs energy

Question 30

Exothermic process

Answer 30

A change that releases heat energy

Question 31

Calorie

Answer 31

The amount of energy required to raise a temperature of one gram of liquid water by one degree

Question 32

Calorimetry

Answer 32

Science of measuring heat

Question 33

Hypothesis

Answer 33

A possible explanation for the observations

Question 34

Theory

Answer 34

An explanation of the behavior and why it happens

Question 35

Physical properties

Answer 35

The properties of a substance that can be measured without changing the identity of the substance (eg. Color, temperature, mass, volume, shape, hardness)

Question 36

Chemical properties

Answer 36

Properties of a substance that cannot be measured without changing the identity of a substance

Question 37

Exact numbers

Answer 37

Counted or defined and has no uncertainty (eg. "2".7)

Question 38

Measured numbers

Answer 38

Obtained with use of some measuring device and will have uncertainty (eg. 2."7")

Question 39

Precision

Answer 39

refers to how close measurements of the same item are to each other

Question 40

Accuracy

Answer 40

refers to how close a measurement is to the true or accepted value

Question 41

Random errors (2)

Answer 41

- Due to uncontrolled variables - Result in a decrease in precision

Question 42

Systematic errors (3)

Answer 42

- Constant errors - Lead to a decrease in accuracy, does not affect precision - Can be accounted for by calibration

Question 43

Significant figures

Answer 43

Digits contained in a measured value. The number of significant digits indicates how precisely a measurement is made

Question 44

Rule of sig figs in multiplication and division

Answer 44

Number of sig figs in the answer is limited to the measurement with the LEAST NUMBER OF SIG FIGS

Question 45

Rules of sig figs in addition and subtraction

Answer 45

Number of sig figs in the answer is limited by the term with the LEAST NUMBER OF DECIMAL PLACES

Question 46

Writing a number in scientific notation (2)

Answer 46

- Decimal point moves to the right in positive exponents until one nonzero digit remains - Decimal point moves to the left in negative exponents until one nonzero digit remains

Question 47

Scientific notation multiplication and division rules

Answer 47

With multiplication, you multiply the coefficients and add exponents. With division, you divide the coefficients and subtract the exponents

Question 48

Density mass volume calculations

Answer 48

- Density = mass/volume - Mass = density x volume - Volume = mass/density

Question 49

Density of water

Answer 49

1g/mL. Thus, objects less dense than 1g/mL will float and objects more dense than 1g/mL will sink

Question 50

Farenheit and Celsius conversion scale

Answer 50

- F = (9/5 x C) + 32 - C = (F-32) x 5/9

Question 51

Kevin scale

Answer 51

Scale used to describe events at very low temperatures and also to predict the way gases behave (K = C + 273.15)

Question 52

Celsius scale

Answer 52

A temperature scale commonly used throughout the world. Water freezes at 0 C and boils at 100 C

Question 53

Farenheit scale

Answer 53

A temperature scale commonly used in US. Water freezes at 32 F and boils at 212 F