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Chemistry Honors > Intro to chemistry & Significant Figures > Flashcards

Intro to chemistry & Significant Figures Flashcards

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1
Q

What is matter?

A

anything that has a mass & volume

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2
Q

Define mass

A

amount of matter an object contains

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3
Q

Define Volume

A

amount/measure of space occupied by the object

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4
Q

Physical properties

A

properties which can be determined without causing a change in identity of the substance

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5
Q

Examples of Physical properties

A

texture, color, odor, mass, taste, boiling point, freezing point, shape, density

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6
Q

Chemical Properties

A

characteristic of a substance that describe how the substance reacts (or doesn’t react) to produce a new substance

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7
Q

Examples of Chemical Properties

A

rusting, tarnish, oxidize

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8
Q

Density

A

a large factor when deciding if an object or substance will sink or float in another substance

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9
Q

Element

A

substance that cannot be decomposed (breakdown) to a simpler substance by ordinary chemical change
Classified as metal, non-metal, & metalloid

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10
Q

Substance (pure substances)

A

a type of mater, all of whose samples have the same exact composition and structure and all of the same properties. ONLY COMPUNDS AND ELEMENTS ARE SUBSTANCES.

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11
Q

Compound

A

a substance composed of two or more different element chemically combined in a fixed ratio

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12
Q

what are the Diatomic Elements

A

Br2, I2, N2, Cl2, H2, O2, F2 = BrINClHOF

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13
Q

Mixtures

A

two or more substance that are PHYSICALLY combined and can be physically separated. The composition is variable (change)

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14
Q

What are the 2 types of mixtures

A

Heterogeneous (different) & Homogenous (same)

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15
Q

Heterogenous

A

has visibly different parts. It is not uniformed throughout & particles are not evenly distributed

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16
Q

Homogenous

A

uniformed throughout and is evenly distibuted

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17
Q

Amalgam

A

Example of a metal alloy
Ag (silver) and Hg (mercury), Brass (Cu and Zn)

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18
Q

Filtration

A

only used for separating large particles that are insoluble (do not dissolve)

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19
Q

Distillation

A

separation by boiling point (different boiling points to work)

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20
Q

Paper Chromatography

A

a solution is separated by allowing it to flow along a stationary phase. Used for inks and pigments

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21
Q

Crystillization

A

a concentrated solution at a relatively high temperature and allow the solution to cool slowly

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22
Q

Solids

A

have a definite shape and volume
- tightly packed together and are incompressible

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23
Q

Liquids

A

have an indefinite shape, flows. and has a fixed volume
- fill the shape of their container
- almost incompressible

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24
Q

Gas

A

take the shape and volume of its container
- can be compressed

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25
Q

Physical change

A

when some properties change, but the composition of the material/identity does not change

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26
Q

Chemical change

A

a change in which the composition and properties of a substance change, and one or more new substance are produced

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27
Q

Malleability

A

refers to a material being able to be hammered into thin sheets

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28
Q

Ductility

A

refers to the ability to be drown into thin wires

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29
Q

Boiling point

A

refers to the temperature at which a substance turns into a liquid into a vapor (gas)

30
Q

Frequency

A

amount of wavelength that passes a given point every single second

31
Q

Viscosity

A

refers to how thick or thin(runny) a liquid is

32
Q

Solubility

A

refers to the ability of a substance to be dissolved

33
Q

Intensive properties

A

properties that do not depend on the amount of matter present
ex: color, odor, malleability, ductility, density

34
Q

Extensive properties

A

properties that depend on the amount of matter
ex: mass, weight, volume, length

35
Q

Energy

A

ability to do work or cause change. In chemistry work is the production of something, like heat

36
Q

Potential Energy

A

energy stored in matter because of its relative position (stored energy)

37
Q

Kinetic Energy

A

energy available because of the motion of an object (energy of motion)

38
Q

Types of Energy are

A

MRCENTS
m = mechanical
r = radiant
c = chemical
e = electrical
n = nuclear
t = thermal
s = sound

39
Q

Mechanical energy

A

energy of motion (kinetic) or energy of position (potential)

40
Q

Radiant energy

A

energy of light also referred as light energy or electromagnet energy
- travels in waves & in a straight path from one place to another

41
Q

Chemical energy

A

energy stored in the bonds of molecules
- a form of potential energy

42
Q

Eletrical Energy

A

energy of moving electrons or electrical charges

43
Q

Nuclear Energy

A

energy locked in the nucleus of an atom

44
Q

Nuclear fission

A

the process of splitting atoms

45
Q

Nuclear Fusion

A

two or more atoms violently joined together to make a larger atoms-stars

46
Q

Thermal energy

A

particles of hot objects move faster than particles of cooler objects
- energy of heat

47
Q

Sound energy

A

energy from vibration in matter (waves)
- can travel through solids, liquids, & gas

48
Q

Conservation of energy

A

can be neither created nor destroyed
- one form of energy can be converted to another

49
Q

Endothermic

A

energy is absorbed from the surrounding. Temperature of the surroundings decrease and the surrounding reaction feels cold

50
Q

Exothermic

A

energy is released. The temperature of the surroundings will increase, and the surrounding reaction feels warm

51
Q

What phase change is Sold to Liquid & is it Endothermic of Exothermic?

A

Melting or Fusion
Endothermic

52
Q

What phase change is Liquid to Gas & is it Endothermic of Exothermic?

A

Boiling or Vaporization
Endothermic

53
Q

What phase change is Sold to Gas & is it Endothermic of Exothermic?

A

Sublimation (sublime)
Endothermic

54
Q

What phase change is Gas to Liquid & is it Endothermic of Exothermic?

A

Condensation
Exothermic

55
Q

What phase change is Liquid to Solid & is it Endothermic of Exothermic?

A

Freezing or crystallization or solidification
Exothermic

56
Q

What phase change is Gas to Solid & is it Endothermic of Exothermic?

A

Deposition
Exothermic

57
Q

Calorimetry

A

measure of heat

58
Q

Specific Heat

A

The quantity of heat needed to raise the temperature of 1.0 gram of a substance by 1 degree Celsius

59
Q

Heat of Fusion

A

the amount of energy required to change a given amount of solid to a liquid or liquid to solid at constant temperature

60
Q

Heat of Vaporization

A

the amount of energy needed to change a given amount of liquid to a gas or gas to liquid at a constant temperature

61
Q

Scientific Notation

A

is the way that scientist easily handle very large numbers or very small numbers

62
Q

Accuracy

A

refers to how closely a measured value agrees with the correct value

63
Q

Precision

A

refers to how closely individual measurements agree with each other

64
Q

Significant figures

A

are digits that are part of any valid measurement
- significant are numbers 1 - 9

65
Q

____ are never significant

A

Leading zeros
ex: 0.ooo1 (1sf)

66
Q

____ are always significant

A

Imbedded zeros (zeros located between nonzero numbers)
ex: 1.0285 (5sf) or 202.03 (5sf)

67
Q

___ are significant if the decimal point is specified

A

Trailing zeros
ex: 60. (2sf) or 60.ooo (5sf)

68
Q

All ___ numbers are significant

A

Nonzero
ex: 2.735 (4sf)

69
Q

Adding and Subtracting significant figures

A

the answer cannot have more decimal places than the measurement that has the LEAST NUMBER OF DECIMAL PLACES.
ex: 10.3 (1 decimal place) + 20.475 (3 decimal places) = 30.8 (1 decimal place)

70
Q

Multiplying and Dividing significant figures

A

the answer cannot have more significant figures than the measurement with the LEAST NUMBER OF SIGNIFICANT FIGURES.
ex: 51 (2sf) / 213 (3sf) = .24 (2sf)

Chemistry Honors (1 decks)

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