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Chemistry Honors > Intro to chemistry & Significant Figures > Flashcards

Intro to chemistry & Significant Figures Flashcards

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
Physical change
when some properties change, but the composition of the material/identity does not change
26
Chemical change
a change in which the composition and properties of a substance change, and one or more new substance are produced
27
Malleability
refers to a material being able to be hammered into thin sheets
28
Ductility
refers to the ability to be drown into thin wires
29
Boiling point
refers to the temperature at which a substance turns into a liquid into a vapor (gas)
30
Frequency
amount of wavelength that passes a given point every single second
31
Viscosity
refers to how thick or thin(runny) a liquid is
32
Solubility
refers to the ability of a substance to be dissolved
33
Intensive properties
properties that do not depend on the amount of matter present ex: color, odor, malleability, ductility, density
34
Extensive properties
properties that depend on the amount of matter ex: mass, weight, volume, length
35
Energy
ability to do work or cause change. In chemistry work is the production of something, like heat
36
Potential Energy
energy stored in matter because of its relative position (stored energy)
37
Kinetic Energy
energy available because of the motion of an object (energy of motion)
38
Types of Energy are
MRCENTS m = mechanical r = radiant c = chemical e = electrical n = nuclear t = thermal s = sound
39
Mechanical energy
energy of motion (kinetic) or energy of position (potential)
40
Radiant energy
energy of light also referred as light energy or electromagnet energy - travels in waves & in a straight path from one place to another
41
Chemical energy
energy stored in the bonds of molecules - a form of potential energy
42
Eletrical Energy
energy of moving electrons or electrical charges
43
Nuclear Energy
energy locked in the nucleus of an atom
44
Nuclear fission
the process of splitting atoms
45
Nuclear Fusion
two or more atoms violently joined together to make a larger atoms-stars
46
Thermal energy
particles of hot objects move faster than particles of cooler objects - energy of heat
47
Sound energy
energy from vibration in matter (waves) - can travel through solids, liquids, & gas
48
Conservation of energy
can be neither created nor destroyed - one form of energy can be converted to another
49
Endothermic
energy is absorbed from the surrounding. Temperature of the surroundings decrease and the surrounding reaction feels cold
50
Exothermic
energy is released. The temperature of the surroundings will increase, and the surrounding reaction feels warm
51
What phase change is Sold to Liquid & is it Endothermic of Exothermic?
Melting or Fusion Endothermic
52
What phase change is Liquid to Gas & is it Endothermic of Exothermic?
Boiling or Vaporization Endothermic
53
What phase change is Sold to Gas & is it Endothermic of Exothermic?
Sublimation (sublime) Endothermic
54
What phase change is Gas to Liquid & is it Endothermic of Exothermic?
Condensation Exothermic
55
What phase change is Liquid to Solid & is it Endothermic of Exothermic?
Freezing or crystallization or solidification Exothermic
56
What phase change is Gas to Solid & is it Endothermic of Exothermic?
Deposition Exothermic
57
Calorimetry
measure of heat
58
Specific Heat
The quantity of heat needed to raise the temperature of 1.0 gram of a substance by 1 degree Celsius
59
Heat of Fusion
the amount of energy required to change a given amount of solid to a liquid or liquid to solid at constant temperature
60
Heat of Vaporization
the amount of energy needed to change a given amount of liquid to a gas or gas to liquid at a constant temperature
61
Scientific Notation
is the way that scientist easily handle very large numbers or very small numbers
62
Accuracy
refers to how closely a measured value agrees with the correct value
63
Precision
refers to how closely individual measurements agree with each other
64
Significant figures
are digits that are part of any valid measurement - significant are numbers 1 - 9
65
____ are never significant
Leading zeros ex: 0.ooo1 (1sf)
66
____ are always significant
Imbedded zeros (zeros located between nonzero numbers) ex: 1.0285 (5sf) or 202.03 (5sf)
67
___ are significant if the decimal point is specified
Trailing zeros ex: 60. (2sf) or 60.ooo (5sf)
68
All ___ numbers are significant
Nonzero ex: 2.735 (4sf)
69
Adding and Subtracting significant figures
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
Multiplying and Dividing significant figures
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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