Chemistry I - Chapter One

Chemistry

Study of matter and the changes matter undergoes

Matter

Anything that has mass and occupies space

Atom

Smallest particle of an element that retains the element's properties

Molecule

Two or more atoms joined by chemical bonds

Element

Pure substance made of only one type of atom

Compound

Pure substance made of two or more elements chemically combined

Mixture

Physical combination of substances

Homogeneous Mixture

Mixture with uniform composition throughout

Solution

Another name for a homogeneous mixture

Heterogeneous Mixture

Mixture with nonuniform composition

Pure Substance

Matter with fixed composition and properties

Solid

State of matter with definite shape and volume

Liquid

State of matter with definite volume but variable shape

Gas

State of matter with neither definite shape nor volume

Plasma

Ionized gas containing charged particles

Mass

Amount of matter in an object

Weight

Force of gravity acting on an object

Volume

Amount of space occupied by an object

Density

Mass divided by volume

Physical Property

Property observed without changing composition

Chemical Property

Property describing how a substance reacts

Physical Change

Change that does not alter chemical identity

Chemical Change

Change that creates new substances

Extensive Property

Property dependent on amount present

Intensive Property

Property independent of amount present

Hypothesis

Tentative explanation that can be tested

Theory

Well-tested explanation of natural phenomena

Law

Statement describing an observed natural relationship

Scientific Method

Observation, hypothesis, experimentation, conclusion

Macroscopic Domain

Observable world seen directly

Microscopic Domain

Atomic and molecular world

Symbolic Domain

Chemical symbols, formulas, equations, graphs

Law of Conservation of Matter

Matter is neither created nor destroyed

Law of Definite Proportions

Compounds contain elements in fixed mass ratios

Accuracy

Closeness to the true value

Precision

Closeness of repeated measurements to one another

Uncertainty

Estimated amount of measurement error

Significant Figures

Digits known with certainty plus one estimated digit

Exact Number

Number from counting or definition

Dimensional Analysis

Method of solving problems using units

Conversion Factor

Ratio used to convert between units

Length

Measurement of distance

Temperature

Measure of hotness or coldness

Meter

SI unit of length

Kilogram

SI unit of mass

Second

SI unit of time

Kelvin

SI unit of temperature

Ampere

SI unit of electric current

Mole

SI unit for amount of substance

Candela

SI unit of luminous intensity

Cubic Meter (m³)

SI unit of volume

Liter (L)

Common metric unit of volume

Milliliter (mL)

One-thousandth of a liter

Cubic Centimeter (cm³ or cc)

Equivalent to 1 mL

Density Formula

Density = Mass ÷ Volume

Accuracy

How close a measurement is to the true value

Precision

How close repeated measurements are to each other

Quantitative Property

Property expressed with numbers

Qualitative Property

Property based on observation

Tera-

T, 10¹²

Giga-

G, 10⁹

Mega-

M, 10⁶

Kilo-

k, 10³

Hecto

h, 10²

Deka-

da, 10¹

Deci-

d, 10⁻¹

Centi-

c, 10⁻²

Milli-

m, 10⁻³

Micro-

μ, 10⁻⁶

Nano

n, 10⁻⁹

Pico-

p, 10⁻¹²

Length

Meter, m

Mass

Kilogram, kg

Time

Second, s

Tempature

Kelvin, K

Electric Current

Ampere, A

Amount of substance

Mole, mol

Luminous Intensity

Candela, cd

Density

d = m/V

Mass

m = dV

Volume

V = m/d

Celsius to Kelvin

K = °C + 273.15

Celsius to Fahrenheit

°F = (9/5 × °C) + 32