Chapter 1 Flashcards
Matter
Anything that occupies space and has mass.
Atoms
A particle that consists of a nucleus of protons and neutrons surrounded by electrons.
The basic building block of all matter.
Molecules
A group of two or more atoms held together by attractive forces known as chemical bonds.
Element
A chemical substance made up of only one type of atom. It cannot be broken down into other substances.
Each element has an atomic number, which denotes the amount of protons of this atom type.
Solid
Shape: Fixed
Volume: Fixed
Compressible: No
Flow: No
Liquid
Shape: Indefinite
Volume: Fixed
Compressible: No
Flow: Yes
Gas
Shape: Indefinite
Volume: Indefinite
Compressible: Yes
Flow: Yes
Physical state of matter
The three basic physical states of matter are solid, liquid, and gas.
This is determined by the molecular structure, each with different properties.
Homogeneous solution
Matter that is uniformly distributed throughout the solution.
Heterogeneous solution
Matter that is non-uniformly distributed throughout a solution.
Physical properties
The characteristics of matter that can be observed without changing its molecular composition.
Any characteristic that is measurable, whose value describes a state of a physical system.
Examples
* Color
* Density
* Hardness
* Melting/Boiling points
* Electrical conductivity
Chemical properties
Any of a substance’s properties that becomes evident during or after a chemical reaction. A quality that can be established only by changing the substance’s chemical identity.
Examples:
* Flammability
* Heat of combustion
* Chemical stability
* Toxicity
Pure substance
Any substance that cannot be broken down through physical means.
Elements & compounds are pure substances
Mixtures
Substances that can be broken down through physical means.
Can be further classified into homogeneous and heterogeneous mixtures.
Separation of mixtures:
Distillation
The physical separation of a mixture through boiling
Separation of mixtures:
Filtration
The physical separation of a mixture through exploitation of the differences in state of matter of its constituent components
Separation of mixtures:
Chromatography
The physical separation of a mixture through exploitation of adherence properties of its constituent components.
Separation of mixtures:
Evaporation
The physical separation of a mixture through conversion of a liquid to its vapor form below the boiling point.
Length
The measure of the two dimensional distance an object occupies.
Meters
Mass
Measure of the amount of matter present in an object.
Grams
Volume
The measure of the three dimensional space occupied by an object.
Cubic Meter (m³)
Density
The ratio of mass over volume of an object.
Solids: g/cm³ (g/mL)
Liquids: g/mL
Gases: g/L
Archimedes Principle
The volume of a solid can be determined by water displacement.
Exception to the density rule
Solids > Liquids > Gases
Water.
Ice is less dense than the liquid form.
SI System
SI System:
Giga
G
Billion: 1,000,000,000
Base x 10⁹
SI System: Giga
Billion: 1,000,000,000
Base x 10⁹
SI System:
Mega
M
Million: 1,000,000
Base x 10⁶
SI System:
Kilo
k
Thousand: 1,000
Base x 10³
SI System:
Hecto
h
Hundred: 100
Base x 10²
SI System:
Deka
da
Ten: 10
Base x 10¹
SI System:
Deci
d
Tenth: 0.1
Base x 10⁻¹
SI System:
Centi
c
Hundredth: 0.01
Base x 10⁻²
SI System:
Milli
m
Thousandth: 0.001
Base x 10⁻³
SI System:
Micro
μ
Millionth: 0.000,001
Base x 10⁻⁶
SI System:
Nano
n
Billionth: 0.000,000,001
Base x 10⁻⁹
Converting volume between prefixes
Multiply the exponent by a factor of 3.
Converting meter to millimeter:
Base x 10⁻³*³ -> Base x 10⁻⁹
1m³ = 1,000,000,000mm³
Scientific notation
- Move the decimal point of a number to the right of the first non-zero digit.
- Multiply by 10ⁿ
- n is the number of places the decimal point was moved.
- If the number is greater than 1, then n is positive.
- If the number is less than 1, then n is negative
12340 = 1.234 x 10⁴
The decimal point was moved 4 places
.001234 = 1.234 x 10⁻³
The decimal point was moved 3 places
Significant Figures
All digits are significant figures.
* Example: 45.872 has 5 significant figures.
Trailing Zeroes with a decimal are significant
* Example: 1.050 has 4 significant figures.
* Example: 500.0 has 4 significant figures
Trailing Zeroes without a decimal are NOT significant
* Example: 5,200 has 2 significant figures
Leading zeroes of a decimal are NOT significant
Example: 0.00123 has 3 significant figures.
Significant Figures: Addition/Subtraction
When adding or subtracting numbers in regards to significant figures, the answer will round to the lowest decimal places.
5.74 + 2.823 = 8.56
2DP + 3DP = 2DP
Significant Figures:
Multiplication/Division
When multiplying or dividing two numbers in regards to significant figures, the answer will round to the lowest significant figures
5.02 * 2.4425 = 12.3
3SF + 5SF = 3SF
Temperature
Measure of the average kinetic energy of the molecules in a sample.
Celsius to Kelvin Conversion
To find Kelvin, add 273.15 to the Celsius value.
K = °C + 273.15
Fahrenheit to Celsius Conversion
°C = (°F-32)/1.8
To find Celsius, subtract 32 from the Fahrenheit value and divide by 1.8
Extensive Property
A property that depends on the amount of matter of a sample
Intensive Property
A property that depends on the type of matter of a sample
