Grade 10 Chem Midterm

Solids

Solids have definite shape and volume with tightly packed particles

Liquids

Liquids have definite volume but no fixed shape with particles that can slide past each other

Gases

Gases have no definite shape or volume with fast-moving particles spread far apart

Volume

the amount of space a substance occupies

Compressibility

how easily a substance’s volume can decrease under pressure

Density

mass per unit volume of a substance

Plasma

high-energy ionized gas state of matter

Phase Changes

transitions between solid

Sublimation

solid changing directly to gas

Deposition

gas changing to solid

Exothermic

process that releases heat

Endothermic

process that absorbs heat

Heating Curve

graph showing temperature change as heat is added

Cooling Curve

graph showing temperature change as heat is removed

IMFs

attractive forces between molecules

Polarity

uneven electron distribution causing partial charges

3 Types of IMFs

London dispersion, hydrogen bonding, Dipole-dipole

Hydrogen Bonding Elements

F O N

Intramolecular Forces

forces holding atoms together within a molecule

Vapor Pressure

pressure from evaporated particles above a liquid

Boiling Point

temperature where vapor pressure equals external pressure

Maxwell-Boltzmann Distribution

graph of particle speed distribution

Electronegativity

how strongly an atom attracts electrons in a bond

Temperature Definition

measure of average kinetic energy of particles

Atmospheric Makeup

composition of Earth’s atmosphere

78% N³

21% O²

0.93% Argon

Water, CO²

Carbon Dioxide History

originaly volcanos, now industrial and coal

Oxygenation of Earth’s Atmosphere

rise of atmospheric O₂ due to photosynthesis

Pressure Conversions

101.325kpa=1atm=760mmHg/torr

Temperature Conversions

converting between Celsius and Kelvin +-273

Boyle’s Law

pressure and volume are inversely related

Charles’ Law

volume and temperature are directly related

Gay-Lussac’s Law

pressure and temperature are directly related

Combined Gas Law

relationship of pressure, volume, temperature

Manometers

devices used to measure gas pressure

Manometer Measurements

using fluid height differences to determine pressure (mmHg)

Definition of Pressure

force per unit area from particle collisions

STP

0°C and 1 atm where 1 mole of gas = 22.4 L

SATP

25°C and 100 kPa

KMT Explanation

gas laws explained using particle motion

Boyle’s formula

P1V1 = P2V2

Gay-Lussac’s formula

P1/T1 = P2/T2

Charles’ formula

V1/T1 = V2/T2

combined gas law formula

P1V1/T1 = P2V2/T2

1 atm = 760 mmHg = 760 torr = 101.325 kPa

pressure unit equivalencies

temperature conversion

0°C = 273 K