IB Chem Semester 1

Particulate Nature of Matter

100

CO₂(g) dissolved in H₂O vs CO₂ produced from combustion

 Mixture vs chemical product

200

Has the same uniform composition throughout

Homogeneous mixture

300

Sample contains particles that move in all directions, have the highest amount of energy and the weakest forces of attraction

gases

400

Explanation of energy change during melting

Heat energy supplied increases the potential energy of the substance to overcome forces between particles with no increase in kinetic energy

500

All alloys are 

mixtures

Atomic Structure & Periodicity

100

Decreases in size from left to right on the periodic table

Atomic radius

200

A negatively charged particle of an atom

electron

300

An atom with the same number of protons but a different number of neutrons

isotope

400

Group 1 of the periodic table

Alkali metals

500

Compared with atomic radius, this increases for metals and decreases for nonmetals

Ionic radius

Ideal Gases

100

Formula to calculate molar volume of gas NOT at STP

V = nRT / P

200

High Pressure and Low Temperature

Conditions when real gases deviate most from ideal behavior

300

At constant Temperature, volume is inversely proportional to its pressure

Boyle's law

400

Volume of 2 moles of CO₂ at STP

45.4 dm³

500

Assumptions of Ideal Gas Model

-particles in constant random motion
-particles have no volume
-no forces between particles
-all collission are elastic

Bonding

100

A bond form when elements attain a full outer electron shell by transferring electrons

Ionic bond

200

Two or more atoms sharing electrons

Covalent Bond

300

London forces, permanent dipole-dipole interactions, hydrogen bonding

Intermolecular forces

400

These forces arise from polar bonds and asymmetry in molecules

Dipole-diole forces

500

These molecules are generally solube in nonpolar solvents

Nonpolar molecules

Classifying Matter

100

Homologous class of compounds containing double bond(s)

alkenes

200

IUPAC name for a 4-carbon alkane with an hydroxyl on carbon 2

butan-2-ol

300

A dark red-brown solution is produced when KI is mixed with

Br₂ or Cl₂ because they are both more reactive halogens and displace the less reactive halogen from solution

400

Alcohols have a higher relative boiling point compared with comparable molecular mass aldehydes and alkanes because of

alcohols can form hydrogen bonds, where as the aldehydes can form dipole-dipole forces, and alkanes only form LDFs

500

Trend in 1st ionization energy across period 3

Ar > Cl > S =P > Si > Mg > Al > Na