General Chemistry Mcat

Front 1

The Bohr Model of the atom has up to how many electrons?

Back 1

One.

Front 2

Aufbau Principle

Back 2

Electrons occupy the lowest energy orbitals available.

Front 3

Hund's Rule

Back 3

Electrons in the same subshell occupy available orbitals singly, before pairing up.

Front 4

Pauli Exclusion Principle

Back 4

There can be no more than 2 electrons in any given orbital.

Front 5

Paramagnetic

Back 5

When an atom's electrons are NOT all spin paired. Will be attracted to an external magnetic field.

Front 6

What are the five exceptions to electron configurations?

Back 6

Cr, Cu, Mo, Ag, and Au.

Front 7

Isoelectronic

Back 7

Atoms sharing same electron configuration due to differences in electrons.

Hint 7

F- and Ne are isoelectronic.

Front 8

Metalloids possess qualities of what and what? Can you name all 7 metalloids?

Back 8

Metals and nonmetals. B, Si, Ge, As, Sb, Te, Po.

Front 9

First ionization energy (IE, or IE1)

Back 9

Amount of energy needed to remove the least tightly bound electron from an isolated atom

Front 10

Second isolation energy (IE2)

Back 10

Amount of energy needed to remove the least tightly bound electron from the cation.

Front 11

How does IE1 compare to IE2?

Back 11

IE2 is always less than IE1.

Front 12

Coordinate Covalent bond

Back 12

When one atom donates BOTH of the shared electrons in a bond.

Front 13

ion-dipole forces

Back 13

polar molecules being attracted to ions

Front 14

dipole-dipole forces

Back 14

+ and - ends of polar molecules being attracted to each other

Front 15

dipole-induced dipole force

Back 15

permanent dipole inducing a dipole in a nonpolar molecule

Front 16

London Dispersion Forces

Back 16

if you have electrons (e-) you have LDF. weakest force. (the more electrons, i.e. bigger molecule, the higher the LDF)

Front 17

Van der Waals

Back 17

dipole forces, hydrogen bonding, LDF. Are weaker than ionic, network, and metallic bonds.

Front 18

How does a stronger intermolecular force affect mp, bp, viscocity, and vapor pressure?

Back 18

higher mp

higher bp

higher viscocity

lower vapor pressure (evaporates less easily, less volatile)

Front 19

Ionic solids

Back 19

held together by attraction between cations and anions

Front 20

Network solids

Back 20

atoms connected in lattice of covalent bonds (diamond, quartz)

Front 21

Metallic solids

Back 21

covalently bound lattice of nuclei with one electron from each atom floating around

Front 22

molecular solids

Back 22

held together by van der waals forces.

Hint 22

much weaker than other forces. lower bp, lower mp.

Front 23

What charge and what size make for the strongest ionic bonds?

Back 23

Larger charges and smaller ions make the strongest ionic bonds!

Front 24

Zeroth Law of Thermodynamics

Back 24

if two systems are both in thermal equilibrium with a third system, than the two initial systems are in thermal equilibrium with each other

Front 25

First Law of Thermodynamics

Back 25

energy cannot be created nor destroyed. an isolated system has constant energy.

Front 26

Hess's Law

Back 26

sum of energies absorbed or given off in steps is the same as the total for a given reaction

Front 27

Second Law of Thermodynamics

Back 27

the universe wants maximum chaos/disorder/entropy

Front 28

Third Law of Thermodynamics

Back 28

defines absolute zero to be a state of zero entropy. all motion stops. S=0, T=OKelvin.

Front 29

Enthalpy

Back 29

heat energy released or absorbed when bonds are broken and formed at constant pressure.

Hint 29

also can be thought of the energy stored in chemical bonds