Unit 2 Chemistry Test

alkali metals

1st group
1+ charge

alkaline earth metals

2nd group
2+ charge

transition metals

3rd -12th group
varying charges, including Sn and Pb, excluding Ag and Cd and Zn

Ag charge

1+

Cd and Zn charge

2+

halogens

17th group
1- charge

noble gases

18th group
no/neutral charge

metalloids

along the staircase, excluding Al
some of the characteristics of metals

metals

left to the staircase
generally solid, shiny, lustrous, ductility, malleable, conductive

nonmetals

right to the staircase
opposite/no characteristics of metals

wavelength

distance between 2 identical points on consecutive waves
λ

frequency

the number of waves that pass a fixed point in unit time
ν

energy

energy of a specific quantum of energy
E=hν
frequency times planck's constant

energy and frequency relationship

directly related

energy and wavelength relationship

inversely related

wavelength and frequency relationship

inversely related

speed of light equation

c=λν

Bohr's Model

circular rings
electrons follow a fixed path
energy levels n=1 to n=7

Quantum Mechanical Model (QMM)

different shaped areas with a 90% chance of finding an electron
electrons do not follow fixed path
energy levels n=1 to n=7

Orbit

Heisenberg Uncertainty Principle

we cannot know both the position and speed of a particle with perfect accuracy, the more we know about the position the less we know about the momentum and vise versa

Orbital

an area where there is a 90% chance of finding a given electron
different shapes = s, p, d, f
energy levels n=1 to n=7

S Orbital

spherical
starts at 1st energy level (n=1)

node

an area with no electrons/low probability of electrons being found

P Orbital

dumbbell/lobe
starts at 2nd energy level (n=2)
each level contains 3 degenerate orbitals

degenerate orbitals

orbitals having the same energy levels but they are positioned differently

D Orbital

clover leaf
starts at 3rd energy level (n=3)
each level contains 5 degenerate orbitals

F Orbital

starbursts
starts at 4th energy level (n=4)
each level contains 7 degenerate orbitals

energy levels

the fixed amount of energy that a system described by quantum mechanics

valence electrons

outer electrons in an atom

core electrons

inner electrons in an atom

orbital diagram

a type of notation which illustrates an atom's electron distribution and electron spin within orbitals.

Hund's rule

electrons must be unpaired before they are paired in a sublevel

Pauli Exclusion

no more than two electrons can occupy the same orbital and two electrons in the same orbital must have opposite spins

Aufba Principle

electrons fill from lowest to highest energy

period similarities

same number of core electrons

group similarities

same number of valence electrons

Trends with atomic radius

decreases as you go the the left and increases as you go down

Trends with ionization energy

increases as you go the the left and decreases as you go down

atomic radius and IE relationship

inversely related

atomic radius and reactivity relationship

directly related

reactivity and IE relationship

inversely related