topic 2

What are atoms made of?

Protons, neutrons, electrons

Mass of protons and neutrons

1.66 x10^(24) g

Mass of an electron

9.1 ×10^(-28)

What subatomic particles impact the charge of an atom/ion?

Protons and elections

Atoms have _ charge

No. Because the number of electrons equals the number of protons

Ions have _ charge

Any charge other than 0. This is because the number of electrons does not equal the number of electrons

Anion

Negatively charged ions; electrons are added

Cation

Positive charged ion; electrons are removed

Isotopes depends on

The number of neutrons

Average mass equation

. Mass # (%) + … + mass #(%)

1 orbital can hold _ elections at a time

2

4 characterized shapes of an atomic orbital

S,p,d,f : from lowest to highest energy levels; the further from the nucleus the orbital is, the larger it is

S orbital

Spherically shaped; hold max of 2 elections

P orbital

Dumbbell shaped. 3 shapes per shell: px, py, pz, holds up to 6 electrons, starts at 2p

D orbital

Generally clover shaped. 5 shapes per shell dxz, dyz, dxy, D( x )^2 (y)^2, dz^2. 1 Shell can hold up to 10 elections

How to use the periodic table to find orbitals of most elements?

Period indicates orbital # ( energy level ). Group indicates orbital shape (subshell/letter)

Group 1 and 2 = s orbital

Transition metals = d orbital

Rest = p orbital

Electron configuration

Lists out the orbitals and electrons. Can use nearest noble gas as a shorthand

When we fill orbitals with elections, we fill each orbital with ..

An unpaired electron, then begin to pair them.

Paramagnetic

If any electron is unpaired

Diamagnetic

. If all electrons are paired. When 2 electrons are in the same subshell, they fill spin up/down and magnetic moments cancel out

list all electron configuration exceptions:

d4 exceptions: (Cr and Mo) s^1 d^5

d9 exceptions: (Cu, Ag, Au, Rg) s^1 d^10

Tc: [Kr] 5s^1 4d^6

Pd: [Kr] 5s^0 4d^10

Ru: [Kr] 5s^1 4d^7

Rh: [Kr] 5s^1 4d²

Pt: [Xe] 6s^1 5d^9

what are the d4 exceptions and why do they exist?

Cr and Mo are the d4 exceptions with the basic electron configuration being 4s^1 and 3d^5

They exist due to Hundt’s Rule

Hund’s Rule

electrons fill the sub shell first before pairing

what are the d9 exceptions and why do they exist

Cu, Ag, Au, and Rg are exceptions to electron configuration. basic configuration is: s^1 d^10

this happens because this electron configuration is lower in energy than s² d^9

electron configuration rule for transition metal cations

electrons must come out of the outer s orbital before the inner/lower energy d orbital

electron configuration rule for group 1 and 2 cations

electrons always come out of higher energy outer shell s orbital

electron configuration of technetium (Tc)

[Kr] 5s^1 4d^6

electron configuration of palladium (Pd)

[Kr] 5s^0 4d^10

electron configuration of rhodium (Rh)

[Kr] 5s^1 4d²

electron configuration of ruthenium (Ru)

[Kr] 5s^1 4d^7

electron configuration of platinum (Pt)

[Xe] 6s^1 5d^9