Unit 3 Period Table - CHEM

group 1

alkali metals

group 2

alkaline earth metals

groups 3 - 12

transition metals

group 17

halogens

group 18

noble gases/inert gases

what does period correspond with

Principle energy level where valence electrons are located

Left of stair case

Metals

right of staircase

gases

on staircase

metalloids

nuclear charge

represented by atomic # and increases by each successive element

Why do valence electrons not experience full nuclear charge

1) repulsion

2) shielding (from inner electrons)

Across a period each element has….

the same shielding, greater nuclear charge, more effective nuclear charge

Down a group elements have….

the same effective nuclear charge, charge increases, shielding increases

atomic radius

half the distance between neighboring atoms

Trend down a group

increase PEL
Atomic radius increases

trend across period

atomic radius decreses

nuclear charge increases but PEL stays the same

Cations

greater nuclear charge

pulls electrons closer

smaller radius

anion

less nuclear charge

can not pull electrons as close

larger radius

isoelectronic

having the same numbers of electrons or the same electronic structure.

Electron affinity

A measure in the change in energy when 1 mole of electrons is added to one mole of gaseous atoms to form gaseous ions

is electron affinity endothermic or exothermic

exothermic

electronegativity

the measure of an elements attraction for an electron in a covalent bond

electronegativity trends

decreases down a group increases across a period

metals low, non metals high

Metals melting point

high, more valence electrons

non metal melting point

low,

metalloids

macromolecules, very high (SO2)

nobel gas

very low, monatomic

Group 1: alkali metals

lose 1 electron/valence electron

reacts with water to form basic solution

reacts with group 17 to form ionic salts

Fr is most reactive metal

Metal oxides

basic

Non metal oxides

acidic

amphoetric oxides

can act as both acid and base

ex: Al2O3

net ionic equation

A net ionic equation shows only the species that participate in a chemical reaction, omitting spectator ions.

Group 17: Halogens

7 valence electrons/ gained 1 electron

less reactive down a group

flourine gas color

yellow

chlorine gas color

yellowish/green gas

bromine liquid color

dark red liquid

iodine solid color

purple solid

displacement reaction

Displacement Reaction

A displacement reaction is a type of chemical reaction where an element or ion in a compound is replaced by another element or ion. There are two main types:

1. Single Displacement Reaction: One element displaces another in a compound.

2. Double Displacement Reaction: The ions of two compounds exchange places.

ending in ate

more Os - ate to c

ending in ite

less Os - ite to ous

transition metals

varying oxidation state

incomplete d sublevel as atom or ion

forms complete ions with ligands

catalytic and magnetic properties

what is zinc

not transition metal

no color (clear)

Ti oxidation states

+2+3+4

V oxidation states

+2+3+4+5

Cr Oxidation states

+2+3+4+5+6

Mn oxidation states

+2+3+4+5+6+7

Fe oxidation state

+2+3+4+5+6

Co oxidation states

+2+3+4+5

Ni oxidation states

+2+3+4

Cu oxidation states

+1+2+3+4

Why does Cr and Mn have high oxidation states mean

Good oxidizing agents down to +2 and +3

heterogeneous catalyst

catayst is in a different phase than the reactant

homogeneous catalyst

catalyst is in the same phase as the reactant

Na_²O + HCl

H₂O + 2NaCl Metal oxide

CaO+ H₂SO₄

CaSO₄ + H₂O Metal Oxides

CO₂+ Ca(OH)₂

CaCO₃+ H₂O Non Metal oxides

SO₃+2NaOH

NaSO₄ + H₂O Non Metal Oxides

Na₂O + H₂O

2NaOH Metal oxide in water

MgO +H₂O

Mg(OH)₂ Metal oxide in water

P₄O₁₀+ 6H₂O

4H₃PO₄

P₄O₆+6H₂O

4H₃PO₃

SO₃+H₂O

H₂SO₄

SO₂+H₂O

H₂SO₃

Cl₂O₇+H₂O

2HClO₄

Cl₂+H₂O

2HClO

Magnetic properties

How they behave when introduced to a magnetic/electric feild

Paramagnetic

Contains unpaired electrons

pulled into magnetic field

doesn’t retain magnetic properties after fields is removed

more unpaired electrons, More attraction

Diamagnetic

Contains only paired electrons

weakly repelled by magntic feild

doesn’t retain magnetic properties when field is removed

ferromagnetic

Contains unpaired electrons that allign parallel eachother in domains

retain magnetic properties when field is removed

Lewis acids

giver up electrons

lewis bases

accept electrons

Spectro Chemicle series

I^→< Cl^-<F^-<OH^-<H₂O<SCN^-<NH₃<NO^₂-<CN^-/CO

Fe⁺³

Heme in blood to transport oxygen

CO⁺³

Vitamin B

Palladium and Platinum (Pd and Pt

Catalyst in catalytic converter in car reduces NO and CO reduction

Iron

haber process/production of ammonia

Vanadium oxide (V2O5)

Contact process production of sulfuric acid

Nickle

Hydrogenation reaction

Manganese oxide MnO2

decomposition of hydrogen peroxide

monodentant ligands

Form one coordinate covalent bond using one lone pair

Color of transition metals

• Partially filled d orbitak

• the color absorbed is determined by the color emitted

What factors increase splitting

larger metals

higher oxidation state

Higher geometry

Stronger ligand

ligands are Lewis bases so transition metals are

lewis acids

Identiity of central ion

Larger metals provide greater splitting

Higher nuclear charge pulls ligands closer causing greater splitting

Oxidation state of metal ion

As oxidation state increases for the SAME metal the d orbital splitting increases

Geometry of a complex ion

Octahedral (6) > Tetrahedral (4) > Linear (2)

identity of ligand

Stronger ligand = greater splitting

(spectrochemical series)

ions with the same number of electrons

isoelectronic