Chapter 3 - Compounds & the Mole

H

Hydrogen

He

Helium

Li

Lithium

Be

Beryllium

B

Boron

C

Carbon

N

Nitrogen

O

Oxygen

F

Fluorine

Ne

Neon

Na

Sodium

Mg

Magnesium

Al

Aluminum

Si

Silicon

P

Phosphorous

S

Sulfur

Cl

Chlorine

Ar

Argon

K

Potassium

Ca

Calcium

Sc

Scandium, transition metal

Ti

Titanium, transition metal

V

Vanadium, transition metal

Cr

Chromium, transition metal

Mn

Manganese, transition metal

Fe

Iron, transition metal

Co

Cobalt, transition metal

Ni

Nickel, transition metal

Cu

Copper, transition metal

Zn

Zinc, transition metal always 2+

Ga

Gallium

Ge

Germanium

As

Arsenic

Se

Selenium

Br

Bromine

Kr

Krypton

Sr

Strontium

Ag

Silver, transition metal, 1+ charge

Sn

Tin

I

Iodine

Xe

Xenon

Pt

Platinum, transition metal

Au

Gold, transition metal

Pb

Lead

Rn

Radon

Ra

Radium

transition metals list

Scary Tiny Vicious Creatures Mean Females Come Nightly to Club Z

• Sc

• Ti

• V

• Cr

• Mn

• Fe

• Co

• Ni

• Cu

• Zn

• Ag, Pt, Au

diatomic elements

Elements that naturally form pairs. Their pure form is as two-atom molecules. Examples include hydrogen (H₂), nitrogen (N₂), oxygen (O₂), fluorine (F₂), chlorine (Cl₂), bromine (Br₂), and iodine (I₂).

HOFBrINCl

ions form when…

atoms or molecules gain or lose electrons

neutral sodium atom transforming to a sodium atom

Na → Na^+ + e^-

neutral oxygen atom transforming into an oxygen ion

O + 2e^- → O^2-

Is there a change in the number of protons when an ion forms?

No

ionic compound

* formed through the transfer of electrons between atoms
* consists of positively charged ions (cations) and negatively charged ions (anions) held together by electrostatic forces
* salt, electrolyte

ionic compound examples

* sodium chloride (Na^+ Cl^-)
* calcium carbonate (CaCO3)
* sports drinks = sugar + salt water (electrolyte)

molecules vs ions

* molecules and atoms typically do not have a charge
* ions have a positive or negative charge because they are extra greedy with electrons

monatomic cations

* positive ions formed from a single atom


* example: sodium ion (Na+).

naming monatomic cations

* Just the names of the element
* Groups 1 & 2 (+1 & +2)
* Add roman numerals to tell you the charge for transition metals (groups 3-12)

Na+ name

Sodium

* monatomic cation

K+ name

Potassium

* monatomic cation

Mn^3+ name

Manganese (III)

* monatomic cation, transition metal

common cations

* Column 1: 1+ charge
* Column 2: 2+ charge
* Zn (Zinc): 2 electrons
* Ag (Silver): 1+ charge
* (NH4)^+ (Ammonium): exception, polyatomic cation

common anion

Hydroxide anion: HO-

If you had 2 ammonium molecules…

(NH4)^+ sub 2

monatomic anion

* negative ions formed from a single atom
* example: (I^-), iodine ion, iodide

naming monatomic anions

* add -ide to element name

F- name

Fluoride

H- name

Hydride

O^2- name

Oxide

N^3- name

Nitride

polyatomic ions

* formed when atoms of different elements combine and gain or lose electrons
* this group of atoms has a charge and acts as a single unit
* most are grouped with oxygen and have a negative charge
* examples:
* sulfate (SO4^2-)
* nitrate (NO3^-)
* carbonate (CO3^2-)

naming polyatomic ions

* add -ate if there is more of the second element (3)
* add -ite if there is less of the second element (2)
* add per- if there is even more of the second element (4)
* add hypo- if there is even less of the second element (1)
* ensure you balance charges

NO2^- name

nitrite

NO3^- name

nitrate

SO4^2- name

sulfate

SO3^2- name

sulfite

ClO4^- name

* halogen
* perchlorate

ClO3^- name

chlorate

ClO2^- name

chlorite

ClO^- name

hypochlorite

Find the formula for Sodium Sulfide

Na^+, S^2-

* you need 2 Na^+ to balance 1 S^2-, you want the charges to be equal

Na2S

Find the formula for Iron (II) Oxide

Fe^2+, O^2-

FeO

binary molecular compounds

don’t begin with a metal like ionic compounds

systematic naming for binary molecular compounds

* the first word: the name of the first element in the formula, with a Greek prefix if necessary
* the second word: Greek prefix, stem of the name of the 2nd element, and the suffix -ide

Greek prefixes

* 2: di-
* 3: tri-
* 4: tetra-
* 5: penta-
* 6: hexa-
* 7: hepta-
* 8: octa-

P4O6 is a…

binary molecular compound, we know by the fact that there are numbers next to both elements

P4O6 name

tetraphosphorous hexoxide

common diatomic acids

* HF, HCl, HBr, HI, HCN, H2S
* In water, acid form b/c of hydro-

naming diatomic acids

* hydro- element, add -ic & acid

HF

Hydrofluoric acid

HCl

Hydrochloric acid

HBr

Hydrobromic acid

HI

Hydroiodic acid

HCN

Hydrocyanic acid

H2S

Hydrosulfiric acid

Oxoacids

polyatomic ions with Hydrogen

naming oxoacids

* if polyatomic ion ends in -ate, change to -ic and add acid
* if polyatomic ion ends in -ite, change to -ous and add acid

HNO3 name

Nitrate → Nitric acid

HNO2 name

Nitrite → Nitrous acid

H2SO4 name

Sulfate → Sulfuric acid

H2SO3 name

Sulfite → Sulfurous acid