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