ElementsSimplest form of matter that retains its
propertiesKnown by common names and abbreviations
Compounds• Made of two or more elements chemically
combined in definite proportions– Law of definite proportions: pure compounds always
have the same ratio of elements H2O = 2 Hydrogen for every 1 Oxygen
(Chemical Formula)
• Two Types:①Ionic Compounds②Molecular Compounds (Molecules)
Paper Clip Lab
• Elements vs. Compounds vs. Mixtures
Ionic Compounds• Made up of Ions: Charged atoms
Cations: Positive chargeEx: Na (Atom) Na+ (Cation)
11 protons (+) 11 protons (+)11 electrons (-) 10 electrons (-)
Anions: Negative ChargeEx: Cl (Atom) Cl- (Anion)
17 protons (+) 17 protons (+)17 electrons (-) 18 electrons (-)
Ions Vs. Atoms
• There are chemical differences between ions and atoms….
Na+ vs. NaUniversity of Nottingham http://www.periodicvideos.com/videos/011.htm
Army disposing of Na http://www.youtube.com/watch?v=HY7mTCMvpEM
Ions and Periodic Table
2 Types of Ions• Monatomic Ions: Single elements
Na+ Zn2+ Br- Cl- O2-
• Polyatomic Ions: Two or more different elementsNH4
+ CO32- CrO4
2- Cr2O72-
See your handout for the list
Ionic Compounds• Cation + Anion = Ionic Compound
Na+ + Cl- = NaCl Ni2+ + 2(IO3
-) = Ni(IO3)2
The positive cation and negative anion attract each other to form neutral compound
Usually solids with high melting and boiling points
Usually form from metal and nonmetal
Naming Ionic Compounds• Binary Ionic Compounds: 2 different ions
K+ + Cl- KCl
①Cation is ALWAYS first ②Net charge is ALWAYS zero③Cation name doesn’t change.④Change anion name by using the “ide” ending
KCl = Potassium Chloride
Naming Ionic Compounds①NaCl =
②MgO =
③KF =
④CaBr2 =
Naming Ionic Compounds• Some elements (called transition metals) can form
more than one type of positive ion. The positive charge of the ion is then indicated by a roman numeral.
Fe2+ = iron(II) Fe3+ = iron(III)Cu+ = copper(I)Cu2+ = copper(II)
Naming Ionic Compounds①CuBr =
②PbCl2 =
③FeN =
④CrP =
Naming Ionic Compounds• Polyatomic ions:– Have special names– Are treated as one unit (they don’t break apart)– Most end in “ite” or “ate”
Ba2+ + CO32- BaCO3
Barium Carbonate Barium carbonate
Naming Ionic Compounds①FePO4 =
②CaCrO4 =
③NaNO3
④SnSO4
Naming Ionic Compounds①Zinc chloride =
②Iron(II) oxide =
③Tin(IV) sulfite =
④Aluminum hypochlorite =
Molecule• Neutral groups of non-metallic elements joined by
covalent bonds (electrons are shared) NO IONS – NO CHARGE
• Low melting and boiling points– Liquids and gases at room temperature
• Ex: H2O, CO2, O2, and Cl2
Naming Molecular Compounds• Name them in the order that they appear– Element with more positive chemical nature will be first• “More positive” means towards the left side of periodic table
– Second element: drop the last syllable and add “ide”
• If there is more than one atom of an element, add a numerical prefix:
CO = Carbon MonoxideCO2 = Carbon Dioxide
N2O3 = Dinitrogen Trioxide
Naming Molecular Compounds①Dinitrogen monoxide =
②Silicon carbide =
③N2O4 =
④Cl2O8 =
Naming Acids and Bases• Acid: Produces hydrogen ion (H+) when dissolved in
H2O– Formula = (H+ to balance the anion charge) + (anion)
Ex: H2S HCl
• Base: Produces hydroxide ion (OH-) when dissolved in H2O• Formula= cation metal + hydroxide ion to balance charge
Ex: NaOH Al(OH)3
Naming Acids• When the anion….– Ends with “ide”:
acid name begins with “hydro”the suffix “ic” is added to the anion
Ex: HCl = hydrochloric acid- Ends with “ite”:
the suffix “ous” is added to the anionEx: H2SO3 = sulfurous acid
- Ends with “ate”:the suffix “ic” is added to the anion
Ex: HNO3 = nitric acid
Naming Bases• Named the same way as ionic compounds– Al(OH)3 = aluminum hydroxide
– Fe(OH)3 = iron(III) hydroxide
Naming Acids and Bases①H2CO3 =
②Phosphoric acid =
③KOH =
④Strontium hydroxide =