Study Guide Chapter 2 - Atoms, Molecules and Ions
1. Skip over 2.1-2.4
2. 2.5 atomic number, atomic mass, # of electrons, protons, neutrons
23
23 units mass, 11 units charge,
11 Na
11 protons, 23-11 or 12 neutrons, neutral atom so electrons = protons =11
22
11
Na 22 units of mass, 11 units of charge
11 protons, 22-11 or 11 neutrons, neutral atom so electrons = protons =11
These two are examples of isotopes same neutrons, different mass
22
11
Na + 22 units of mass, 11 units of charge
11 protons, 22-11 or 11 neutrons, + atom missing an electron, so electrons =
protons-1 =10
3. Covalent bonds and Ionic bonds
Covalent -atoms held together by electrons shared between two atom
Ionic atoms - held together by charge attraction between oppositely charged ions
4. The Periodic table
Vertical columns - families
Alkali metals +1
Alkaline earth metals +2
Transition metals in between
Halogens (F downward)
Nobel Gases (He downward)
Horizontal rows - periods 1 st period H and He
5. Naming compounds
A. Ionic vs covalent
B. Binary ion involving 1A,2A, Al, Ag or Zn
Cation 1 st, then anion
cation takes name of atoms
anion takes name of atom -ide
Study table 2.3 for names of various anions
do not use bi-,tri- etc, figure from 0 net charge
C. Binary compounds - other metals
Same as above, but give charge of cation with roman numeral
D. Covalent
name first element as atom, second as ion
use mono-, di-, tri-, tetra-, penta-, hexa-, hepta-, octa-, nona-, deca- etc.
Do not use mono for 1 st atom
Don’t bother for water and ammonia
Chapter 2 review - Continued
E. Acids
acid dissociates to H+ and anion -Anion is key
Anion with no oxygen add hydro to element name
Hydrochloric, hydrocyanic, etc
Anion with oxygen
Anion is -ate Use -ic for acid Sulfate, sulfuric acid
Anion is -ite Use -ous for acid nitrite, nitrous acid