2. Chemistry Background Information!
Our classroom set of textbooks – Pearson
Chapter 2
Define all bold words/concepts vocabulary in
sections 2.1-2.3!
Your definitions need to be complete enough
that another person (not in class) can
understand!
3. I recommend you title the entry as the chapter and section you
are working in (helps with clarity and continuity)!
Mass
Volume
Extensive Properties
Intensive Properties
Etc.
Again, your definitions need to be complete enough that another
person (not in class) can understand!
4. Section 2.3 – Elements and Compounds…1st look at
the PERIODIC TABLE! (Time to color!!!)
Handout: Periodic Table of Elements
Periods (1-7)
Groups or Families (1-18)
Metals/Nonmetals/Metalloids
Transition Metals; Post Transition Metals;
Lanthanides & Actinides
Family Names
Oxidation Number – [Charge on an ion due to difference
between protons and electrons.]
Known Oxidation States: (memorize)
5.
6. Chemical nomenclature falls into 4 categories for us
in this class:
1. Ionic Compounds - metal bonding to a nonmetal
via an ionic bond…transfer of electrons
2. Covalent Molecules - nonmetal bonding to
another nonmetal via a covalent bond…sharing
electrons
3. Acids – Hydrogen bonded to a nonmetal or
polyatomic ion (formula starts with ‘H’)
4. Organic Chemistry – typically carbon-based
molecules (very brief for this level of chem)
8. Use your notes from yesterday and your periodic table:
1. List two intensive and two extensive properties of a 25 g sample of
water.
2. A student from another class states that gold is dense and that
density is an extensive property. Is this correct or incorrect? Justify
your answer with a short statement.
3. What method of separation is most effective for separating the
following mixtures:
a. A mixture of rubbing alcohol dissolved in water.
b. A mixture of dirt in water.
4. Identify the period, family and most probable oxidation state for
each of the following elements:
He; K; Ag; P; Br; Sn; Mg
9. Binary Ionic Nomenclature
Practice Problems – On Canvas…Unit 0 & 1…Early Nomenclature
More Practice…worksheet!
Google Slides – Binary Molecular Nomenclature
10. Nomenclature Flowchart
Practice Problems – Binary Ionic…tile
activity again but now you need to name the
compounds!
Nomenclature Flowchart and practice
problems worksheet.
11. Quiz on Unit 1 and the initial periodic table!
12.
13. NaI _____________
Potassium oxide_________
Al(NO3)3 ______________
Zinc phosphate ________
AuCl3 _____________________
Iron (II) sulfide _____________
Cr2(SO4)3 ___________________
Cobalt (I) phosphate __________
14. Covalent bonding = nonmetal to nonmetal (Nonmetals
form anions and two negative particles will not ‘stick’ to each other so we
cannot use charges here!)
Nonmetals share electrons…so the nomenclature
system simply uses prefixes to note the formula of
the molecule.
Prefixes:
Note:
avoid two vowels if possible
Mono= 1 Hexa = 6
Di = 2 Hept = 7
Tri = 3 Oct = 8
Tetra = 4 None = 9
Penta = 5 Deca = 10
15. Two types of acids:
Binary…H and another nonmetal
Hydro(root of nonmetal)ic acid
Oxyacids…involves a polyatomic containing
oxygen!
17. Two types of acids:
Binary…H and another nonmetal
Hydro(root of nonmetal)ic acid
Oxyacids…involves a polyatomic containing oxygen!
Look at the polyatomic suffix…
-ate becomes –ic
-ite becomes –ous
Simply add acid at the end!
Examples: H2SO4 vs H2SO3
18. Unfortunately, there are almost always some
exceptions to the rules we learn!
Examples: (all have an asterisk on the back
of your periodic table)
19. 1. How many significant figures are in each of the
following:
a) 0.006 050 b) 40,500 c) 1.200 x 106 d) 10,001,000
2. Round this value off to four sig figs and write your final
answer in scientific notation: 4,059,401
3. Which of the following names or formulas is/are
incorrect? Correct the error(s) if present.
a) Pb(NO3)2 = lead nitrate
b) cadmium(II) sulfide = CdSO4
20. More practice than you could ever need
worksheet (cont.)
Bottom and back of the Flowchart Handout!
Our quiz tomorrow:
NOMENCLATURE...ALL WE HAVE COVERED TO
DATE!
Significant Figures.
Material (limited) from the textbook (sections 2.1-2.3).
22. Units of metric measurement – Table 3.2 p. 75 (record
this in your notes…or the chart at the front of the class)
Textbook – p. 84 …read section 3.3
Examples on the board of the technique…
Sorry but you MUST show all work for credit!
NO EXCEPTIONS! Ratio method will yield correct answers
but you will not get credit as your units are obscured.
Work problems #74-75 on p. 96 (show all work and pay
attention to sig figs)
23. Showing all work…normal conversions…
Using scientific notation to your advantage…
Short-cut from one metric unit to another…
Converting square or cube conversions factors…
Known conversions…
1 cm3 = 1 mL
24. Convert to the desired unit…showing all work!
1) 45.5 inches to feet
2) 0.550 gal to ounces (4 qt = 1 gal; 2 pints = 1 qt; 16 oz = 1
pt)
3) 14,259 feet to miles