Name:____________________
Chapter 3 Reading Guide: Molecules, Compounds, and Chemical Equations
3.1 Hydrogen, Oxygen, and Water (p. 86-88)
When hydrogen and oxygen combine to form the compound water, a dramatically
_____________________ substance results.
When two or more elements combine to form a ______________________, an entirely
______________ substance results.
In a compound, elements combine in ________________, ____________________ proportions;
in a mixture, elements can mix in ____________ proportions whatsoever.
3.2 Chemical Bonds (p. 88-90)
Compounds are composed of atoms held together by ________________________________.
Chemical bonds result from the _______________________ between charged particles (the
________________ and __________________) that compose atoms.
We can classify most chemical bonds into two types: _________________ and
_________________________.
Ionic bonds—which occur between ____________________ and ___________________—
involve the _______________________ of electrons from one atom to another.
Covalent bonds—which occur between _______________________________________—
involve the ________________________ of electrons between two atoms.
Metals have a tendency to _______________ electrons and nonmetals have a tendency to
__________________ them.
The metal atom becomes a _______________________ (a positively charged ion), and the
nonmetal becomes an _______________________ (a negatively charged ion).
Covalently bonded atoms compose a _____________________________.
We call covalently bonded molecules ________________________________________.
3.3 Representing Compounds: Chemical Formulas and Molecular Models (p. 90-93)
The quickest and easiest way to represent a compound is with its ___________________
__________________, which indicates the elements present in the compound and the relative
number of ______________ or _____________ of each.
Chemical formulas normally list the more ______________________ (or more
_____________________ charged) elements first, followed by the less _________________ (or
more _______________________ charged elelments.
Empirical formula:
Molecular Formula:
Structural Formula:
Ball-and-stick molecular model:
Space-filling molecular model:
3.4 An Atomic-Level View of Elements and Compounds (p. 93-95)
Atomic elements:
Molecular elements:
Molecular compounds:
Ionic compounds:
Formula Unit:
Polyatomic ion:
3.5 Ionic Compounds: Formulas and Names (p. 95-101)
Ionic compounds always contain ___________________________________________.
In a chemical formula, the sum of the charges of the positive ions (______________________)
must equal the ____________ of the charges of the negative ions (__________________).
The formula of an ionic compound reflects the _________________ whole-number ratio of ions.
Common names:
Systematic names:
Ionic compounds are usually composed of _________________ and _____________________.
Binary compounds:
Oxyanions:
Hydrates:
Waters of hydration:
3.6 Molecular Compounds: Formulas and Names (p. 101-105)
The formula for a molecular compound ______________________ readily be determined from
its constituent elements because the same combination of elements may form many
____________________ molecular compounds, each with a _____________________ formula.
Molecular compounds are composed of two or more _____________________.
Generally, write the name of the element with the ______________________ group number
first.
If the two elements lie in the same group, then write the element with the ________________
row number first.
Prefixes:
1=
2=
3=
4=
5=
6=
7=
8=
9=
10=
If there is only one atom of the first element in the formula, the prefix ____________ is
normally omitted.
Acids:
(aq) means _________________________________________________
Oxyacids:
3.7 Summary of Inorganic Nomenclature (p. 105-107)
3.8 Formula Mass and the Mole Concept for Compounds (p. 107-109)
Formula Mass:
Molar mass:
3.9 Composition of Compounds (p. 109-114)
Mass percent:
Mass percent composition as a conversion factor:
Conversion factors from chemical formulas:
3.10 Determining a Chemical Formula from Experimental Data (p. 114-119)
Empirical formula:
Empirical formula molar mass:
Combustion Analysis:
3.11 Writing and Balancing Chemical Equations (p. 119-123)
Chemical reaction:
Combustion reaction:
Chemical equation:
Reactants:
Products:
Balance the equation:
3.12 Organic Compounds (p. 123-126)
Organic compounds:
Hydrocarbons:
Alkanes:
Alkenes:
Alkynes:
Functional group:
Alcohols:
Family: