CP Chem Chapter 4 Study Guide
· Review all of the following key terms related to chapter 4 (lessons 17-23):
a. Octet Rule
b. Zero-charge rule
c. Isoelectronic
d. Noble gas
e. Valence electrons
f. Anion
g. Cation
h. Monatomic ion
i. Polyatomic ion
· Review atom structure (type and charge of subatomic particles in neutral versus charged ions, what subatomic particle is lost or gained to become an ion?).
· Review the organization of the periodic table: a) general locations of the metals, nonmetals and metalloids; b) Is a period a horizontal row or a vertical column? c) Is a group a vertical column or a horizontal row?
· Review the family names for groups 1A, 2A, 7A and 8A; Group B metals
Chapter 4 Specifics
1. Lewis Dot representations are a shortcut method to represent the number of:
VALENCE or CORE electrons (Circle ONE).
** You should be able to write the Lewis Dot representation of a neutral atom, as well as its ion!
2. The number of valence electrons that a neutral atom that is a representative element has can be predicted based on its PERIOD or GROUP number (Circle ONE).
3. Going across a period, the number of core valence electrons:
Stays the same or Increases by one (CIRCLE ONE)
every time the atomic number of the element changes.
4. When a neutral atom becomes an ion:
It becomes isoelectronic with members of family ____A (group number), also known as the ______(Family name). For instance, when the element Calcium becomes an ion, it contains as many ______(what subatomic particle?) as Argon (Ar).
Elements tend to form ions so that they will contain _____ electrons (fill in how many) in their highest occupied energy level. (This is also known as the ______Rule). (Fill-in)
5. Metals form a (+)-charged ion called a ______and nonmetals form a
(-)-charged ion called an ______. (Metals are GIVERS and Nonmetals are TAKERS).
Metals form (+) ions because they GAIN or LOSE electrons (Choose ONE)
Nonmetals form (-) ions because they GAIN or LOSE electrons (Choose ONE).
6. Some ions form from a single type of atom and are called monatomic.
7. But some ions contain more than one type of atom and are combined in a specific ratio and have either a net positive charge or a net negative charge. In other words, they are _____-atomic (unscramble these letters to get the correct prefix: “yolp”).
Remember: the number of each type of atom in a combination of atoms is called the subscript. In this polyatomic ion, how many P and O atoms are in combination with each other?
PO4 3-
Which of the following diagrams correctly represents it?
**Memorize the polyatomic ions (formulas and charges) listed on page 111 in your etextbook and these two additional polyatomic ions:
Cyanide CN1-
Acetate C2H3O21-
8. The charge of a monatomic ion for an element that is in an “A” group on the periodic table can be predicted as follows:
Group 1A: + 1
Group 2A: + ____ (fill-in number)
Group 3A: + ____ (Fill-in number)
Group 5A: - 3 (Group # - 8)
Group 6A: - ____ (fill in number)
Group 7A: - ____ (fill-in number)
9. Some metals form more than one charge. These elements are known as the group ____ (fill-in letter) or the transition metals. Look on the periodic table below and identify the location of the transition metals:
Some of the more common transition metals we come in contact with are:
Cu: Copper
___: Iron (What is the chemical abbreviation for iron?)
Sn: ______(What is the name of this element?)
10. Ionic compounds consist of a metal and a nonmetal/metalloid (Circle ONE).
Ionic compounds are electrically neutral- in other words, they obey the ____ (fill in; what number?) Charge Rule: the number of positive charges equals the number of negative charges.
Remember: In an ionic compound’s formula, we write the symbol for the Cation followed by the symbol for the anion.
Remember: In an ionic compound’s name, the name of the cation preceeds the name of the anion. Some cations are polyatomic and
some anions are polyatomic. Polyatomic ions travel as a GROUP!
Remember: We always write an ionic formula as the simplest whole number ratio AND if there is only one of an ion, we don’t need to write 1”- it is understood (NaCl NOT Na1Cl1).
**You should be able to 1) recognize the cation and its charge from a formula (reverse the criss-cross rule) and 2) be able to write a formula if given the cation and the anion or the elements (forward criss-cross rule) and 3) write the name of a compound if given its formula.
**Go over the specific naming rules for Group A and Group B metals!
**Do the practice naming and formula writing worksheet!! Answers will be posted on L. O’Reilly Teacher Webpage under CP Chem tab/chapter 4 resources.
11. When does an ionic bond form? An ionic bond forms when there is an attraction between ____-charged ions and _____-charged ions; the attractive forces are strong because ONE or MORE THAN ONE (circle one) of the opposite charges is/are ATTRACTED or REPELLED (circle one) to each other.
Remember- this unit was about MOVING electrons! Metals give nonmetals their Electrons!