Download Part 2: Write the oxidation number for the

General Chemistry
Review Worksheet for Chapter 7
Fill in the blank.
1. Atoms with loosely held valence electrons have _____low__________ ionization energy and
____low__________ electron affinity.
2. A metal that can be drawn into a thin wire is said to be __ductile________________.
3. A metal that can be hammered into thin sheets without breaking is said to be
____malleable_________________.
4. Elements that tend to gain electrons easily are called ___nonmetals__________________.
5. An element that is considered to be unreactive because it has a filled outer energy level is
_Noble__________ _Gas________.
6. The energy needed to remove electrons from an atom is called _ionization energy ______________.
7. Elements that exist in nature as two atoms covalently bonded are called _diatomic________________.
8. Aluminum is a metallic element with 3 valence electrons. Its oxidation number is ___+3___________.
9. Elements found touching the zigzag line on the periodic table are called ____metalloids_____________.
10. Elements to the right of the zigzag line on the periodic table are called _nonmetals________________.
11. Bonding that occurs when there is a transfer of electrons is called __ionic bonding_________________.
12. The number of electrons an atom gains, loses or shares is called its __oxidation number_____________.
13. The electrons in the outermost energy level of an atom are called __Valence Electrons_______________.
Fill in the table:
Element
Sodium (Na)
Calcium (Ca)
Antimony (Sb)
Fluorine (F)
Oxygen (O)
Phosphorus (P)
Valence electrons
1
2
5
7
6
5
1. Describe the formation of a positive and negative ion.
A positive ion forms when an atom loses electrons. Metals form cations
A negative ion forms when an atom gains electrons. Nonmetal form anions
Electron dot diagrams:
Draw the dot for the following elements.
1. H
7. C
2. Rb
8. O
3. He
9. P
4. B
10. Xe
5. Mg
11. Ba
6. Se
12. As
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General Chemistry
Vocabulary
Define the following terms
1. luster - shininess
2. ductile - capable of being molded or shaped without breaking
3. malleable - Can be hammered, pressed, formed or bent into many shapes
4.
corrosion - gradual wearing away of metal due to a chemical reaction
5. Chemical bonding - force that holds atoms or ions together
6. valence electron - electrons in the outer shell
7.
ionic bonding - transferring of electrons
8.
ion - a charged atom
9. ionization energy - amount of energy used to remove an electron
10. Electron affinity - tendency of an atom to attract electron
11. electron-dot diagram - Chemical symbol for an element represents the nucleus and all the inner energy
levels of the atom, except the outermost. Dots surround the symbol to represent the valence electrons
12. diatomic element - two atoms of same element covalently bonded together
13. polyatomic ion - a group of covalently bonded atoms that acts like a single atom when combining with
other atom
14 Oxidation number - # of electrons an atom gains, loses , or shares when it forms chemical bonds.
(describes combining capacity)
Fill in the blanks
1.
2.
3.
4.
5.
6.
7.
8.
9.
A chemical bond is formed when _electrons________________ are gained, lost, or shared.
A charged particle is called an __ion_________________.
A negatively charge particle is called a(n) ____anion______________.
A positively charge particle is called a(n) ____cation_____________________.
A group of atoms that act as a single atom and that have a charge are called __polyatomic
ion_________________.
The ___valence________________ electrons are the electrons in the outer shell of an atom.
The ____oxidation number______________________ is the # of electrons an atom gains, loses , or
shares when it forms chemical bonds. (describes combining capacity)
The small number written above and to the right of the symbols is called a
____superscript__________________.
The small number written below and to the right of the symbol is called a
___subscript____________________.
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General Chemistry
10. An ionic bond forms between ____metal_____________ and __nonmetal__________________.
11. A covalent bond forms between ___nonmetal___________________ and
_nonmetal____________________.
12. When naming a compound prefixes are only used for ___covalent_____________ bonded elements.
13. The cross over method using oxidation numbers to write chemical formulas is only used for
___ionic_____________ bonded elements.
14. A metallic bond is a bond between _valence electrons_ and __positively charged metal ions_______
15. Metal are good conductors of electricity because they contain __ mobile valence electrons____.
Part 1: Please fill in the valence electron numbers for the following elements. (Use a Periodic table)
Element
Valence
Element
Valence
C
4
He
2
Mg
2
N
5
B
3
Br
7
Ba
2
Ar
8
Li
1
S
6
Part 2: Write the oxidation number for the following elements. (Use a Periodic table)
1. F ___-1_____
6. K ____+1______
2. Na ___+1_____
7. Ne _____0____
3. O ___-2_____
8. P _-3_________
4. Al __+3_______
9. Si ___+/- 4______
5. Ca ___+2______
10. N ____-3______
Part 3: Write the chemical formulas for the following elements. (Use periodic table and oxidation
table I gave you in class)
1. O and Na __Na2O_____________
11. H and SO4 __H2SO4_____________
2. Be and S ___BeS_______________
12. Al and SO4 __Al2(SO4)3__________
3. Al and Cl ___AlCl3_____________
13. Na and CO3 __Na2CO3_________
4. Ca and P ___Ca3P2_______________
14. NH4 and OH ____NH4OH___
5. C and Cl ____CCl4______________
15. H and NO3 ___HNO3____________
6. O and Al _____Al2O3___________
16. Al and PO4 ___AlPO4___________
7. Mg and Br ____MgBr2__________
17. Ca and PO4 ___Ca3(PO4)2________
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General Chemistry
8. K and S _______K2S___________
18. K and OH _____KOH___________
9. B and N _____BN_____________
19. NH4 and PO4 ___(NH4)3PO4_______
10. Be and O ____BeO______________
20. Mg and NO3 ____Mg(NO3)2______
Write the names of the following ionically bonded compounds.
1. NaF – Sodium Fluoride
2. Fe2O3 – Iron (III) Oxide
3. Al2O3 – Aluminum Oxide
4. CaO – Calcium Oxide
5. CuBr – Copper (I) Bromide
6. K2S – Potassium Sulfide
Write the formulas from the following names:
1. Iron (II) oxide - FeO
2. sodium chloride - NaCl
3. copper (I) carbonate – Cu2CO3
4. hydrogen hydroxide - HOH or H2O
5. magnesium bromide – MgBr2
6. Iron (II) fluoride – FeF2
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