Download presentation
1
Unit 4 Test Review
2
Identify the following as covalent or ionic.
water (H2O) salt (NaCl) iron (II) sulfide (FeS) calcium bromide (CaBr2) covalent ionic
3
CS2 BaI2 N2O4 PCl3 covalent ionic
Identify the following as covalent or ionic. CS2 BaI2 N2O4 PCl3 covalent ionic
4
Identify the following as covalent or ionic.
compound is a gas at room temperature compound, when melted, conducts an electric current compound is composed of a metal and a nonmetal compound is composed of a nonmetal and a nonmetal
5
What is a polyatomic ion?
An ion that contains more than 1 element
6
What is meant by binary ionic?
2 elements (metal and nonmetal) joined by ionic bonds
7
What is meant by binary molecular?
2 elements (both nonmetals) joined by covalent bonds
8
What is meant by ternary ionic?
3 elements (metal and nonmetals) joined by ionic bonds
9
What part of the atom is involved in chemical reactions?
Valence electrons
10
Why do atoms share electrons?
To gain the electron configuration of a noble gas
11
Which intermolecular attractive force is the strongest?
Hydrogen bonds
12
Why is carbon special? it has four electrons in its outermost energy level it readily bonds with other carbon atoms it can form single, double, or triple bonds with other atoms
13
What is the Octet Rule? in chemical compounds, atoms tend to have the electron configuration of a noble gas
14
What is the electron configuration of the sulfide ion (S-2)?
1s22s22p63s23p6
15
A compound that ends in -ate or -ite contains ____.
A polyatomic ion
16
How many valence electrons are transferred from the aluminum atom to oxygen in the formation of the compound aluminum oxide? 3
17
Why are metal good electrical conductors?
They have mobile electrons
18
Which elements can form diatomic molecules joined by a single covalent bond?
halogens and hydrogen
19
Which elements can form diatomic molecules joined by double covalent bonds?
oxygen
20
Which elements can form diatomic molecules joined by triple covalent bonds?
nitrogen
21
What is VESPR Theory? molecules adjust their shapes to keep valence electrons as far apart as possible
22
What is a polar molecule?
A molecule that has partial positive and negative charges
23
Which of the following covalent bonds is the most polar?
a. H—F b. H—C c. H—H d. H—N
24
What is the charge on the cation in the ionic compound magnesium chloride?
+2
25
What is the net charge of the ionic compound potassium fluoride?
26
What is the formula unit of calcium nitride?
Ca3N2
27
What is the formula for potassium sulfate
K2SO4
28
What is the formula unit for sodium sulfide?
Na2S
29
What is the name of the following compound? NaClO2
Sodium chlorite
30
Are the following pairs of elements likely to form ionic or covalent compounds?
phosphorus and sulfur magnesium and oxygen aluminum and chlorine
31
What are some properties of ionic compounds?
High melting points Metal and nonmetal Conducts electricity in solution solid
32
What is a cation? An ion with a positive charge due to loss of electrons The metal part of an ionic compound
33
What is an anion? An ion with a negative charge due to gain of electrons The nonmetal part of an ionic compound
34
Will group 6A elements gain or lose electrons when forming ions
Will group 6A elements gain or lose electrons when forming ions? How many electrons will be gained or lost? gain 2
35
What is the purpose of a Roman numeral following the name of an element?
To indicate the presence of a transition metal that can have more than one common ionic charge.
36
What ion will sulfur form?
sulfide
37
What is the formula for iron (III) oxide?
Fe2O3
38
What is the formula for phosphorus tetrachloride?
PCl4
39
What is the formula for trisulfur dioxide?
S3O2
40
Reactions between atoms involve which part of the atom?
Valence electrons
41
What is the name of the following compound? CrF3
Chromium (III) fluoride
Similar presentations
© 2024 SlidePlayer.com Inc.
All rights reserved.