Exam 2 - PREP Flashcards
topics: GASES, ATOMS AND ELEMENTS, MOLECULES COMPOUNDS AND NOMENCLATURE
1
Q
2.1) A _________ is a neutral species that is comprised of two or more atoms that are linked together.
A
Molecule
2
Q
P2Cl5
sub2
sub5
is a type of Binary covalent compound because both phosphorus and chlorine are nonmetals. By using the rules for naming this compound the name is
A
diphosphorus pentachloride
3
Q
MgClO3
sub3
is an NONBINARY compound because three elements are present in the compound. In this case, recognize the POLYATOMIC ion ClO3-
sub 3 with 1 negative charge.
ClO3- is bound to a metal. the rule is to _____________
therefore the name is __________.
A
The rule for naming compounds with polyatomic atoms attached is
1. keep the same order
2. use the polyatomic name properly (don’t forget the ate, ite, per, hypo)
the name is
magnesium chlorate
4
Q
During chemical reactions- metals tend to __________
electrons. nonmetals tend to ________ electrons. Noble gases tend to __________ electrons due to their complete outer energy level.
A
lose electrons (cation),
gain electrons (anions),
neither gain nor loose
5
Q
Naming compounds by their formulas
Na2S (sub2)
Pb3N2 (sub3sub2)
explain each
A
Both are binary compounds, therefore you must add the ide at suffix to the last element.
Na2S is Sodium sulfide
Lead is a transition metal and REQIURES roman numberals to express the type of charge it has. Cross down method can be done it reverse to find the ORIGINAL charges before they synthesized. Therefore Pb’s charge was 2 and N charge was 3. Nitrogen must have an ide at the end because its binary compound.
Pb3N2 is Lead (III) Nitride
6
Q
2.1) The rows of the periodic table are called: ___________
A
PeRiods
7
Q
Whats the formula for potassium Nitrate?
explain
A
Potassium nitrate intells K and Nitrogen polyatomic compound. Therefore the rules is for naming a nonbinary compound must be applied.
KNO3 (sub3)
8
Q
The _______ ________ is the same for all atoms of an element. While isotopes is a species of an element with different # of neutrons.
A
Atomic number
9
Q
Name the compound SF6
A
Sulfur hexafluoride
it’s a BINARY compound. keeps the ide.
It’s a covelant compound because both are NONmetals. therefore to write symbols correctly add the “honorifics” numerical prefixes
hexa hepta mono etc
hexa is 6.
10
Q
because the most active metals react with water to form bases, they’re called ________ metals. As you move to the right of the periodic table, the base forming properties ________ and the __________ properties increase.
A
alkali metals
decreases
acid forming
11
Q
Whats the formula for Sodium sulfide?
A
Na2S
sodium sulfide is made of sodium Na and Sulfur S. they’re a metal and nonmetal. therefore the naming convention is to use their electric charges and cross or reverse cross method. the cross method will give you the correct numver of atoms.
Original is Na1 S2
cross down Na2S
12
Q
The elements in the first 2 groups are light metals, the metals toward the center are __________ metals.
A
heavy
13
Q
Whats the formula for Aluminum Chloride?
A
AlCl3
binary compounds are cross up or cross down method iot cancel the charges. Chlorine is -1 Aluminum is +3 so it has to be AlCl3 to
14
Q
Periodic table charge patterns start
Grp1 ____
Grp2 ____
Grp3-12____
Grp13_____
Grp14_____
Grp15____
Grp16____
Grp17____
Grp18____
A
1 +1 alkali
2 +2 alkali earth
3-12 varies
13 +3
14 0
15 -3
16 -2
17 -1 halogens
18 0 noble gases
15
Q
2.1) The columns of the periodic table are called: ____________
A
Groups
16
Q
In general, on the periodic table:
Metallic properties and acid forming properties are greatest on the _______ side and decrease as you move right.
Nonmetallic properties and base-forming properties are greatest on the _________ side of the table and decrease as you move left.
A
left (group 1 and 2)
right (group 18,27)
17
Q
GAS PROPERTIES
As the temperature of a gas is increased, its __________ energy is increased. thereby increasing random motion.
A
kintetic
18
Q
Group 17 on the periodic table is called: _______________
A
halogens or (halides organic chem)
19
Q
What’s the definition of an acid?
A
“a water solution that has an excess of hydrogen ions”
20
Q
an acid turns litmus paper pink or red, has a sour taste, and _________ __________ to form ________.
A
neutralizes bases
salts
21
Q
definition of a metal:
An element whose oxide combines with ______ to form a base; can also refer to an element that readily ______ electrons and becomes a cation.
A
water
loses
22
Q
Group 1 on the periodic table is called: ________________
A
Alkaline Metals
23
Q
definition of a nonmetal:
an element whose oxide reacts with _______ to form an acid; can also refer to an element that takes on an ________ and acquires a negative charge anion.
A
water
electron
24
Q
What group is the Alkaline Earth metals?
A
Group 2
25
plasma is very hot ionized _______.
gases
26
What group are the halides in?
Group 17
27
a chemical reaction is a __________ _________. the four basic types are combination (synthesis), decomposition (analysis), single replacement or single displacement, and double replacement or double displacement.
chemical change or transformation
28
What group are the noble gasses?
Group 18
29
Ions are defined as,
a atom or group of combined atoms that carry one or more electric charges
30
Name some elements in group 18:
Ne (neon)
Rn (Radon)
He (helium)
Og (Ogganeeson)
A (argon)
K (Krypton)
31
FORMULA WRITING RULES:
Binary compounds containing a metal with only one charge possibility (Li+1) + nonmetal element
Binary compounds containing a metal element that has more than one charge possibily (ie Fe) + nonmetal element
Binary COVALENT compounds containing two nonmetal elements rules....
Rule 1. write down the elemental symbols
2. cross subscripts to balance the charges use "Cross down method"
balance charges to make the resulting overall compound neutral
(AlCl3) (metal with 1 charge possible and non metal)
metal with more that one possible example Iron (III) Oxide.
for binary COVALENT (sharing electron) rules are 1. write down the elemental symbol
2. use the prefixes (di,hept,pent,etc) and write the subscript for each element. (ex sulfur hexafluoride bc sulfur is group 16 fluoride 17)
32
FORMULA WRITING RULES:
NONBINARY compounds ionic compound containing atleast three elements
1. write down the elemental symbols or polyatomic ion formulas (ie NH3 ammonia)
2. use subscripts to balance the charges of of the ions. include parantheses when necessary for multiple molecules.
ie ammonium phosphate is (NH4)3PO4
33
Name the two groups that compose the periodic table:
Metals and Non-Metals
34
35
2.1) True/False: Hydrogen can be a Metal and Non-metal?
True
36
2.1) What are metaloids?
any element that's directly adjacent to the zigzag line. The metaloids are transition metals whose properties are less predictable than other elements.
37
Definition of Atomic Mass
A weighted average of the mass of all the isotopes (species of an atom with varying # of neutrons in the nucleus) naturally occurring.
38
How do you calculate the Atomic Mass of an element?
Give a formula
(Mass of Isotope(a)(Abundance of a) + (Mass of Isotope(b)(Abundance of b) + (Mass of Isotope(c)(Abundance of c) + (Mass of Isotope(d)(Abundance of d)...etc
You take the different known species of an element,
convert the abundance percentage to decimal (multiply by 100)
then multiply the decimal of its abundance together with their mass,
then divide by the number of species you have.
39
What is the atomic mass calculation based on?
Their natural abundance and the mass of each isotope added.
40
Calculate the Atomic Mass of Hydrogen.
H is point 1.008 amu
1H 99.9885 % abundance (1neutron 1 proton) & 1.0078 amu
2H 0.0114 % abundance (2 neutrons 1 proton) & 2.0141 amu
3H 0.0001 % abundance (3 neutrons 1 proton) & 3.0160 amu
Final answer: 1.0079126... rounded it's 1.008amu
Work:
(0.999885)(1.0078amu) + (0.000114)(2.0141amu) + (.000001)(3.0160amu) =
(1.00768amu) + (0.0002296amu) + (0.000003016amu) =
= 1.0079126...
41
X , the symbol of an element is determined by Z. Z is the number of _____________.
protons
42
The Mass Number represents _______________ While the
_______________ represents the number of protons in an element. And the Atomic Mass represents the weighted average of the number of naturally occurring _____________.
the sum of Protons and Neutrons in an element.
The Atomic Number (Z).
Isotopes
43
Where is the atomic number located on the periodic table?
Each element has their atomic number located in the right corner. ie the 1 for H is in the right corner of the box.
44
Calculate the Atomic Mass of Oxygen
45
The difference between Atomic Weight and Atomic Mass?
Atomic Mass is the calculation of a SINGLE isotope's mass.
Atomic Weight is the average of all the isotopes and their natural abundance.
46
The difference between Atomic Mass and Mass Number?
Atomic mass is the weighted average of masses of the naturally occuring isotopes of a specifies. It's the average mass of the atoms of an element.
47
Alkali metals are __________ reactive.
1A Groups of elements that are highly reactive
48
Akaline Earth metals are __________ reactive.
2A Groups of elements that are fairly reactive
49
What's an Anion?
An electrically negative charged atom
50
What's a Cation?
An electrically positive charged atom
51
"Oxygen" Dr. Cotton is refering to
O2 (g)
52
"Oxygen atom" Dr. Cotton is refering to
O
53
"Everything on the periodic table is a _____________ with few exceptions.
mono-atomic solid
54
Write the natural formula and state for the following:
Oxygen
Sulfur
Phosphorus
Mercury
Bromine
Oxygen is O2 (gas)
Sulfur is S8 (solid)
Phosphorus is P4 (solid)
Mercury is Hg (liquid)
Bromine is Br2(liquid)
55
Atomic Number (Z) is
The number of protons in an atom's nucleus.
56
Define atomic theory
a theory stating that all matter is composed of tiny particles called atoms.
57
From memory, how does group 1-2, and group 13-17 form ions according to Dr. Cotton?
Group 1 +/-?
Group 2 +/-?
Group 13* +/-?
Group 14* +/-?
Group 15 +/-?
Group 16 +/-?
Group 17 +/-?
*state the special cases too
By looking at the periodic table and knowing what groups are stable and which are not
Group 1 always froms plus 1 cations +1
Group 2 always forms plus 2 cations +2
Group 13 B/Al forms plus 3 cations* +3
Group 14 Carbon and Silicon does not form (for our purposes)* NEUTRAL STATE (consider it 0 for our purposes right now)
Group 15 forms minus 3 anions -3
Group 16 forms minus 2 anions -2
Group 17 forms minus 1 anions -1
58
All unpredictable species form __________.
and give an example.
cations positive ion
example, IRON Fe can form Fe2+ or Fe3+
59
NOMENCLATURE: for a ___________ is to have the ions name + "ion"
give an example
Predictable Cation.
Naming a positively charged atom (Cation) is the atom name + "ion" a suffix.
example:
Na+ Sodium Ion
Ca+2 Calcium Ion
Mg+2 Magnesium Ion
etc
60
NOMENCLATURE: for a _______________ naming convention is to use Atom name + Roman Numeral + "ion" in order to let people know which species an atom is.
give an example
Unpredictable cations
example Iron is Fe
Fe+2 = Iron(II) Ion
Fe+3 = Iron(III) Ion
61
NOMENCLATURE: For a ________________ the naming convention is to use the atom root + "ide"
give an example
Anion
O2- = Oxide
N3- = Nitride
62
Carbon is a metal or non-metal?
non-metal
63
Mercury is a metal or non-metal?
metal
64
B, Si, Ge, As, Sb, Te, and At are metals, non metals, or metalloids?
metalloids
65
The ____________ is the number of protons in the nucleus of an atom, and is denoted as Z. The number of protons in the nucleus of an atom is the defining trait of an element: Its value determines the identity of the element.
Atomic Number
(def. from ext lesson)
66
The ____________ the sum of the number of protons and neutrons in an atom, and it is denoted as A (and A = #protons + #neutrons). Atoms of the same element may have different ____________.
mass numbers
67
Atoms of an element with different numbers of neutrons (or different mass numbers) are called _____________. The symbol for an ______________ of an element (X) is written by placing the mass number as a superscript and the atomic number as a subscript to the left of the element symbol as shown below.
isotopes
68
The _______________ of an element is the weighted, average mass of all the isotopes present in a naturally occurring sample of that element.
atomic mass
69
2.2 True of False? the suffix "ide" will always refer to a monatomic anion
True
70
What is the convention for naming Ionic Compounds per Dr. Cotton?
with example
Take the Cation name - "Ion" then add the Anion element at the end.
ex. Sodium Chloride
Sodium Ion - Ion + Chloride
71
How do you name the Ionic Compound Fe3+ and O2-
Iron(III) Oxide
72
How would you right the name of the Ionic Compound Ca and Fl?
Ca is a cation(2+) and Fluoride(-) is an anion
CaF2
73
EXPLAIN Why there are 2 Fluoride atoms in the Ionic Compound CaF2??
Ca is a Cation with charge 2+ (group2) and Fluoride is an Anion with charge -1(group17). In order to get an overall neutral charge for the compound the COMBINED CHARGES MUST CANCEL OUT.
therefore, the LCD of 2 and 1 is 2. 2 Fluorine atoms must attach to 1 Ca atom so the charges 2(pos)+2(neg)=0.
74
What are the 7 strong acids?
HCl
HBr
HI
HNO3
H2SO4
HClO4
HClO3
Hydrochloric acid
Hydrobromic acid
Hydroiodic acid
Nitric acid
Sulfuric acid
Perchloric acid
Chrloric acid
75
What are the individual charges of the Ionic Compound Fe2O3
The Ionic Compound is Iron(III) Oxide
Using the cross down method to formulate the compound's correct number of atoms (as per their charges), the individual charges for Fe was positive 3(per III), the charge for Oxygen is negative 2(group16)
76
What's the formula for Oxide?
Why?
O2 (O subscript 2)
The reason is being the naming convention is to specify "ide" of a negative Oxygen atom.
77
Why do we use roman numerals to express the charge number on transition metals?
The roman numerals represent the positive charge values of unpredicatable elements. This needs to be specified in roman numbers each time, because the charge number is not predictable when it reacts with different atoms. Unlike other atoms who always react to loose or gain electrons predictably i.e O2 always O2.
78
List the 4 transition metals that are not written with roman numerals because they develop a predictable cation formula
__________ +1
__________ +2
__________ +2
__________ +2
Silver ion Ag+1
Nickel ion Ni+2
Zinc Ion Zn+2
Cadmium ion Cd+2
79
Write the name for the Formula:
CrCl2
explain the charges.
Chromium(II) Chloride
the charges need to be so that the compound is overall neutral compound,
Therefore, Chloride (two atoms of chloride) each with a charge of negative -1 means it's overall negative charge is -2. Chromium needs to be able to cancel out -2 charge. Therefore, it's cation charge can be predicted as II. Hence Chromium II.
80
Name the Compound
Mn2O3
(3 subscript, 2 subscript)
Manganese(III) Oxide
3 Oxygen atoms means the total charge is 3(-2) = -6. Because O is in Gr16. Therefore, the Mn needs to be able to cancel out the -6 with +6. The Mn has 2 atoms. 2(3) = 6. Therefore the Cation Mn has a positive charge of 3- (III) must be expressed in roman numerals.
81
You should always reduce your formulas to the lowest whole number ratio.
Mg2+S-2
What would it reduce to?
MgS
divide by 2.
82
Should you indicate the charges in your answers for products?
NEVER. The value for charges of compounds should be understood (implied).
83
Write the formula of
Lead (IV) Dioxide
PbO2
(subscript2)
84
You use roman numerals for transition metals and _______ transition metals to indicate the charges because they're unpredictable.
post transition metals.
85
Name
CoN2
(subscript 2)
Cobalt (VI) Nitride
N brings a Charge of 3*2=-6 therefore for the net charge of the compound to be neutral you must have +6. 1 cobalt cation must bring +6 charge.
86
True or False
To indicate a negative charge on Bromine it's fine to write minus 3.
False, write 3 minus.
The number is written first, then the + or -. The opposite of an exponent.
Br3-
87
True/False Polyatomic ions are molecules (multiple atoms of an element bonded together).
True
88
Metalloids
Elements that fall along the boundary between the metals and the nonmetals in the periodic table; their properties are intermediate betwen those of metals and those of nonmetals.
example
they are shiny (metals)
and brittle (nonmetals)
89
"_________ tend to loose electrons in chemical reactions. They are found at the left side and center of the periodic table."
Metals
90
"A compound formed from two or more nonmetals. These compounds have distinct molecules as their simplest identifiable units."
Molecular Compound
91
"___________ two or more atoms joined in a specific arrangement by chemical bonds and is the smallest identifiable unit of a __________ compound."
Molecule
Molecular
92
"____________ are Elements that tend to gain electrons in chemical reactions. They are found at the upper right side of the periodic table."
Non metals
93
"___________ ions are ions composed of a group of atoms with an overall charge."
Polyatomic
94
Give an example of a polyatomic ion
NO3 (subscript 3)
95
(2.2)
True/False
One can calculate/predict the charges of a Monoatomic ions, while with Polyatomic ions you cannot predict or figure out.
True
96
NH4+ and NH3+
subscript 4
subscript 3
Ammonium and Ammonia
97
-OH or OH-
Hydroxide
98
C2H3O2-
subscript2
subcscript3
subscript2
Acetate
99
NO3-
subscript 3
Nitrate
100
Nitrate
NOH3-
101
SO4-2
subscript 4
Sulfate
102
PO43-
subscript 4
Phosphate
103
CO32-
subscript3
Carbonate
104
NO2-
subscript2
Nitrite
105
SO32-
subscript3
Sulfite
106
PO33-
subscript3
Phosphite
107
ClO3-
subscript3
Chlorate
108
ClO2-
subscript2
Chlorite
109
ClO4-
subscript 4
ClO-
subscript is 1 (implied)
perchlorate
110
ClO-
subscript is 1 (implied)
hypochlorite
111
Bro4-
sub4
Bro3-
sub3
Bro2-
sub2
Bro-
sub1implied
Peribromate
Bromate
Bromite
Hypobromite
112
IO4-
sub4
IO3-
sub3
IO2-
sub2
IO-
sub1implied
Periodate
Iodate
Iodite
hypoiodate
113
prefixes and suffixes
hypo _______
per ________
______ mite
______mate
______ ate
below/sub/least
indicates hyper or highest
small tiny
friend, counterpart
passionate/full of
114
Molecular/Covalent compounds have _________ bonds. While Ionic compounds have _________ bonds.
Covalent
Ionic
115
Binary compounds = _________ elements
Nonbinary Compounds = _____________ elements
two elements for binary
more than 2 elements for nonbinary
116
Ionic compounds contain two elements: one ______ one _______.
metal (anion)
nonmetal (cation)
117
if two or more polyatomic ions are needed to balance the charge, ________ are used around the polyatomic ion. For instance, the compound Fe(OH)2 has parentheses around the OH group and a subscript of 2 following. This is because there are two hydroxide ions (OH-) in the formula. Without the __________, we would have FeOH2 which is incorrect.
Parentheses
118
There must be three or more elements in the formula in order for a compound to be classified as ____________.
nonbinary
119
When naming Nonbinary Ionic Compounds the what do you do step by step?
The cation is named first followed by the anion. The word ion is omitted, and use roman numerals to express the charge of a metal that varies.
120
Is Ba(OH)2
a. barium dihydroxide
b. barium hydroxide
b. barium hydroxide.
For ionic compounds we don't use numbered prefixes~
121
The _______ ending on the name of an ion means it is an anion or a negatively charged ion or non-metals. _______ is used as a suffix at the end of the name of an atom when any non-metal is present singly and bears a negative charge.
"Ide"
as in Nitride
Oxide
Fluoride
Sulfide
Root + "ide"
122
_____________ are made up of nonmetallic elements or nonmetallic elements and ___________.
Molecular Compounds
Metalloids
123
Molecular compounds do not contain ______. They are instead made up of discrete units called molecules.
ions
124
A molecule is a neutral species that is made up of two or more _______ that share electrons.
atoms
125
Binary, Nonbinary, and acids are the 3 ___________ for compounds.
molecular categories
126
Acids are divided into two groups: ______________.
binary acids and oxyacids.
127
Is potassium fluoride and sulfur dioxide pairs of binary molecular compounds? Explain why or why not.
No, they're not pairs of molecular compounds because the compounds are ionic. Ionic compounds are only formed by the transfer of electrons between the potassium and fluoride atoms.
128
Acids are -
compounds that form H3O+ when reacting with water. Must have an H+ Ion in the molecule it combined with.
129
Is N2O3 a binary molecular compound?
Why or why not?
Yes, Dinitrogen trioxide (N2O3) is a binary molecular compound because the elements bonded together with nitrogen dioxide with nitrogen (NO2) oxide (NO)
130
a molecular compound are made from only non-metal elements and metalloids. (past the transition metals). give some examples:
CO2
N2O5
H2O
PO3
131
whats the difference between an ionic compound and a molecular compound?
Ionic compounds are made from a metal and non metal. Plus, there are polyatomic ions involved form./
132
HCl
Hydrochloric acid
133
HBr
Hydrobromic acid
134
HI
Hydroiodic acid
135
HF
Hydrofluoric acid
136
List the 7 strong acids
HCl Hydrochloric acid
HBr - HydroBromic acid
HI - HydroIodic acid
137
Which of the following is NOT a molecular compound?
A) GeCl4
B) NH4Br
C) PCl3
B) NH4Br8
138
Naming Convention
Ate Ions become ic acids
ite ions become _______ acids
"ous" suffix
ex: nitrate = nitric
139
Why isn't NH4Br a molecular compound?
Because NH4Br is ionic. the Cation ammonium does not share its electrons but gains one and therefore its not a moleculre.
140
Whats the formula for bromic acid?
HBro3
H+BrO3-
"taking the bromate ion and adding a hydrogen."
141
HBrO is what acid?
hypobromous acid
142
A Molecure is made up of two or more atoms that ________ an electron.
share
143
_______ molecular compounds are made up of two nonmetallic elements.
binary
144
Binary molecular compounds use numeric prefixes to indicate the numbers of atoms of the two elements that share ___________ with a compound.
electrons
145
List the Numeric prefixes up to 10:
1 ______
2 ______
3 ______
4 ______
5 ______
5 _______
6 _______
7 _______
8 _______
9 ______
10 _____
mono
di
tri
tetre
penta
hexa
hepta
octa
nona
deca
146
Sulfurous acids would have a different suffix instead of ous. What is the suffix?
"ite" based on the naming convention.
"Sulfite" become ous in order to indicate how many hydrogens come about from the reaction.
147
What is the chemical formula for Dihydrogen Phosphite?
H2PO3-
148
How do you determine the name of a chemical when given just the formula?
1st determine the elements involved using their symbols. Then identify the prefixes and use the numbers that they represent as subscripts in the formula. For example, is PCl5 was given you would see P has no subscript but Cl does.
Therefore the name is Phosphorus "penta"chloride.
149
What's the chemical formula for
Iron (III) sulfite trihydrate
*trihyrdrate is when you add the dot and put 3molecules of hydrogen in the formula.
Fe2(SO3)3 * 3H2O
150
Important exceptions to naming conventions with numeric prefixes are the:
water H2O
NH3 ammonia
PH3 ________
phosphine
151
Give the chemical formula or the name for the following
152
Which of the following compounds are nonbinary?
A) Acetic acid
B) HCHO, formaldehyde
C) ethanol,C2H5OH
D) All of the above are nonbinary compounds
D) all of the above are nonbinary compounds
153
heptahydrate means what?
To put a dot and then write the chemical formula 7H2O next to your compound. (basically means add water)
154
(2.4) What is the correct name for H2SO3?
A) hyposulfurous acid
B) sulfurous acid
B) Sulfurous acid
155
What is the correct name for SCI4?
A) monosulfur tetrachloride?
B) sulfur chloride
C) sulfur tetrachloride
C) sulfur tetrachloride
156
name of the compound
Cl2O7
Dichlorine heptoxide
157
again... Whats a binary compound? Give an example:
a chemical made of two different elements.
NaCl2 sodium chloride
158
What is the correct formula for hydrosulfuric acid?
A) H2SO4
B) H2S
C) H2SO3
D) H2S(aq)
D) H2S(aq)
the aq indicates is important bc its a binary compound.
159
Chemical formula for iodic acid is:
A) HI(aq)
B) HIO3
C) HIO
B) HIO3
not a binary so no need for aq
160
Which of the following is an oxyacid?
A) nitrous acid
B) hypochlorous acid
C) carbonic acid
D) All of the above
D) All of the above
161
What is the name of the acid that contains the following polyatomic group: BrO4-
A) hydrobromic acid
B) bromous acid
C) perbromic acid
C) perbromic acid
162
(2.3HW) Which of the following is a binary ionic compound?
a) NaOH
b) FeCl2
c) CaSO4
d) Br2
B) FeCl2
163
What is the change on tin in the following compound?
Sn(SO4)2
A) 0
B) 2+
C) 4+
D) 2-
C) 4+
164
What is the formula of the compound formed when oxygen and aluminum combine?
A) Al2O3
B) AlO2
C) AlO
A) Al2O3
(cross products, process of elimination bc u know 2 needs to be there)
165
What is the formula of the compound formed when magnesium ions and nitride ions combine?
A) MgN
B) Mg3N
C) Mg3N2
C) Mg3N2
166
Which of the following pairs has the correct name for given formula?
A) K2O - dipotassium monoxide
B) PCl3 - phosphorus chloride
C) PbCO3 - lead (II) carbonate
C) PbCO3 - lead (II) carbonate
167
What is the correct formula for the compound that forms between calcium ions and hydroxide ions?
A) CaOH2
B) Ca2OH
C) Ca(OH)
D) none of the above
D) none of the above
168
What is the correct formula for barium hypochlorite?
A) Ba(ClO)2
B) Ba(ClO)
C) Ba(ClO3)2
A) Ba(ClO)2
169
The chemical formula for manganese (II) oxide is:
A) Mn2O3
B) Mn3O2
C) Mn3O
A) Mn2O3
170
Which of the compounds below is not a nonbinary ionic compound?
A) AgNO3
B) NH4Cl
C) CaCO3
D) All of the above are nonbinary ionic compounds!
D) All of the above are nonbinary ionic compounds
171
What is the name of the following compound
NaHSO4?
A) sodium hydrogen sulfate
B) sodium hydrosulfate
C) sodium hydrogen sulfite
D) sodium sulfate
172
What statements are true?
1) Bromine is more likely to form a cation than an anion
2) Be is more likely to form a cation than anion
3) For a particular element, a cation will have more electrons that an anion
4) In case of the main group elements, their atoms gain or lose electrons in order to have the same number of electrons as their nearest noble gas
2) and 4)
173
Which of the following elements is likely to form an anion?
A) H
B) Mg
C) Se
D) Fe
C) Se
Selenium
174
The charge on an aluminum ion having 10 electrons is:
A) 3+
B) 3-
C) 2+
D) 2-
A) 3+
175
When tellurium forms an ion which of the following would be the likely ion that would form?
A) Te4-
B) Te6+
C) Te2-
D) none of the above
C) Te2-
176
If an atom of bromine gains electrons so that it has a total of 36 electrons, what is the charge on the ion that is formed?
A) 1
B) 1-
C)0
D) none of the above
B) 1-
177
Identify the metal that is likely to have variable charges.
A) Zinc
B) Copper
C) Aluminum
D) Barium
B) Copper
178
Which of the following is a polyatomic ion?
A) NO2
B) SO3
C) NH4+
sub4
D) Pb4+
C) NH4+
179
Select all the statements that are correct?
1) the formula for the hydrogen carbonate ion is HCO32
sub 3
2)The name of the O2- formula is oxide ion
3) The formula of the Mercury (I) ion is Hg+
4) The nitrate ion is an oxyanion
2) the name of the O2 formula is oxide ion
4) The nitrate ion is an oxyanion
180
What is the name of the following ion: HSO4-
sub4
A) hydrosulfate ion
B) hydrosulfite ion
C) hydrogen sulfate ion
D) hydrogen sulfite ion
C) hydrogen sulfate ion
181
Which of the following is written correctly as the name of the following ion: CO2+
A) copper Ion
B) Cobalt ion
C) Copper (II) ion
D) Cobalt (II) ion
D) Cobalt (II) ion
182
Which of the following, if any, is a binary ionic compound?
A) F2
B) KOH
C) AgCl
D) NaClO
C) AgCl
183
What is the charge on lead in PbSO4?
2+
184
Predict the charge on the silver in the following compound:
Ag2CrO4
A)1+
B)2+
C)0
A) 1+
185
Which of the following pairs has the correct formula-name match?
A) K2O
B) CuCO3
D) AgNO3
B) CuCO3- Copper (II) carbonate
186
What is the correct formula for the compound that forms from the combination of aluminum and oxygen?
A) Al2O3
B)AlO
C)AlO2
A)Al2O3
187
What is the correct formula for the compound that forms between lithium ions and hydroxide ions?
A) LiOH2
B) LiOH
C) Li(OH)2
D) none of the above
B) LiOH
188
Give the correct name for the compound with the following formula: PbCO3
A)lead carbonate
B) lead II carbonate
B) lead II carbonate
189
What is the correct formula for barium hypochlorite?
Ba(ClO2)
190
What is the correct name for SCl4?
A) monosulfur tetrachloride
B)sulfur tetrachloride
C) tetrasulfur chloride
B) sulfur tetrachloride
191
The chemical formula for manganese (III) oxide is
'
A) Mn2O3
B) Mn3O2
C) Mn3O
A) Mn2O3
192
Consider an atom of an element X, if this atom gain three electron, which of the statements below would most likely be true for this element?
A) The element is a metal and it forms a cation with a 3+ charge.
B) The element is a nonmetal and it forms an anion with a 3 -charge
C) The element is a metal and it forms an ion with a 3 charge
B) The element is a nonmetal and it forms an anion with a 3-charge
193
Which of the following elements is likely to form a cation?
A) lithium
B) tellurium
C) iodine
D) argon
A) litium because its inn Group 1 where 1 gains.
194
How many electrons must a strontium atom gain or lose to form the strontium ion?
A) lose 5
B) gain 2
C) lose 2
C) lose 2
195
What is the charge on an aluminum ion that has 10 electrons?
3+
196
When Tellurium forms an ion which of the following would be the likely formula for the ion?
A) Te4-
B) Te6+
C) Te2-
C) Te2-
197
If radium were to form an ion, what is the common charge that it is likely to have?
A) 2+
B) 2-
A) 2+
198
When iodine forms an ion, how many electrons do you expect the ion to have?
A)52
B)53
C)54
C)54
199
Which of the following is a polyatomic ion?
A) N2
B)Hg2 2+
sub2 charge 2+
C) NH3
C) NH3
200
What is the name of the following ion: Pb4+?
Lead (V) ion
201
What is the name of the following ion
N3-
Nitride Ion
202
Which is the correct formula for the carbonate ion?
A)CO3-
B) CO3 2-
sub 3 charge -2
B) CO3 2-
202
203
Choose the correct statement as True or False.
1) The cation that forms from calcium ion needs a roman numeral in the name so that the reader knows what is the charge on the ion
2) The cation that forms from calcium ion does not need a roman numeral in the name because there is only one possible cation charge variation
3) Since calcium is in group two of the periodic table, its charge can not be predicted.
4) since calcium is in group 2 of the periodic table, its charge cannot be predicted.
2,3,4 are true
203
204
Which of the following elements exist as a diatomic molecule?
A) Sulfur
B) Hydrogen
C)Neon
B) Hydrogen
204
Name some elements in group 18:
Ne (neon)
Rn (Radon)
He (helium)
Og (Ogganeeson)
A (argon)
K (Krypton)
205
Which of the following properties is true for metals?
A) shiny
B) electroconductive
C) malleable
D) brittle
E) A-C
E) A-C
206
What is the other name for group 2?
Alkaline earth metals
207
What is the average atomic mass of chlorine if the mass of one isotope is 34.97 amu and has a percent abundance of 75.77%. The other isotope has a mass of 36.97 amu and has a percent abundance of 24.23%.
35.45 amu
208
Which of the following elements are main group elements?
A) Selenium and Iron
B) Lithium and Lead
C) Silver and Tin
B) Lithium and Lead
209
Name 5 transition metals
Ti - titanium
V vanadium
Cr chronium
Mn Manganese
Fe Iron
Co Cobalt
Ni Nickel
210
True or False?
1) Silicon and arsenic are shiny but brittle
2) selenium is a nonmetal
3) iron and silver are transition metals
4) Gold and lead are post transition metals
1,2,3 are true
211
Name 5 Metalloids
Boron B
Silicon Si
Arsenic As
Tellurium Te
Astatine At
Germanium Ge
Antimony Sb
(these are all the metalloids)
212
