Chem Chapter 3 & Nomeclature Flashcards
1
Q
What are elements composed of according to Dalton’s Atomic Theory?
A
Tiny, indivisible, indestructible particles called atoms*
This concept emphasizes the fundamental nature of atoms in forming elements.
2
Q
How do atoms of a given element compare to each other?
A
They are identical (same size, mass, and chemical properties)*
This principle suggests uniformity among atoms of the same element.
3
Q
How do atoms of one element differ from atoms of another element?
A
Atoms of one element are different from atoms of all other elements*
This underscores the distinct nature of different elements.
4
Q
What are compounds composed of according to Dalton’s Atomic Theory?
A
Atoms of more than one element*
Compounds consist of different types of atoms bonded together.
5
Q
In any given compound, what is true about the types of atoms present?
A
The same types of atoms are always present in the same relative numbers*
This indicates a fixed ratio of atoms in a specific compound.
6
Q
What can atoms do in terms of forming compounds?
A
Combine in more than one ratio to form different compounds*
This highlights the versatility of atomic combinations in chemistry.
7
Q
True or False: Dalton’s first two proposals were later shown to be incorrect.
A
True*
Subsequent scientific advancements revealed limitations in Dalton’s initial theories.
8
Q
What does the law of definite composition state?
A
Different samples of a given compound always contain the same elements in the same mass ratio.
Proposed by Dalton.
9
Q
What is an example of the law of definite composition?
A
Water (H2O) always contains hydrogen and oxygen in a 2:1 mass ratio.
Regardless of the source, the ratio remains constant.
10
Q
What does the law of multiple proportions state?
A
Different compounds made up of the same elements differ in the number of each kind of atom.
Proposed by Dalton.
11
Q
Give an example of the law of multiple proportions.
A
Carbon monoxide (CO) and carbon dioxide (CO2) contain carbon and oxygen in different ratios: 1:1 and 1:2, respectively.
This illustrates how the same elements can combine in different ways.
12
Q
What model of the atom did JJ Thomson propose in 1903?
A
Plum-pudding or raisin pudding model
This model suggested that atoms are divisible, containing electrons and protons.
13
Q
What significant discovery did JJ Thomson make regarding atoms?
A
Identified the electron and the proton
This discovery proved the divisibility of atoms.
14
Q
What experiment did JJ Thomson conduct to support his atomic model?
A
Cathode Ray Experiment
This experiment was crucial in the identification of the electron.
15
Q
What is the name of the model proposed by Ernest Rutherford?
A
Rutherford’s model of the atom
This model introduced the concept of a nucleus at the center of the atom.
16
Q
What are the three types of radioactivity?
A
- Alpha (α) rays (positively charged)
- Beta (β) rays (negative charges)
- Gamma (γ) rays (no charge)
These types of radiation were identified as part of Rutherford’s research.
17
Q
What was the purpose of the Alpha Particle Scattering Experiment conducted in 1906?
A
To study the angles at which alpha particles were deflected by gold foil
This experiment was crucial in developing Rutherford’s atomic model.
18
Q
What did Rutherford’s data from the gold foil experiment reveal?
A
It was inconsistent with the plum pudding model of the atom
This inconsistency led to the development of a new atomic model.
19
Q
In what year did Rutherford discover protons?
A
1919
This discovery was a significant advancement in atomic theory.
20
Q
What did Rutherford discover about the structure of the atom?
A
There is a positively charged nucleus inside an atom
This finding was a key element of his atomic model.
21
Q
Who discovered the neutron?
A
James Chadwick in 1932
Chadwick’s discovery was a significant advancement in understanding atomic structure.
22
Q
What is the charge of an electron?
A
-1
The negative charge of an electron is fundamental to its interactions with protons.
23
Q
What is the charge of a proton?
A
+1
The positive charge of a proton is crucial for forming atomic nuclei.
24
Q
What is the charge of a neutron?
A
0
Neutrons are neutral particles and play a key role in stabilizing atomic nuclei.
25
Which subatomic particle is the smallest?
Electron
## Footnote
Electrons are significantly smaller than protons and neutrons.
26
Which subatomic particles are located inside the nucleus?
Proton and neutron
## Footnote
The nucleus is the dense center of an atom, containing protons and neutrons.
27
Where is the electron located in an atom?
Outside the nucleus
## Footnote
Electrons exist in orbitals surrounding the nucleus.
28
What does amu stand for?
Atomic mass unit
## Footnote
amu is a standard unit of mass that quantifies mass on an atomic or molecular scale.
29
Fill in the blank: The neutron is the _______ subatomic particle.
largest
## Footnote
Neutrons have a greater mass compared to protons and electrons.
30
What is the structure of an atom?
An atom consists of a nucleus surrounded by electrons.
31
What is the composition of the nucleus of an atom?
The nucleus contains all the positive charge and nearly all the mass of an atom.
32
What is the charge of an atom?
All atoms are neutral.
33
What must be true for an atom to be electrically neutral?
The number of electrons must equal the number of protons.
34
What occupies the space outside the nucleus of an atom?
Electrons.
35
True or False: An atom is mostly solid.
False.
36
Fill in the blank: An atom is mostly _______.
empty space.
37
What is the nature of the nucleus in terms of density?
The nucleus is extremely small and extremely dense.
38
How does the total charge of electrons compare to the positive charge of the nucleus?
The total charge of electrons exactly balances the positive charge of the nucleus.
39
What is the definition of Mass Number (A)?
Mass Number (A) = # protons AND # neutrons in the nucleus
## Footnote
Mass number is important in determining isotopes of an element.
40
Is the Mass Number found on the periodic table?
No
## Footnote
The mass number is not listed on the periodic table.
41
What is the definition of Atomic Number (Z)?
Atomic Number (Z) = # protons
## Footnote
The atomic number is essential for identifying elements.
42
How can Atomic Number (Z) be used in relation to atoms?
It can be used to identify elements and is equal to the # of protons in a neutral atom
## Footnote
The atomic number helps determine the element's position in the periodic table.
43
How is the periodic table arranged?
According to Atomic Number (Z)
## Footnote
Each element is placed based on its atomic number.
44
Do all elements have the same Atomic Number (Z)?
No, each element has a different Z
## Footnote
This uniqueness is what distinguishes one element from another.
45
Fill in the blank: The Mass Number (A) is important in _______.
[isotopes]
## Footnote
Isotopes are variants of elements with different mass numbers.
46
Provide an example of Atomic Notation.
Examples include ¹²C for Carbon-12 and ¹⁴C for Carbon-14
## Footnote
These notations indicate the mass number and the element symbol.
47
What is atomic notation?
A system for representing the composition of an atom
## Footnote
Atomic notation includes the mass number and atomic number.
48
In atomic notation, where is the mass number located?
On top
## Footnote
The mass number represents the total number of protons and neutrons in the nucleus.
49
In atomic notation, where is the atomic number located?
On bottom
## Footnote
The atomic number indicates the number of protons in the atom.
50
Fill in the blank: In atomic notation, the _______ is on top and the atomic number is on bottom.
mass number
51
True or False: The mass number represents only the number of protons in an atom.
False
## Footnote
The mass number includes both protons and neutrons.
52
What are isotopes?
Atoms of the same element having different masses (different # of neutrons)
## Footnote
Isotopes can differ in stability.
53
How does the mass number of an element change?
It varies as the number of neutrons in the nucleus varies
## Footnote
The mass number is the sum of protons and neutrons.
54
What is the stable isotope of hydrogen with one proton and no neutron called?
Protium
## Footnote
Protium is the most abundant hydrogen isotope.
55
What is the stable isotope of hydrogen with one proton and one neutron called?
Deuterium
## Footnote
Deuterium is often used in nuclear fusion and as a tracer in chemical reactions.
56
What is the unstable isotope of hydrogen with one proton and two neutrons called?
Tritium
## Footnote
Tritium is radioactive and used in nuclear fusion and self-luminous devices.
57
Fill in the blank: Isotopes have the same number of _______ but different numbers of neutrons.
protons
## Footnote
The number of protons defines the element.
58
What is the format for naming isotopes?
Name of the element followed with its A value
59
How is Carbon-14 represented in terms of protons and neutrons?
Z = 6 protons, A = 14, Neutrons = 8
60
How is Carbon-12 represented in terms of protons and neutrons?
Z = 6 protons, A = 12, Neutrons = 6
61
Fill in the blank: The number of neutrons in an isotope can be calculated using the formula A - Z. For Carbon-14, this equals _______.
8
62
True or False: Both Carbon-14 and Carbon-12 have the same number of protons.
True
63
What is the value of A for Carbon-14?
14
64
What is the value of A for Carbon-12?
12
65
What are compounds?
Contain more than one type of atom
66
How many types of compounds will we learn to name?
3 types:
* Binary Molecular Compounds
* Ionic Compounds
* Acids
67
What must be recognized to know which rules of naming to apply?
The type of compound
68
What does 'binary' mean in the context of binary molecular compounds?
2
69
What do binary molecular compounds contain?
2 elements only
70
Is hydrogen a metal or non-metal?
Non-metal
71
What types of elements are involved in binary molecular compounds?
Nonmetal + Nonmetal or Nonmetal + Metalloid
72
Which of the following are molecular? NaCl, XeF4, H2O, Fe2O
XeF4, H2O
73
What is the first word in the naming of binary molecular compounds?
Name of the element appearing first in the formula, includes a prefix to indicate the number of atoms of this element in the molecule
74
What is the second word in the naming of binary molecular compounds?
Name of the element appearing second, changed to end in '-ide', and includes a prefix to indicate the number of atoms of this element in the molecule
75
What are Greek prefixes used for in binary molecular compounds?
To indicate the number of atoms of each element in the compound
76
What is the Greek prefix for one atom?
mono-
77
What is the Greek prefix for two atoms?
di-
78
What is the Greek prefix for three atoms?
tri-
79
What is the Greek prefix for four atoms?
tetra-
80
What is the Greek prefix for five atoms?
penta-
81
What is the Greek prefix for six atoms?
hexa-
82
What is the Greek prefix for seven atoms?
hepta-
83
What is the Greek prefix for eight atoms?
octa-
84
What is the Greek prefix for nine atoms?
nona-
85
What is the Greek prefix for ten atoms?
deca-
86
How is N2O3 named?
dinitrogen trioxide
87
How is P2O5 named?
diphosphorus pentoxide
88
What is the correct name for CCl4?
Carbon tetrachloride
## Footnote
The prefix 'mono-' is usually omitted for the first element.
89
What is the correct name for CO2?
Carbon dioxide
## Footnote
The prefix 'mono-' is omitted, and the final 'o' of the prefix is dropped when the element name begins with a vowel.
90
What is the correct name for P2O5?
Diphosphorous pentoxide
## Footnote
The prefix 'penta-' denotes five oxygen atoms.
91
What is the correct name for P4O10?
Tetraphosphorous decoxide
## Footnote
'Deca-' indicates ten oxygen atoms.
92
What is the correct name for BF3?
Boron trifluoride
## Footnote
The prefix 'tri-' indicates three fluorine atoms.
93
What is the correct name for H2O?
Dihydrogen monoxide
## Footnote
'Di-' indicates two hydrogen atoms.
94
What is the correct name for NO?
Nitrogen monoxide
## Footnote
'Mono-' indicates one oxygen atom.
95
What is the correct name for S4N4?
Tetrasulfur tetranitride
## Footnote
'Tetra-' indicates four sulfur and four nitrogen atoms.
96
What is the correct name for SF6?
Sulfur hexafluoride
## Footnote
'Hexa-' indicates six fluorine atoms.
97
What is the correct name for CO?
Carbon monoxide
## Footnote
'Mono-' indicates one oxygen atom.
98
What is the correct name for SO3?
Sulfur trioxide
## Footnote
'Tri-' indicates three oxygen atoms.
99
What is an ion?
An atom that loses or gains electrons, resulting in an unequal number of protons and electrons
100
What charge does a particle have if it gains electrons?
Negative (–)
101
What charge does a particle have if it loses electrons?
Positive (+)
102
What is a charged particle called?
Ion
103
Should Greek prefixes be used with ionic compounds?
No
104
What is a monoatomic ion?
An ion formed when a single atom gains or loses one or more electrons
105
What is the charge on an ion sometimes called?
Oxidation Number or Oxidation State
106
What is the oxidation number of Na+?
+1
107
What is the oxidation number of Ca2+?
+2
108
What is the oxidation number of Fe3+?
+3
109
What is the oxidation number of F-?
-1
110
What is the oxidation number of S2-?
-2
111
What is the oxidation number of N3-?
-3
112
What is the chemical formula and oxidation number of Nitrate?
NO3⁻, -1
113
What is the chemical formula and oxidation number of Sulfate?
SO4²⁻, -2
114
What is the chemical formula and oxidation number of Phosphate?
PO4³⁻, -3
115
What is the chemical formula and oxidation number of Ammonium?
NH4⁺, +1
116
What is the chemical formula and oxidation number of Acetate?
C2H3O2⁻, -1
117
What is the chemical formula and oxidation number of Hydroxide?
OH⁻, -1
118
What is the chemical formula and oxidation number of Chlorate?
ClO3⁻, -1
119
What is the chemical formula and oxidation number of Nitrite?
NO2⁻, -1
120
What is the chemical formula and oxidation number of Hydrogen sulfate?
HSO4⁻, -1
121
What is the chemical formula and oxidation number of Sulfite?
SO3²⁻, -2
122
What is the chemical formula and oxidation number of Carbonate?
CO3²⁻, -2
123
What is the chemical formula and oxidation number of Hydrogen Carbonate?
HCO3⁻, -1
124
What is a Polyatomic ion?
A charged species containing more than one atom
125
What is the tendency of Group 1A elements on the periodic table with regard to electrons?
Tendency to lose 1 electron (+)
126
What is the tendency of Group 2A elements on the periodic table with regard to electrons?
Tendency to lose 2 electrons (+2)
127
What charge does aluminum (Group 3A) typically have?
+3
128
What are the possible charges for carbon (Group 4A)?
+4 or -4
129
What is the tendency of Group 7A elements regarding electrons?
Tendency to gain 1 electron (-)
130
What is the tendency of Group 6A elements regarding electrons?
Tendency to gain 2 electrons (-2)
131
What is the tendency of Group 5A elements regarding electrons?
Tendency to gain 3 electrons (-3)
132
What are cations?
Positive ions formed from loss of 1 or more electrons
133
What is the relationship between protons and electrons in cations?
Protons outnumber electrons (p+ > e-)
134
Which type of elements typically form cations?
Metals
135
How are cations named?
Element name + ion
136
What is the name of the ion formed from sodium?
Na+ sodium ion
137
What is the name of the ion formed from aluminum?
Al3+ aluminum ion
138
What is the charge of calcium ion?
Ca2+
139
What is the charge of potassium ion?
K+
140
Which transition metal has a +3 charge and how is it named?
Fe3+ 'iron three ion' or iron(III) ion
141
What is the name for Fe2+?
'iron two ion' or iron(II) ion
142
How is the charge indicated for transition metals with multiple charges?
A Roman numeral in parentheses is used to indicate charge
143
Which elements can form multiple charges along with transition metals?
Tin (Sn) and Lead (Pb)
144
What is the charge of Zinc?
Zinc (Zn) will always be 2+
145
What is the charge of Silver?
Silver (Ag) will always be +1
146
What is the charge of Cadmium?
Cadmium (Cd) will always be +2
147
What are anions?
Negative ions formed from the gain of 1 or more electrons
## Footnote
Anions have fewer protons than electrons.
148
What is the relationship between protons and electrons in anions?
#p+ < #e-
## Footnote
This indicates that there are more electrons than protons.
149
Which types of elements typically form anions?
Nonmetals
## Footnote
Nonmetals are more likely to gain electrons to form anions.
150
How are anions named?
Named from root of atom + -ide ion
## Footnote
For example, the oxide ion is derived from the root of oxygen.
151
What is the formula for the oxide ion?
O2-
## Footnote
The oxide ion is a common example of an anion.
152
What is the formula for the fluoride ion?
F-
## Footnote
The fluoride ion is derived from fluorine.
153
What is the formula for the nitride ion?
N3-
## Footnote
The nitride ion is derived from nitrogen.
154
What is the formula for the sulfide ion?
S2-
## Footnote
The sulfide ion is derived from sulfur.
155
What is the formula for the chloride ion?
Cl-
## Footnote
The chloride ion is derived from chlorine.
156
What is the formula for the bromide ion?
Br-
## Footnote
The bromide ion is derived from bromine.
157
What is the formula for the iodide ion?
I-
## Footnote
The iodide ion is derived from iodine.
158
Fill in the blank: The anion formed from phosphorus is called _______.
phosphide ion
## Footnote
Phosphide is the anion derived from phosphorus.
159
Fill in the blank: The anion formed from sulfur is called _______.
sulfide ion
## Footnote
Sulfide is the anion derived from sulfur.
160
What are Ionic Compounds made of?
Cations and anions
161
What must be the net charge of Ionic Compounds?
Zero
162
What is the structure of Ionic Compounds?
Large 3-D arrays of (+) and (-) ions
163
What types of elements typically make up Ionic Compounds?
Metal and nonmetal
164
Can cations or anions in Ionic Compounds be polyatomic ions?
Yes
165
What do Ionic Compounds conduct when melted or dissolved in water?
Electricity
166
What are Ionic Compounds also known as when they conduct electricity?
Electrolytes
167
What do the subscripts in a compound formula indicate?
Number of ions
168
Give an example of an ionic compound made from a metal and a nonmetal.
NaCl
169
Give an example of an ionic compound made from a metal and a polyatomic ion.
CaSO4
170
Give an example of an ionic compound made from a polyatomic ion and a nonmetal.
NH4Cl
171
Give an example of an ionic compound made from two polyatomic ions.
NH4NO3
172
What is the first step in writing Ionic Compound formulas?
Put (+) and (-) ions together in a ratio so that total (+) equals total (-)
## Footnote
This ensures the overall charge of the compound is neutral.
173
What must you know to write Ionic Compound formulas?
The charge of each ion
## Footnote
Knowing the charges allows for correct balancing of the compound.
174
What is the formula for the compound formed from Na+ and Cl-?
NaCl
## Footnote
The charges of +1 and -1 balance each other out.
175
How many Cl- ions are needed to balance Mg2+?
2
## Footnote
The formula is MgCl2, since +2 from Mg requires two -1 from Cl.
176
What is the formula for the compound formed from Al3+ and Cl-?
AlCl3
## Footnote
Three -1 Cl ions are needed to balance the +3 from Al.
177
How many Na+ ions are needed to balance S2-?
2
## Footnote
The formula is Na2S, as two +1 Na ions are needed for the -2 charge of S.
178
What is the lowest common denominator for Ca2+ and P3-?
6
## Footnote
This is used to balance the charges for the formula Ca3P2.
179
What is the formula for the compound formed from Ca2+ and P3-?
Ca3P2
## Footnote
The balancing requires three +2 Ca ions and two -3 P ions.
180
True or False: Charges are included in the formulas of ionic compounds.
False
## Footnote
The final compound formulas do not display the individual charges.
181
What are compounds containing polyatomic ions based on?
The charges of the ions
182
What must you know to work with polyatomic ions?
The charges and formulas of polyatomic ions
183
How do you indicate multiple polyatomic ions in a formula?
Enclose the polyatomic ion in parentheses and use subscript outside ()
184
Fill in the blank: Na+ SO42- requires ______ Na+ to balance the charge.
2
185
What is the formula for the compound formed from Na+ and SO42-?
Na2SO4
186
Fill in the blank: Mg2+ requires ______ of OH- to balance the charge.
2
187
What is the formula for the compound formed from Mg2+ and OH-?
Mg(OH)2
188
What is the formula for the compound formed from NH4+ and NO3-?
NH4NO3
189
What is the formula for the compound formed from Al3+ and OH-?
Al(OH)3
190
What is the formula for the compound formed from Al3+ and SO42-?
Al2(SO4)3
191
What is the formula for the compound formed from NH4+ and PO43-?
(NH4)3PO4
192
What is the formula for the compound formed from NH4+ and CO32-?
(NH4)2CO3
193
What is the first step in naming ionic compounds?
Name cation (first ion in formula)
## Footnote
The cation is the positively charged ion in the compound.
194
What is the second step in naming ionic compounds?
Name anion (2nd ion in formula)
## Footnote
The anion is the negatively charged ion in the compound.
195
How is CaCl2 named?
calcium chloride
## Footnote
This compound consists of calcium cations and chloride anions.
196
How is KI named?
potassium iodide
## Footnote
This compound consists of potassium cations and iodide anions.
197
How is NH4OH named?
ammonium hydroxide
## Footnote
This compound consists of ammonium cations and hydroxide anions.
198
What is the naming convention for the first element in ionic compounds with monatomic ions?
The first element is just the element name
## Footnote
This applies to the cation in the compound.
199
What is the naming convention for the second element in ionic compounds with monatomic ions?
The second element is the element name with the ending changed to '–ide'
## Footnote
This applies to the anion in the compound.
200
How is NaCl named?
sodium chloride
## Footnote
This compound consists of sodium cations and chloride anions.
201
How is MgBr2 named?
magnesium bromide
## Footnote
This compound consists of magnesium cations and bromide anions.
202
How is Na2S named?
sodium sulfide
## Footnote
This compound consists of sodium cations and sulfide anions.
203
What is used to determine the formula of ionic compounds?
Charge on ions
## Footnote
Balancing the charges of cations and anions is essential for formula determination.
204
What is the first step in naming ions with polyatomic ions?
Name any monatomic ion just as you would normally
## Footnote
This applies similarly to monatomic ions in the compound.
205
What is the second step in naming ions with polyatomic ions?
Name the polyatomic ion
## Footnote
Polyatomic ions have specific names that need to be learned.
206
How is NaNO3 named?
sodium nitrate
## Footnote
This compound consists of sodium cations and nitrate anions.
207
How is NH4Cl named?
ammonium chloride
## Footnote
This compound consists of ammonium cations and chloride anions.
208
How is Al(OH)3 named?
aluminum hydroxide
## Footnote
This compound consists of aluminum cations and hydroxide anions.
209
How is (NH4)3PO4 named?
ammonium phosphate
## Footnote
This compound consists of ammonium cations and phosphate anions.
210
Which elements have multiple oxidation states?
Iron, copper, cobalt, mercury, tin, and lead
211
What does it mean for an element to have multiple oxidation states?
It means they form more than one cation
212
What is the formula for the iron(II) ion?
Fe2+
213
What is the formula for the iron(III) ion?
Fe3+
214
What is the name of the ion Co3+?
Cobalt(III) ion
215
What is the name of the ion Sn2+?
Tin(II) ion
216
What is the name of the ion Pb4+?
Lead(IV) ion
217
How is copper(I) chloride represented in chemical formulas?
CuCl
218
How is copper(II) chloride represented in chemical formulas?
CuCl2
219
What is the formula for lead(IV) sulfate?
Pb(SO4)2
220
True or False: Cations with multiple oxidation states do not require specification in their names.
False
