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CHEMISTRY 107: FUNDAMENTALS > MOD 5-3 MAJOR CHECK & 1-2MINOR > Flashcards

MOD 5-3 MAJOR CHECK & 1-2MINOR Flashcards

revuew cards for mods 5--3 especially quizzes and calculations from textbook!!!

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1
Q

2.1) A _________ is a neutral species that is comprised of two or more atoms that are linked together.

A

Molecule

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2
Q

What Three different kinds of equations are used to represent chemical reactions in aqueous solution: __________________

A

Molecular equation
Ionic
and Net Ionic

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3
Q

A ___________________ is a chemical equation showing the complete, neutral formulas for every species in a reaction.

A

molecular equation

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4
Q

Classify the following reaction
A) decomposition
B) gas forming
C) combination
D) percipitation

A

B) gas forming

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5
Q

A reaction in which two aqueous salt solutions combine to form an insoluble salt is called, ___________________

A

precipitation reaction

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6
Q

Is this a single replacement reaction? why?

A

yes,

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7
Q

________________ Ions that are the same on both sides of an ionic equation

A

spectator ions

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8
Q

___________ An equation that shows the formulas of all the species involved in a chemical reaction

A

molecular equation

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9
Q

An equation that shows all the ions as well as other species involved in a chemical reaction

A

ionic equation

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10
Q

An equation that shows only the species that are involved in the change that occurs during a chemical reaction

A

net ionic equation

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11
Q

In a single- replacement reaction, sodium metal reacts with water to form aqueous sodium hydroxide as one of the products. Which equation below correctly represents this reaction?

A

C)

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12
Q

which of the following two solutions will result in the formation of a precipitate when they are mixed?

A

A)

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13
Q

The following repersents a ______ ______ equation.

A

net ionic equation

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14
Q

K is an example of a _______ ion.

A

spectator ion

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15
Q

What will be the net ionic equation for this reaction?

A

B)

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16
Q

What is the identity of the gas that is produced when a lithium sulfite solution and hydrochloric acid are mixed?

A) sulfur dioxiode
B) sulfur trioxide
C) chlorine

A

A) sulfur dioxide

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17
Q

What is evidence of a chemical reaction?
A) a color change during a reaction
B) formation of precipitate
C) the sublimation of a solid to a gas
D) Both A and B

A

D) Both A and D

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18
Q

The ______ quantity must always be the same on both sides of a balanced chemical equation?

A

The number of each type of atom

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19
Q

What are the coefficients, written from left to right that will correctly balance the following equation?

A

2, 9, 6, 8

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20
Q
A

2

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21
Q

This reaction is a good example of a ________ reaction:
A) combustion
B) decomposition

A

B) decomposition reaction

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22
Q

When C3H8 burns completely in oxygen, what are the likely products?
_____________ and _____________

A

CO2 and H2O

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23
Q

True/False
An example of a correctly balanced reaction of solid copper reacting with solid sulfur to form solid copper(I) sulfide.

A

False

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24
Q

True/False
An example of a correctly balanced reaction of solid copper reacting with solid sulfur to form solid copper(I) sulfide.

A

False

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25
Q

If solid lithium hydrogen carbonate decomposes upon heating to form solid lithium oxide, gaseous carbon dioxide, and liquid water, which reaction below is the complete and balanced molecular equation for the process?

A

Option 4 with the LIzO(solid) at the end and the 2 Li at the beginning

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26
Q

An ______________________ (or complete ____________) is a chemical equation showing all of the species as they are actually present in the solution. When a soluble ionic compound is placed in water, the cations and anions dissociate (that is, separate from each other) resulting in just ions in solution.

A

ionic equation

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27
Q

So, when writing _____________, only strong acids and soluble ionic compounds (that is, strong electrolytes) are separated into ions because that is how they exist in the solution. All other species will remain as they appear in the molecular equation. The following is the __________ for the molecular equation for the reaction between silver nitrate and magnesium chloride shown above.

A

ionic equation

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28
Q

A _____ ____________ ___________ is an equation showing only the species that actually participate in the reaction. Ions that are the same on both sides of the equation are called spectator ions because they are not participating in the reaction.

A

net ionic equation

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29
Q

To balance an equation (in order to show the reality of chemical reactions where matter must be conserved) we insert ___________ not subscripts in front of the chemical formulas as needed inorder to make the number of each type of atom in the reactants equal to the number of each type of atom in the products.
Multiply the ____________ by the subscript of an atom in order to determine the number of atoms.

A

coefficients

WHY: Change only the coefficients because changing the subscripts changes the KINDS of molecules not the number.

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30
Q

The following equation shows the chemical reaction of methane gas, reacting with oxygen, to form carbon dioxide and water, such as on a kitchen stove.
WRITE A BALANCED EQUATION

A
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31
Q

In order for this equation to be balanced, the coefficient x must be
a) 3
b) 6
c) 9
d) 12

A

6
because the Ox on the reactant side has 18 atoms. on the product side its 8. the O2’s coefficient would be 6. bc 6*2=12 plus 6 from the CHO molecule. thus getting 18 atoms

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32
Q

Write a balanced equation for the reaction of solid aluminum with aqueous sulfuric acid to form aqueous aluminum sulfate and hydrogen gas.

A

steps 1) write the correct chemical compounds

2) balance the free elements last. Sulfur and oxygen occur in only one compound on each side of the equation so balance them first.
3) balance polyatomic ions as one unit. therefore put 3 infront of SO and 3 infront of HSO
4) balance Al next. 2 Al atoms on the right side of the equation, place a 2 infront of Al on the left.
5) balance H next. 6 H on the left side. put 3 on the left

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33
Q

Write a balanced equation for the reaction of aqueous lead (II) acetate with aqueous potassium iodide to form solid lead (II) iodide and aqueous potassium acetate

A

here’s each step in the equation

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34
Q

Chemistry is the science that studies the connections between the properties of _________ and the particles that compose that __________.

A

matter
matter

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35
Q

To convert mass to moles or moles to mass, we use the mole relationship: ____ mole of a substance = molar mass of the substance.

A

1

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36
Q

To figure out the amount of each reactant or product in a reaction, we apply ____________.

A

stoichiometry

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37
Q

stoichiometry allows chemists to predict the following:

A

the amounts of products that form in a chemical reaction based on the amounts of reactants
how much of the reactants are necessary to form a given amount of a product
how much of one reactant is required to completely react with another reactant

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38
Q

The ________________ or _________________ is the reactant that is completely used up in a reaction. It is important to note that in some cases, all the reactants are completely used up. When that happens, the reactants are said to be in _____________ amounts.

A

Limiting reactant or limiting reagent

stoichiometric

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39
Q

The following rules can be applied to identify

I) If there is only one reactant (i.e. a decomposition reaction), that reactant is the limiting reactant.

II) If two or more reactants are used but quantities are provided for only one reactant, the reactant whose quantity is provided is the limiting reactant.

III) If the quantities are provided for two or more reactants, we need to calculate the quantities required and compare them with the amounts provided in order to determine which reactant is the limiting reactant.

A

the limiting reactant

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40
Q

The maximum calculated amount of product formed from the limiting reactant is called the ______________. reported in percentages

A

theoretical yield

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41
Q

the ____________ is the maximum amount of a product possible in a reaction. If the actual yield is more than the theoretical yield, we would be violating the ______________________.

A

theoretical yield
law of conservation of mass.

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42
Q

_____________ is the determination of the Heat Absorbed or Released in a Reaction

A

Thermochemistry

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43
Q

to calculate formula mass of a molecular compound (also called molecular mass) ________ the atomic masses of each element that makes up the molecule.

A

add

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44
Q
A

= 119.37 amu

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45
Q

How do you calculate the formula mass of an ionic compound? Why?

A

The same way you calculate the formula mass for molecular compounds.
Sum the average atomic masses (use the periodic table) of all the atoms in the compound’s formula.
The formula for an ionic compound is the ratio of the cations to the anions.
Because the formula for an ionic compound does not represent the composition of a discrete (isolated) molecules as with molecular compounds.

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46
Q

T/F the formula mass of N2O5 is 108.02

A
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47
Q

an ionic compound is the result of a ________ and ________ combining which forms an ionic bond between the atoms.

A

metal
non metal

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48
Q

a mole of a monatomic element is made up of individual _________; a mole of a molecular compound is made up of individual ____________, and a mole of an ionic compound is made up of formula ________.

A

atoms
molecules
units

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49
Q

The numerical value of things in a mole is refered to as _____________ number or ___________________ constant.

A

Avogadro’s number or Avogadro’s constant

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50
Q

TRUE/FALSE The molar mass is the mass of one mole of a substance or the mass of 6.022 x 1023 individual units of the substance.

A

TRUE
1 mol = molar mass

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51
Q

one molecule of CHCl3 contains one C atom, one H atom, and three Cl atoms; similarly,
one mole of CHCl3 contains
_____ mole C,
_____ mole H, and
_____ moles Cl.
and the unit is _______ instead of amu.

A

ONE mole of C
ONE mole of H
THREE moles of Cl
grams per mole (g/mol)

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52
Q

What is the molar mass of CHCl3?

A

the Molar mass is 119.37 g/mol

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53
Q

What’s the formula mass of sodium? What’s the mass of one mole of sodium?

A

the formula mass of sodium is 22.99amu
the mass of one mole of sodium is 22.99g

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54
Q

What is the molar mass of ammonium carbonate?

A

the molar mass is 96.09 g/mol
add each element’s atomic mass from the periodic table. If there is a subscript, multiply by that many times. NH4CO3^2

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55
Q

The first conversion factor converts _______ to ________.
The second converts __________ to __________.

A

grams to moles
moles to grams
(whatever unit is the numerator is what you’re converting to!! and denominator is what your converting from!!))

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56
Q

Avogadro’s number can be used to convert between the ________ of individual particles and the number of ________ in a substance.

A

number
moles

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57
Q
A
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58
Q
A
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59
Q
A

This gives you approximately 0.544 moles of sodium.

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60
Q
A
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61
Q

check all that apply

A

The first two answer are correct.
When using the proper conversion factors you convert 0.162 moles to atoms using avogado’s constant
next you convert 0.162 moles of silver to grams using the atomic mass of silver found on the periodic table. The atomic mass of silver is 107.87amu. remember THE MOLAR MASS IS THE SAME AS ATOMIC MASS EXPRESSED IN GRAMS INSTEAD OF AMU.

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62
Q

This formula calculates the __________ percent.

A

The mass percent composition, or mass percent.

The mass percent of an element, is the element’s percentage of the total mass of the compound
When calculating mass percent, either the actual mass of the element or the atomic mass can be used in the calculation. Examples are shown below.

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63
Q
A
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64
Q
A
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65
Q

______ ________ __________ can be used as a conversion factor between grams of a constituent element and grams of the compound. For this, we assume that we have _____________ of the compound.

A

mass percent composition
100.00 grams

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66
Q

Whats the mass percent of chlorine in aluminum chloride?

A

get the formula for alcl
then calculate the amu of the compound.
amu cl/total amu of alcl *100 = mass percent of chlorine in aluminum chlorine

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67
Q

An empirical formula gives on the smallest _____ _____ ratio of each type of atom in a compound. Therefore, if the subscripts in a formula of a compound can be reduced to smaller whole numbers, the formula ______ an empirical formula.

A

whole-number
is NOT

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68
Q

What’s the molecular and empirical formulas of water?

A

empirical: H2O
molecular: H2O
the empirical and molecular formulas are the same, because the subscripts cannot be reduced. In other words, When n is equal to 1, the empirical and the molecular formulas are the same. For example, the formula H2O is both the empirical and molecular formula for water.

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69
Q

The molecular formula for hydrogen peroxide is H2O2 and its empirical formula is _________.

A

HO
because H2O2 can be reduced in lowest terms so each subscript is one.

70
Q

3

A
71
Q
A

B

72
Q
A

C

73
Q
A

B

74
Q

A _______ is the atomic mass expressed in grams. For a compound, a _________ is the formula mass or molecular mass expressed in grams.

A

mole
mole

75
Q

1

A

A) microwaves

76
Q
A

D) all of the above

77
Q
A

B) Arsenic

78
Q
A

C)

79
Q

7

A

B)

80
Q
A

D) Cs or Cesium

81
Q

The Alkali metals have _____ electrons valence
The Alkali Earth Metals have _____ electrons valence
The Halogens have _____ electrons valence
The Noble Gases have ______ electrons in their valence
Excluding transition metals, to find the number of electrons in an element’s valence count by 1 in each group, skipping 3-12. So that the final group has 8, first group has 1!

A

1
2
7
8

82
Q

The atomic size of an atom is determined by the distance between its ___________ electrons and its _______. As move ________ the periodic table, The number of _______ increase resulting in a greater pull on the electrons to the nucleus, therefore the atomic size ________________.

A

outermost,
nucleus,
protons
decrease

83
Q

_________ decreases as we move to the right. Atomic size decreases from bottom to top.

A

atomic size

84
Q

Choose the larger atom in each pair
a) C or O
b) Li or K
c) Se or I

A

a) C
b) K
c) Unable to tell based oin periodic table placement alone,
because the path between Se and I is one down and one to the left, the atomic size decreases. These effects tend to cancel out.

85
Q

As we move across a period to the ______, ionization energy increases.
As we move down the groups the ionization energy ____________.

Ionization of an atom is the ______________________________________.

A

right
decreases

Ionization of an atom is the amount of energy required to remove an electron from the atom in order to make it’s electron configuration closer to a noble gas.

86
Q

Choose the element with the high ionization energy from each pair:
a) Mg or P
b) As or Sb
c) N or Si
d) O or Cl

A

a) P
b) As
c) N
d) you cannot tell because ionization energy decreases when you go down a column but increases when you move to the left to CL.These facts tend to cancel out, therefore you cannot tell by the periodic table alone.

87
Q

As you move down a column, metallic characteristics _________ and ionization energy __________.

A

increases
decreases

88
Q

Which property increases as you move from LEFT TO RIGHT across a row in the periodic table?
a) atomic size
b) ionization energy
c) metallic character

A

b) ionization energy (takes more energy to break apart because the electrons and protons are more anchored bc the number of protons increase as you move left to right).

89
Q

What;s the electron configuration for lithium?
remember the number of electrons are in its ________ number.

A
90
Q

Electrons occupy orbitals with the lower energy orbitals first, then move to higher energy orbitals. Therefore the further away (increase in n) increases the energy of the orbitals.
The order:
1s
2s
_p
3s
_p
_s
_d
_p
5s
4d
5p
_s

A

Orbitals fill in the following order:
1s
2s
2p
3s
3p
4s
3d
4p
5s
4d
5p
6s

91
Q
A

D

92
Q
A

C) Carbon

93
Q
A

B) Arsenic (count across for the valence orbitals!)

94
Q
A

A) F
increases as you move to the right because the protons contract electrons and the atom’s ionization is stronger with the addition of protons. also gets smaller as you move UP COLUMNS

95
Q

To write an electron configuration for an element, we first find its atomic number from the periodic table—this number equals the number of electrons in the neutral atom.

to distribute the electrons in the appropriate orbitals. Remember that each orbital can hold a maximum of two electrons. Consequently:

the s subshell has only one orbital and therefore can hold only \_\_\_\_ electrons.

the p subshell has three orbitals and therefore can hold \_\_\_\_\_ electrons.

the d subshell has five orbitals and therefore can hold \_\_\_\_\_ electrons.

the f subshell has seven orbitals and therefore can hold \_\_\_\_\_\_ electrons.
A

TWO the s subshell has only one orbital and therefore can hold only two electrons.

SIX the p subshell has three orbitals and therefore can hold six electrons.

TEN the d subshell has five orbitals and therefore can hold ten electrons.

FOURTEEN the f subshell has seven orbitals and therefore can hold 14 electrons.
96
Q

Write the electron configurations for each element
a) Mg
b) S
c) Ga

A
97
Q
A

C)

98
Q

complete the orbital diagram for Silicon

A
99
Q
A
100
Q
A
101
Q
A

A) no double bonds

102
Q
A

B) 120

103
Q
A

D)

104
Q
A

C)

105
Q
A

C) bond dipoles are formed when two atoms share electrons and one atom attracts the shared electrons greater than the other

106
Q
A

D) all of the above

107
Q
A

9.85 x 10^27

108
Q
A

23.0m/s

109
Q
A

LAST 2 OPTIONS

110
Q
A

C) 6MOL Al

111
Q
A

A)

112
Q
A

correct sig figs. no answer yet but should be 7.3

113
Q
A

B)

114
Q
A

C)**
feedback says to use dimensional analysis. water is the limiting reactant. to figure out how much product can be made calculate using the limiting reactant

115
Q
A

C)

116
Q
A

D)

117
Q
A

D)

118
Q
A

B)

119
Q
A

C)

120
Q
A

C)

121
Q
A

B)

122
Q
A

C)

123
Q
A

C)

124
Q
A

B)

125
Q
A

B)

126
Q
A

A)

127
Q
A

D)

128
Q
A

C)

129
Q
A

A)

130
Q

4.5

A

A)

131
Q
A

A)

132
Q
A

B)

133
Q
A

B)

134
Q
A

D)

135
Q
A

D)** says incorrect but i recieved credit
ensure the equation is balanced and determine if the reaction is endo or exo to decide how the eheat should be displayed

136
Q
A

B) 113g

137
Q
A

D) -0.109kJ

138
Q

MOD 3 AND BELOW CARDS START HERE ABOUT 34 CREATED
**
Definition of Atomic Mass

A

A weighted average of the mass of all the isotopes (species of an atom with varying # of neutrons in the nucleus) naturally occurring.

139
Q

How do you calculate the Atomic Mass of an element?
Give a formula

A

(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.

140
Q

What is the atomic mass calculation based on?

A

Their natural abundance and the mass of each isotope added.

141
Q

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

A

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…

142
Q

X , the symbol of an element is determined by Z. Z is the number of _____________.

A

protons

143
Q

The difference between Atomic Weight and Atomic Mass?

A

Atomic Mass is the calculation of a SINGLE isotope’s mass.
Atomic Weight is the average of all the isotopes and their natural abundance.

144
Q

The difference between Atomic Mass and Mass Number?

A

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.

145
Q

Atomic Number (Z) is

A

The number of protons in an atom’s nucleus.

146
Q

Define atomic theory

A

a theory stating that all matter is composed of tiny particles called atoms.

147
Q

NOMENCLATURE: for a ___________ is to have the ions name + “ion”
give an example

A

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

148
Q

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

A

Unpredictable cations
example Iron is Fe
Fe+2 = Iron(II) Ion
Fe+3 = Iron(III) Ion

149
Q

NOMENCLATURE: For a ________________ the naming convention is to use the atom root + “ide”
give an example

A

Anion
O2- = Oxide
N3- = Nitride

150
Q

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.

A

Atomic Number
(def. from ext lesson)

151
Q

2.2 True of False? the suffix “ide” will always refer to a monatomic anion

A

True

152
Q

How do you name the Ionic Compound Fe3+ and O2-

A

Iron(III) Oxide

153
Q

Name the Compound
Mn2O3
(3 subscript, 2 subscript)

A

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.

154
Q

Write the formula of
Lead (IV) Dioxide

A

PbO2
(subscript2)

155
Q

Binary compounds = _________ elements

Nonbinary Compounds = _____________ elements

A

two elements for binary

more than 2 elements for nonbinary

156
Q

Acids are -

A

compounds that form H3O+ when reacting with water. Must have an H+ Ion in the molecule it combined with.

157
Q

Which of the following is NOT a molecular compound?

A) GeCl4
B) NH4Br
C) PCl3

A

B) NH4Br8

158
Q

Which of the following compounds are nonbinary?

A) Acetic acid
B) HCHO, formaldehyde
C) ethanol,C2H5OH
D) All of the above are nonbinary compounds

A

D) all of the above are nonbinary compounds

159
Q

Chemical formula for iodic acid is:

A) HI(aq)
B) HIO3
C) HIO

A

B) HIO3
not a binary so no need for aq

160
Q

(2.3HW) Which of the following is a binary ionic compound?

a) NaOH
b) FeCl2
c) CaSO4
d) Br2

A

B) FeCl2

161
Q

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

A

C) PbCO3 - lead (II) carbonate

162
Q

What is the charge on lead in PbSO4?

A

2+

163
Q

Which of the following properties is true for metals?

A) shiny
B) electroconductive
C) malleable
D) brittle
E) A-C

A

E) A-C

164
Q

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%.

A

35.45 amu

165
Q

Which of the following elements are main group elements?

A) Selenium and Iron
B) Lithium and Lead
C) Silver and Tin

A

B) Lithium and Lead

166
Q

What’s the definition of an acid?

A

“a water solution that has an excess of hydrogen ions”

167
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

168
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

169
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

170
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.

171
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

CHEMISTRY 107: FUNDAMENTALS (5 decks)

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