Connect Homework Flashcards
1
Q
Which subatomic particle is found in the space that surrounds the nucleus?
A
ELECTRON
2
Q
In a single element _____ type(s) of atoms can be found.
A
ONE
3
Q
A pure substance made up of only one atom is called a(n)?
A
ELEMENT
4
Q
Which of the following best describes a contemporary model of electron movement within atoms?
A
Electrons move in orbitals, although their exact location cannot be precisely predicted in these orbitals.
5
Q
Anything that contains mass and occupies space is called?
A
MATTER
6
Q
Within an atom’s structure, electrons can be found ______.
A
IN CLOUD LIKE ORBITALS
7
Q
Which of the following is an element?
Gasoline, Coffee, Water, Carbon
A
CARBON
8
Q
Orbitals are found in ______ or energy levels.
A
ELECTRON SHELLS
9
Q
True or false: An element is made up of two or more types of atoms?
A
FALSE ( An element is composed of only one kind of atom.)
10
Q
Energy is defined as ______.
A
THE CAPACITY TO DO WORK
11
Q
Select all that apply
Which of the following are subatomic particles that are confined to a small volume within the nucleus of an atom?
- Protons
- Neutrons
- Electrons
- Prions
A
PROTONS AND NEUTRONS
12
Q
Chemical bonds can form among atoms due to the presence of unpaired _____ electrons
A
VALENCE
13
Q
Here are three descriptions of the modern model of atomic structure. Which is the best?
- A central nucleus surrounded by cloudlike orbitals containing electrons
- A collection of positive and negative charges uniformly distributed throughout the atom
- A central nucleus surrounded by electrons traveling in clearly defined orbits
A
A central nucleus surrounded by cloudlike orbitals containing electrons
14
Q
What type of subatomic particle occurs in each different element in a unique number and is therefore used to identify specific elements?
A
PROTON
15
Q
The region within an atom that surrounds the nucleus and in which there is a high probability of finding an electron is called an electron ____
A
ORBITAL
16
Q
What does the atomic number of an atom represent?
A
THE NUMBER OF PROTONS
17
Q
Within atoms, electrons are organized by energy levels called?
A
ELECTRON SHELLS
18
Q
The capacity to do work is known as?
A
ENERGY
19
Q
Select all that apply:
Select all of the following that are true about atoms that have partially filled energy shells.
A
- Can form compounds
- Tend to share, lose, or gain electrons
20
Q
Atoms of different chemical elements can be differentiated based on the number of ______ ?
A
PROTONS IN THE NUCLEUS
21
Q
Electrons in an atom’s outermost energy shells are called ____ electrons?
A
VALENCE
22
Q
An atom’s atomic number is based on the number of ______
it contains. In an atom that is not in a chemical reaction, this number equals to the number of _____ ?
.
A
Blank 1: PROTONS
Blank 2: ELECTRONS
23
Q
Within an atom, particles with nearly equal mass are ____ and neutrons, while _____ have a much smaller mass.
A
Blank 1: PROTONS
Blank 2: ELECTRONS
24
Q
Orbitals are found in ______ or energy levels.
A
ELECTRON SHELLS
25
An element's atomic ______ is based on the protons and neutrons it contains, while an element's atomic ______ is based only on the number of protons.
Blank 1: MASS
| Blank 2: NUMBER
26
The most common type of carbon atom has 6 protons, 6 electrons, and 6 neutrons. What is its atomic mass?
12 AMU or 12 DALTONS
27
Valence electrons are found in ______.
THE OUTERMOST ENERGY SHELL
28
Atomic mass is measured in what units?
AMU (atomic mass units)
DA (Daltons)
29
Which two particles are the primary determinants of an element's atomic mass?
PROTONS AND NEUTRONS
30
Phosphorus exists in several isotopes, including 31P and 32P. These are expected to have different ______.
NUMBER OF NEUTRONS
31
The atomic number of an element is equal to the number of ____
it contains. Its atomic mass includes the number of protons and the number of ____
Blank 1: Protons
| Blank 2: Neutrons
32
What four elements are the most common in living organisms?
OXYGEN, CARBON, HYDROGEN, NITROGEN
33
Oxygen has eight protons, 8 electrons, and 8 neutrons. What is its atomic mass?
16
34
Water, with the chemical formula H2O, contains ____ hydrogen atom(s) and _____ oxygen atom(s).
Blank 1: 2
| Blank 2: 1
35
Atoms share a pair of electrons when they form a(n) ____ bond.
COVALLENT
36
One ______ equals 1/12 the mass of a carbon atom.
DALTON
37
In which of the following scenarios are atoms the most stable?
When their outer shells are filled with electrons.
38
Isotopes of an element differ from one another in the number of ____
they contain.
NEUTRONS
39
Why are atoms likely to share electrons?
Because they have unfilled outer valence shells.
40
By mass, the most abundant element in living organisms is ______.
OXYGEN
41
What is a likely predictor of how many covalent bonds an atom can form?
The electron configuration in the outermost shell
42
The chemical formula of glucose is C6H12O6. How many oxygen atoms are in one molecule of glucose?
6
43
According to the octet rule, many atoms are most stable when they have ______ electrons in their outermost shell?
8
44
A covalent bond is one in which a pair of electrons ______.
is shared between 2 atoms
45
Electronegativity is the ability of an atom to ______.
attract electrons
46
Atoms are most stable when their outer shells are filled with?
electrons
47
What is true of a polar covalent bond?
- The two atoms in the bond share the electrons unequally
| - The atoms in the bond differ in electronegativity
47
Atoms tend to be most stable when their outer shells are _____ ; this can be accomplished by gaining, losing, or sharing _____.
Blank 1: Filled
| Blank 2: Electrons or Valence electrons
48
Nitrogen has five electrons in its outer shell, so it can bond with up to ______ other atoms to complete its outer shell?
3
49
A covalent bond in which the atoms share electrons unequally is a(n) _____
covalent bond.
Polar
50
Atoms are chemically the most stable when which of the following occurs?
Their outer shell is full.
51
The hydrogen bonds connecting water molecules form between a(n) ______ atom on one molecule and a(n) ______ atom on another molecule.
Blank 1: oxygen
| Blank 2: hydrogen
52
The measure of an atom's ability to attract electrons when in a bond with another atom is called its ______?
Electronegativity
53
What best describes how a hydrogen bond forms?
A partially positive hydrogen atom and a partially negative atom in another molecule are attracted by electrostatic interactions.
54
A(n) ______ bond is formed when two atoms of different electronegativities share electrons.
Polar covalent
55
Why are atoms likely to share electrons?
Because they have unfilled outer valence shells.
56
An atom that has gained or lost electrons, and thus has a net electric charge, is called a(n)
Ion
57
In a polar covalent bond, the shared electrons are closer to the nucleus of the atom with ______.
Greater electronegativity
58
If an atom gains or loses a(n) _____ it acquires a net electrical charge and becomes an ion.
Electron
59
When two water molecules are near each other, a hydrogen bond will form between the more positive _____ and the more negative _____
atoms of neighboring water molecules.
Blank 1: Hydrogen
| Blank 2: Oxygen
60
Anions are types of ions that have a net ____ charge.
Negative
61
A hydrogen bond forms when a hydrogen atom with a partial ____ charge becomes electrically attracted to an electronegative atom with a partial ____ charge.
Blank 1: Positive
| Blank 2: Negative
62
Which of the following statements are true of a polar covalent bond?
- The two atoms in the bond share the electrons unequally.
| - The atoms in the bond differ in electronegativity.
63
An atom with a net electric charge is called a(n) ______.
Ion
64
Molecules with covalent bonds ______.
Are flexible within certain limits
65
A Na+ ion forms when a sodium atom ______.
Loses an electron
66
An ion that carries a net negative charge is a(n) ______.
Anion
67
A(n) ____ containing an atom with a single, unpaired electron in its outer shell is known as a free radical.
Molecule
68
An atom or ion is most stable when its outermost shell is occupied by its full complement of ____.
8 electrons
69
Which of the following are common features of chemical reactions?
- Chemical reactions require a source of energy.
- Many chemical reactions in living organisms take place in a watery environment.
- Chemical reactions proceed toward equilibrium.
- Many chemical reactions that occur in cells require catalysts.
70
True or false: Molecules that contain covalent bonds are rigid, inflexible structures.
False
71
Which of the following properties are shared by many chemical reactions that occur in cells?
- They tend to proceed toward equilibrium.
- They require energy.
- They often require a catalyst.
72
A free radical is a molecule containing an atom with a single unpaired electron in its ______.
Outer shell
73
In which of these conditions would an atom or ion be most stable?
When its outermost shell is occupied by its full complement of electrons
74
Consider the reaction: CH4 + 2 O2 ⇌ CO2 + 2 H2O. Oxygen serves as a(n) ______.
Reactant
75
What occurs during all chemical reactions?
Chemical bonds are broken or formed.
76
In a chemical reaction, if there is no longer a change in the concentration of reactants and products, then ______.
Equilibrium has been reached
77
Which component of humans has the greatest percent of water?
Lungs
78
Chemical reactions require a source of energy and also may require a substance called a(n) ____ that speeds up the reaction rate. Most chemical reactions proceed toward a state called ____ in which the rate of product formation equals the rate of reactant formation.
Blank 1: Catalyst
| Blank: Equilibrium
79
Substances dissolved in liquid are called ______.
Solutes
80
A solution is composed of ______ dissolved in a ______.
solutes; solvent
81
In the conversion of methane and oxygen to carbon dioxide and water, carbon dioxide is a(n) ______.
Product
82
A solution in which water is the solvent is called a(n)
Aqueous
83
When the rate of the forward reaction is equal to the rate of the reverse reaction, chemical ____ has been reached.
Equilibrium
84
In a micelle, which portion of the amphipathic molecules are oriented toward the surface of the sphere?
The polar region
85
In humans, water comprises approximately ______ of body weight.
60-70%
86
The concentration of a liquid is defined as the amount of ______ dissolved in a unit volume of solution.
Solute
87
A liquid that can dissolve substances is known as a(n) ____
Solvent
88
Solutes dissolved in a solvent form a ______.
Solution
89
The molecular mass of a molecule is equal to the ______ in the molecule.
Sum of the atomic masses of all atoms
90
An aqueous solution is one in which the solvent is ______.
Water
91
Put the physical states of water in order based on the intermolecular distances between water molecules. The TOP position should be the state in which the molecules are the farthest apart.
1) The Gaseous state
2) The Solid state
3) The Liquid state
92
What part of an amphipathic molecule would be oriented toward the center of a micelle?
The nonpolar region
93
The amount of solute (in grams) dissolved in a given volume of solution is the solution's ______.
concentration
94
Why does ice float in liquid water?
Ice is less dense than liquid water.
95
When water is heated, the rate at which ____ bonds break increases, and water molecules are converted to the ____.
Blank 1: Hydrogen
| Blank 2: Gaseous
96
The sum of the atomic masses of all atoms in a molecule is equal to the molecule's ____ mass.
Molecular
97
Which state of water is the most dense?
Liquid
98
Compared with liquid water, ice has ______.
- More hydrogen bonds between individual water molecules
| - A more orderly arrangement of water molecules
99
Ice floats in liquid water because ice has a lower ______ than liquid water.
Density
100
Which of the following changes in the physical state of water require the input of energy?
- Changing from liquid to gas
| - Changing from solid to liquid
101
What happens when water freezes?
- Water molecules are packed into a less dense formation.
- The rate of hydrogen bond breakage slows.
- The H2O molecules in ice are in a much more orderly arrangement than in the liquid state.
102
Rank each state of water in order of increasing density, starting with the least dense state at the top of the list.
1) Water vapor
2) Ice
3) Liquid water
103
What is the heat of fusion of a substance?
The amount of heat energy released when 1 mole of the substance is converted from liquid to solid
104
______ is the amount of energy required to raise the temperature of 1 gram of a substance by 1o C
Specific heat
105
Properties of a solution that depend strictly on the total number of dissolved solutes, and not the specific type of solute, are called ____ properties.
Colligative
106
To freeze water, energy is ______.
Released
107
Water is used to break apart another molecule in a(n) ____ reaction.
Hydrolysis
108
High specific heat, surface tension, and cohesion are several properties of water involving ____ bonds.
Hydrogen
109
What is heat of vaporization?
The heat energy required to convert 1 mole of a substance from liquid to gas
110
What is heat of fusion?
The heat energy that must be withdrawn or released from a substance to convert it from liquid to solid
111
What is specific heat?
The heat energy required to raise the temperature of 1 gram of a substance by 1 degree Celsius
112
What is heat Capacity?
The heat energy required to raise the temperature of an entire object
113
Pure water can ionize into which of the following?
Positively charged protons (H+) and negatively charged hydroxide (OH-) ion
114
pH is defined as the ____ ____ to the base 10 of the ____ ion concentration.
Blank 1: negative
Blank 2: logarithm
Blank 3: Hydrogen
115
Colligative properties depend on the ______ dissolved in a solution.
Number of particles
116
What happens to the pH of a solution when H+ ions are added to it?
The pH decreases
117
Hydrolysis reactions ______.
Break apart molecules via water
118
A solution at pH 5 is said to be ______ because it contains more ______.
Blank 1: Acidic
| Blank 2: (Hydrogen) H+ ions than (Hydroxide) OH- ions
119
Polar covalent O-H bonds in water molecules enable hydrogen bonds to form between water molecules. Which of the following properties of water result from hydrogen bond formation?
- Cohesion
- High heat of vaporization
- Surface tension
- High specific heat
- Adhesion
120
Which ions are produced when water ionizes?
- H+ ( Hydrogen)
| - OH– (Hydroxide)
121
What type of compound minimizes pH fluctuations in the fluids of living organisms?
Buffer
122
The ______ of a solution is the negative base 10 logarithm of the H+ concentration of the solution.
pH
123
If you add H+ ions to a solution, it becomes more ______.
Acidic
124
Which of the following solutions contains the highest concentration of protons?
A solution with pH 2.0
125
A ____________ of a substance contains the same number of particles as there is in 12g of carbon.
Mole
126
One ____________ is approximately the mass of one proton or a hydrogen atom.
Dalton
127
The ____________ of an atom is a relative measure of its mass compared to other atoms.
Atomic Mass
128
____________ of carbon = 1 mole.
12g
129
____________ of hydrogen = 1 mole
1g
130
____________ of lithium = 1 mole.
7g
131
Hydrogen has a total of ____________ electron(s), ____________ are in the valence shell, and ____________ lie in the p orbitals.
1, 1, 0
132
Carbon has a total of ____________ electron(s), ____________ are in the valence shell, and ____________ are in the 1s orbital.
6,4,2
133
Nitrogen has a total of ____ electron(s), ____ are in the valence shell, and ____ lie in the p orbitals.
7,5,3
134
Oxygen has a total of ____________ electrons, ____________ are in the valence shell, and ____________ are in the p orbitals.
8,6,3
135
These 2 have the same number of electrons in their outermost shells.
Nitrogen & Phosphorus
136
These 2 have two electron shells.
Carbon & Nitrogen
137
Their outermost electron shell is full.
Helium & Argon
138
They have one electron shell.
Hydrogen & Helium
139
hey have three electron shells.
Sodium & Chlorine
140
Which two elements show similarities in the pattern of chemical bonding?
Lithium and Sodium
141
A polar covalent bond is created when
Bonded atoms have unequal pull on the shared electron, so that the electron spends more time around one atom than the other.
142
The unequal sharing of electrons between the oxygen and hydrogen atoms within a water molecule makes water a ____________ molecule.
Polar
143
As a result of the electron configuration of a water molecule, water is a great ____________ because water can break up and surround a ____________ , as long as it is not ____________ , dissolving it into solution.
Solvent, Solute, nonpolar
144
The reason water behaves in this manner is because the ____________ charge on the hydrogen end of the water molecule is attracted to the negative charge of a polar molecule, while the ____________ charge of the oxygen end of the water molecule is attracted to the positive side of a polar molecule.
Positive, Negative
145
True or False: The bonds between water molecules are stable.
False
146
True or False: As temperature drops the bonds between water molecules are less likely to break.
True
147
True or False: Ice is denser than liquid water at all temperatures
False
148
True or False: The polar covalent bonds between hydrogen and oxygen atoms within a water molecule create slight positively and negatively charged ends to the molecule
True
149
True or False: The fluid nature of water is due to hydrogen bonds continually breaking and reforming.
True
150
True or False: A hydrogen atom of one water molecule binds via a hydrogen bond to a hydrogen atom of another water molecule.
False
151
True or False: Bonds between water molecules are stronger than the bonds between the atoms within a water molecule.
False
152
Decide which example best describes each property of water.
| 1. Water is less dense at 0°C compared to 4°C.
Ice floats
153
Decide which example best describes each property of water.
| 2. Water provides structural support due to its inability to be compressed.
Turgid pressure in plants
154
Decide which example best describes each property of water.
| 3. The charged ends of a water molecule allow it to surround a solute in solution.
Solvent
155
Decide which example best describes each property of water.
4.The temperature of water rises slowly due to its high specific heat; requiring a lot of energy to convert liquid water to water vapor.
Evaporative cooling
156
Decide which example best describes each property of water.
5. While hydrogen bonds are constantly breaking and reforming, a large percentage of the hydrogen bonds between water molecules exist at all times.
Cohesive force
157
Decide which example best describes each property of water.
| 6. Due to hydrogen bonding, water tends to adhere to surfaces, such as the lining of the digestive tract.
Lubricant
158
Decide which example best describes each property of water.
| 7. The addition of water can break apart molecules into two smaller molecules.
Hydrolysis
159
Decide which example best describes each property of water.
| 8. Water is formed when two molecules come together to form a large molecule.
Dehydration reaction
160
The ____________ of water molecules, resulting from the ____________ bonds between water molecules, causes a movement of the water through the plant's vessels, as it moves up from the roots.
Cohesion; Hydrogen
161
As water ____________ from the pores of the leaves, more water is pulled up from below resulting in a constant supply of water moving up through the vessels of a plant.
Evaporates
162
Trees take up water from their roots. Water must travel against ____ up to all of the branches and leaves.
Gravity
163
6 CO2 + 6 H2O + Light → C6H12O6 + O2 is an example of a chemical reaction. What is occurring during this reaction?
Substances are changed into other substances by the making or breaking of chemical bonds.
164
Adding NH3 (ammonia) to water makes NH4+. What will be the general pH of this new solution, and what will happen to the ion concentrations?
Alkaline; decreased H+ ions and increased OH- .
165
Stable blood serum has a pH of around 7.4. The release of bicarbonates as a buffer to maintain this pH in a body with high hydrogen levels would cause the pH to move
From acidic to slightly alkaline.
166
The property of water that allows the basilisk lizard to run across its surface is
The high surface tension caused by the polar qualities of water.
167
The best summary of the properties of water is
less dense at 0oC than at room temperature, ideal solvent for biological molecules, absorbs considerable heat energy without raising temperature, and high percentage of hydrogen bonds.
168
When H2O is added to a compound in a chemical equation, a new compound can be formed via what type of reaction?
Hydrolysis
169
When two atoms are bonded together via electrons, and one of those atoms has a greater pull upon the electrons shared, the bond formed would be
A polar covalent bond.
170
Carbon 12, 13, and 14 are isotopes of the same element. They share the same place on the periodic table but possess varying numbers of neutrons. If carbon 12 has 6 protons, how many neutrons will carbon 14 have?
8
171
Water (H2O) is critical to sustain life. One of its major roles is creating and breaking bonds in chemical reactions. Other significant roles of water include
- acting as a solvent in the transport of dissolved substances around the body.
- the protection and support of organs.
- maintaining body temperature homeostasis.
172
Electrons that orbit the nucleus of an atom
- Require input of discrete amounts of energy to move between shells.
- Have lower potential energy as they move closer to the nucleus.
173
What element is found in all organic molecules?
Carbon
