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Biology 1 > Chapter 2/3 - Molecules > Flashcards

Chapter 2/3 - Molecules Flashcards

1
Q

Any substance in the universe that has mass and occupies space

A

Matter

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2
Q

Small particles that make up matter

A

Atoms

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3
Q

Tunneling microscopy

A

Technology used to locate atoms

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4
Q

What located at the center of an atom?

A

Nucleus

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5
Q

What subatomic particles form the nucleus?

A

Protons and neutrons

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6
Q

What subatomic particles surround an atom?

A

Electrons

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7
Q

Electrons are found in

A

Orbitals

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8
Q

Orbitals surround the

A

Nucleus of an atom

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9
Q

Region within an atom where the electron will most likely be located

A

Orbital

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10
Q

How many electrons can an orbital contain

A

2

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11
Q

Atomic theory

A
  1. Every atom contains electrons

2. Protons and neutrons are at the core of an atom

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12
Q

What charge does a proton have?

A

Positive

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13
Q

What charge does an electron have?

A

Negative

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14
Q

What charge does a neutron have?

A

No charge

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15
Q

Any substance that cannot be broken down into any other substances by ordinary chemical means

A

Element

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16
Q

Atomic number is equal to the number of

A

Protons

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17
Q

True or False

Atoms with the same atomic number belong to the same element

A

True

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18
Q

True or False

Different atoms have the same number of protons

A

False

Different atoms have a different number of protons

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19
Q

Pure substance that contains one atom

A

Element

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20
Q

True or false

Our body is made up of elements

A

True

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21
Q

Oxygen has eight protons so that atomic mass is

A

8

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22
Q

The atomic mass is equal to

A

Protons plus neutrons

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23
Q

Which subatomic particles contribute to mass

A

Protons and neutrons

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24
Q

True or false

Electrons contribute to mass and are heavier than protons and neutrons

A

False

Electrons do not contribute to mass and are not heavier than protons or neutrons

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25
Q

An atom is generally neutrally charged when

A

Where is an equal number of protons and electrons

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26
Q

Keeps electrons in their orbitals but opposite charge attraction

A

Protons

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27
Q

Can be gained or lost, turning into an ion

A

Electrons

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28
Q

Ion

A

When the number of electrons does not equal the number of protons

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29
Q

Name two types of ions

A

Cation

Anion

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30
Q

Cation

A
  1. Positive charge ion

2. Contains more protons than electrons

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31
Q

Anion

A
  1. Negative charge ion

2. Less protons than electrons

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32
Q

True or false

Typically, an atom has one electron for each proton and is thus electrically neutral

A

True

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33
Q

The chemical behavior of an atom is due to the number and configuration of

A

Electrons

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34
Q

Positive charges in the nucleus of an atoms are neutralized by

A

Negatively charged electrons

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35
Q

Isotope

A

Different form of the same element that possesses the same number of protons but different number of neutrons

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36
Q

The mass of atoms and subatomic particles is measured in units called

A

Daltons

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37
Q

A proton weighs approximately

A

1.007 Dalton

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38
Q

A neutron weighs approximately

A

1.009 dalton

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39
Q

Electrons weigh

A

1/1840 of a dalton, so they contribute almost nothing to the overall mass of an atom

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40
Q

Na , Cl

Na+ —> Cl-

Which element is a cation/ which is an anion? Explain.

A

Na+ is the cation. It shared/lost its electron to Cl-. Giving it more protons than electrons. Thus, the positive charge.

Cl- is the anion. A gain an electron from an Na+. Giving it more electrons than protons. Thus, the negative charge.

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41
Q

Hydrogen has 1 proton, 0 neutrons.

Deuterium has 1 proton, 2 neutrons.

Tritium has 1 proton, 3 neutrons.

What is being described?

A

An isotope.

Same element possessing the same number of protons but different number of neutrons.

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42
Q

Radioactive isotope

A
  • Unstable isotopes that will break down into an atom with a lower number of neutrons and or atomic number
  • Undergoes radioactive decay
  • release energy
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43
Q

Radioactive decay

A

Unstable isotope that decays to an element with a lower atomic number

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44
Q

True or False

Some radioactive isotopes are more unstable than others

A

True

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45
Q

The decay time for a radioactive isotope is expressed as

A

Half life

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46
Q

The time it takes for 1/2 of the atom in a sample to decay

A

Half life

  100%.   Vs.    50%  Ex: 12C --- > Half Life = 7C
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47
Q

How are fossils dated?

A

Through radioactive decay

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48
Q

Emits large quantities of energy that are harmful to living cells

A

Radioactive decay

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49
Q

Determines the chemical behavior of an atom

A

Electrons

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50
Q

What shapes are ORBITALS known to have

A

Spherical

Dumbbell shaped

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51
Q

Describe the 1s orbital

A
  1. Closest to the nucleus of an atom

2. Lowest energy level

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52
Q

Describe 2s, 2p orbital

A
  1. Further away from the nucleus of an atom
  2. Second lowest energy level
  3. 2s = 2 electrons
  4. 2p = 3 orbitals

**Max of eight electrons

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53
Q

Name all energy levels alphabetically from lowest to highest

A
  1. K —-> lowest (1s)
  2. L (2s;2p)
  3. M
  4. N —-> highest
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54
Q

How can you move electrons away from the nucleus?

A

Add energy

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55
Q

How can you move electrons closer to the nucleus?

A

Release energy

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56
Q

When energy is released electrons move

A

Closer to the nucleus —–> because energy at lower orbitals contain less energy than orbitals further away from the nucleus

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57
Q

When energy is absorbed electrons move

A

Further away from the nucleus, or the outer orbital

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58
Q

What energy level is closest to the nucleus and which is furthest?

A

Close , K

Far , N

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59
Q
  • How many electrons can the outer most energy level contain?
  • Name two exceptions.
A
  • 8

- He, H —-> Each contains a 1s orbital ONLY.

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60
Q

How can you increase the potential energy of an electron

A

Input energy

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61
Q

The amount of energy and electron possesses it is related to its distance from

A

The nucleus

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62
Q

Electrons that are the same distance from the nucleus have the same

A

Energy

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63
Q

Oxidation

A

Transfer/Loss of an electron by an atom or molecule, in metabolism

Usually associated with the gain of oxygen or loss of hydrogen

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64
Q

Reduction

A

Gain of electron

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65
Q

Redox Reaction

A

An atom or molecule becomes oxidized, while another is reduced in the same reaction

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66
Q

How many naturally occurring elements are there?

A

90

Each w different number of protons and a different arrangement of electrons

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67
Q

True or false

Elements have a repeating pattern of 6 elements

A

False

Elements have a repeating pattern of eight elements

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68
Q

Electrons in the outer most energy level are called

A

Valance electrons

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69
Q

Nonreactive/ Inert / “Happy”

A

Elements that contain all eight valance electrons in their outer most energy level

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70
Q

If an element contains all eight electrons in its outer most energy level can it bond with other elements

A

No because it is non-reactive, happy or inert

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71
Q

Elements that contain less than eight electrons are

A

Very reactive

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72
Q

Elements that contain seven electrons will try to

A

Fill up their outer most energy level

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73
Q

Elements that contain one electron will try to

A

Rid there outermost electron

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74
Q

What is it called when one element loses its electron to another element

A

Ionic bond

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75
Q

Octet rule

A

Atoms like to completely fill their outer energy levels

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76
Q

If helium has two valance electrons and nitrogen has four valance electrons, which element would be very reactive?

A

Helium is non-reactive due to its 1s orbital, therefore nitrogen would be very reactive

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77
Q

What 12 elements are found in living organisms?

A

C, H, O, N, P, S, Na, K, Ca, Mg, Fe, Cl

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78
Q

Which elements make up 96.3% of your bodyweight?

A

C, H, O, N

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79
Q

Compounds found in living organisms that contain carbon

A

Organic compounds

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80
Q

Carbon is found in

A

Sugars, fatty acids, and amino acids

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81
Q

What does the Periodic Table display

A

Elements according to atomic number and properties

82
Q

K has 1 valence electron/Br has 7 valence electrons. Based on the octet rule which element will be oxidized and which will be reduced? Explain.

A

K will be oxidized. It is very reactive and will rid its 1 valence electron.

Br will be reduced. It also is very reactive and will gain an electron from K instead of getting rid of its 7 valence electrons.

83
Q

True or false

All noble gases are non-reactive

A

True

84
Q

Majority of molecules that make up your body

A

Organic compounds

85
Q

A group of atoms held together by energy and a stable association is called a

A

Molecule

86
Q

ELEMENT Na has lost an electron to ELEMENT Cl, what type of bond is this?

A

Ionic bond

87
Q

When a molecule contains atoms of more than one element it is called

A

A compound

88
Q

When to or more elements are joined

A

Chemical bond

89
Q

How can an ionic bond or lattice be broken?

A

In the presence of water/ or present water/ H2O

***ex: Na+ , Cl-

Na+ and CL- are attracted to the opposite poles of water, this allows Na to retain its + charge and Cl to retain its - charge

90
Q

What bond that forms a Crystal, Solid, or lattice?

A

Ionic bond

91
Q

Covalent bond

A

When 2 atoms share a valance electron

   Or

When 2 or more atoms share one or more pairs of electrons

92
Q

Forms when atoms with opposite electrical charges (ions) attract
(+)Cation ^ Anion(-)

A

Ionic bonds

93
Q

True or false

NaCl is common table salt

A

True

Lattice, solid, crystal

94
Q

Are covalent bond stable? Explain.

A

Yes, covalent bond are stable.

  1. NO NET CHARGE, so neither atom loses or gains electrons
  2. SATISFIES OCTET RULE, shared electrons can orbit both atoms.
  3. HAS NO UNPAIRED ELECTRONS , free electrons shared between two atoms are now paired.
95
Q

Do double bonds satisfy the octet rule?

A

Yes, by allowing to atoms to share two pairs of electrons

96
Q

True or false

The strength of covalent bond depends on the number of shared electrons

A

True

Ex: Triple bond > double bond > single bond

97
Q

In a covalent bond what does — represent?

A

The sharing of one electron pair

98
Q

How many valence electrons does carbon have?

A

4

99
Q

Carbon can form multiple covalent bonds because it has

A

Four valance electrons

100
Q

Affinity for electrons

A

Electronegativity

101
Q

Increases left to right across a row of the periodic table and decreases down the column

A

Electronegativity

102
Q

Nonpolar covalent bond

A
  1. Affinity for electrons is the same, the electrons are equally shared.
  2. Equal electronegativity

**Neither element is pulling the electrons more than the other because equal electronegativity

** Same element

** different elements with a very similar electronegativity

103
Q

Polar covalent bond

A

Unequal electronegativity

Electrons are not shared equally

Atoms differ greatly in electronegativity

Shared electrons are more likely to be closer to the atom with greater electronegativity and less likely to be near the atom of lower electronegativity

Electrically neutral

104
Q

Contains regions of partial negative charge near the more electronegative atom

A

Polar covalent bonds

105
Q

Contains regions of partial positive charge near the less electronegative atom

A

Polar covalent bond

106
Q

Formation or breaking of chemical bonds

A

Chemical reaction

107
Q

What are chemical reactions to dependent on?

A
  1. Temperature, which affects the speed of molecular movements
  2. Centration of products or reactants,

More reactant = more reaction
Less reactant = less reactant

  1. Catalysts

Speeds the rate of reactions

108
Q

What protein catalyzes almost every chemical reaction in living systems

A

Enzymes

109
Q

Consist of 2H covalently bonded to 10

A

Water

110
Q

True or false

Water is not stable

A

False

Water is very stable

  1. Satisfies octet rule
  2. All electrons paired
  3. Carries no net electrical charge
111
Q

Which has a higher electronegativity, oxygen or hydrogen?

A

Oxygen

112
Q

Is a water molecule polar or nonpolar?

A

Polar

113
Q

H2O carries two partial negative charges near

A

Oxygen

114
Q

H2O carries to partial positive charges on

A

Each hydrogen

115
Q

High polarity of water allows formation of

A

Hydrogen bonds

116
Q

True or false

Hydrogen bonds organize most of the molecules in living systems

A

True

117
Q

Bonds between partially negative O atoms and the partially positive H atoms of two water molecules form

A

Hydrogen bonds

118
Q

Since water molecules attract each other they are

A

Cohesive

119
Q

Because water molecules are attracted to other polar molecules they are

A

Adhesive

120
Q

True or false

The polarity of water allows water molecules to be attracted to one another

A

True

Water is cohesive

121
Q

What is responsible for water being a liquid and not a gas

A

Waters cohesion

122
Q

True or false

The polarity of water allows it to be attracted to other polar molecules

A

True

Water is adhesive

123
Q

Specific heat

A

The amount of heat needed to be absorbed or lost by 2g of a substance to raise or lower is the temperature by 1°C

124
Q

How much energy do you need to put into a substance to raise or lower its temperature?

This question describes what.

A

Specific heat

125
Q

Heat of vaporization

A

The amount of heat needed to change a liquid to a gas

126
Q

How much heat do you need to put into change that substance from a liquid to a gas

The question is an example of what.

A

Heat of vaporization

127
Q

Does water have a high specific heat

A

Yes

Due to its unique nature in forming hydrogen bonds

128
Q

Partial + and Partial - allow water to form

A

Hydrogen bonds

129
Q

How can a hydrogen bond be broken

A

By an abundance of thermal energy or heat

130
Q

Does water take awhile to heat up?

A

Yes, because it has a high specific heat so you need a lot of heat to heat up water

131
Q

Biological systems/living organisms are mostly composed of water which helps to maintain

A

Body temperature

132
Q

Biological reaction

A
  • Produces heat

- Transfers heat to surrounding water ( breaks a couple hydrogen bonds )

133
Q

Overheating and biological systems is possible without the presence of

A

Water

134
Q

Does water have a high heat of vaporization?

A

Yes.

As he is released from the body, any water to the surface of the body, he will break down does hydrogen bonds, water will evaporize to air.

Ex: Too hot—-> sweat

135
Q

Do polar ions carry a charge?

A

Yes.

Anion / cation

136
Q

Is a polar ion soluble in water?

A

Yes

137
Q

True or false

Water is not attracted to polar ions

A

False

Water is attracted to polar ions

138
Q

Water surrounds ions to form

A

Hydrogen bonds within a water molecule

139
Q

Is water a solute, or solvent?

A

Solvent

140
Q

Are ions solute or solvent?

A

Solute

**Soluble in water

141
Q

Polar ions want all of their surface exposed to water therefore they are

A

Hydrophilic

142
Q

Oil is an example of what type of molecule

A

Non-polar molecule because it is hydrophobic, water fearing

143
Q

Aggregate, or clumps together to minimize their disruption of hydrogen bonding in water

A

Nonpolar molecules

Because they are hydrophobic, water fearing

144
Q

What does water cause nonpolar molecules, such as oil to do

A

Aggregate, or push together

145
Q

What determines the PH of a solution?

A

Concentration of H+ and OH-

146
Q

PH measures

A

The # or concentration of protons and hydrogen ions

147
Q

Based on a Ph scale

0=

7=

14=

A

0 is most acidic

7 is neutral

14 is most basic

148
Q

Substance resistant to PH change

A

Buffer

149
Q

What does a buffer do when pH is too high or acidic

A

Releases H+

150
Q

What does a buffer do when pH is too low or basic

A

Absorbs H+

151
Q

Maintains constant pH

A

Buffer

152
Q

Substance that dissolves in water to increase H+ concentration

A

Acid

153
Q

A substance that combines with H+ when dissolved in water, thus lowering H+

A

Base

154
Q

True or false

Living organisms are not sensitive to pH change

A

False

living organisms are very sensitive to pH change

155
Q

Blood pH is maintained by which to buffers

A

Carbonic acid

Bicarbonate

156
Q

True or false

The pH inside almost all living cells, and in the fluid surrounding cells in multicellular organisms,is fairly close to neutral, 7.

A

True

157
Q

Is CO2 basic?

A

No. CO2 is acidic

158
Q

In our bodies CO2 is converted to

A

Bicarbonate

159
Q

What does bicarbonate do in our body

A

Transfers CO2 to the lungs so that we can breathe it out

160
Q

If blood is too acidic bicarbonate will add or retain a_________________ to form _____________________.

A

Proton

Carbonic acid

161
Q

If too basic carbonic acid can release a____________ to form ________________.

A

Proton

Bicarbonate

162
Q

Can form chemical compounds

Are chemically reactive

Can form bonds with other atoms

A

Atoms that have unfilled electrons cells

163
Q

Arrange states of water from most dense to least dense

Sold
Liquid
Gas

A

Liquid - water is more dense than ice

Solid (ice)

Gas

164
Q

Made of two or more atoms held together by chemical bonds and stable association. The Atoms may or may not belong to the same element

A

Molecule

165
Q

Arrange least to greatest based on electronegativity

H,C,O,N

A

H

C

N

O

166
Q

Van der waals attraction

A

Weak attraction between atoms due to oppositely polarized electron clouds

167
Q

Attraction between covalently bound H atom with a slight positive charge and another covalently bound atom with a slight negative charge

A

Hydrogen bond

168
Q

Hydrophobic interaction

A

Nonpolar regions of a molecule are forced together in order to minimize contact with water molecules

169
Q

Elements possessing all 8 valence electrons are said to be

A

Inert

Noble gases

170
Q

Rank the following bonds and interactions in order from strongest to weakest starting with the strongest at the top

Ionic bond 
Hydrogen bond 
Covalent bond 
Van der walls attraction 
Hydrophobic interaction
A

Covalent bond

Ionic bond

Hydrogen bond

Hydrophobic interaction

Van der waals attraction

171
Q

Cohesion

A

Plant leaves pull water up from roots

172
Q

Many types of ions and molecules move freely in cells, permitting a diverse array of chemical reactions

A

Solubility

173
Q

Why is H2 stable? (, a molecule formed by two hydrogen atoms )

A

Held together by covalent bond

No net charge

No unpaired electrons

174
Q

Water is polar

True or false

A

True

175
Q

O2, CH4, N2 are all nonpolar

True or false

A

True

176
Q

Hydrogen atoms always have one proton

True/false

A

True

177
Q

Ex: molecular formula

A

H2

178
Q

Elements in the same chemical group have the same bonding properties because they have the same number of valance electrons

True/false

A

True

179
Q

The number in configuration of electrons determine and elements

A

Chemical properties

180
Q

Hydrogen < single covalent < double covalent < triple covalent

These bonds are arranged from weakest to strongest

True or false

A

True

181
Q

Chemical bonds are broken and new bonds are formed on a

A

Chemical reaction

182
Q

One____________ of the element carbon contains 6.02 x 10^23 atoms of carbon

A

Mole

183
Q

The pH up of the solution is defined as

A

The negative logarithm of the hydrogen ion concentration in the solution

184
Q

For most of the on the elements in living organisms

A

Hydrogen ,oxygen , nitrogen and carbon

185
Q

Water rises inside a glass tube with narrow diameter due to

A

Water molecules adhere to the surface of the glass

186
Q

Element

A

Substance that cannot be broken down into simpler substances by ordinary chemical means

187
Q

Trace elements

A

Present in tiny amounts

Play cry or ole in living processes

188
Q

The ability of water to rise inside a tube of narrow diameter against the pull of gravity is called

A

Capillary action

189
Q

Dalton =

A

Atomic mass

190
Q

Surface tension of what is due to

A

The cohesion of water molecules

191
Q

The property of ______________ is a measure of how difficult it is to stretch or break the surface of a liquid

A

Surface tension

192
Q

Polar molecules

A

Attracted to other polar molecules

Electrically neutral

Same number of protons and electrons

193
Q

When writing out structural formulas, covalent bonds are represented by the

A

Lines between atomic symbols

194
Q

Hydrogen bond can form between partial negative ___________ atom of one water molecule and partial positive ___________ atom of another molecule

A

Oxygen

Hydrogen

195
Q

Non polar covalent bond

A

Equal sharing of one or more pairs of electrons

196
Q

Hydrocarbon chains are considered nonpolar

A

True

197
Q

Buffers stabilize pH by releasing hydrogen ions when a base is added and absorbing hydrogen ions when an acid is added

A

True

198
Q

Bond formed between two hydrogen atoms

A

Nonpolar covalent

199
Q

A substance whose molecules are made of atoms of more than one element held together by chemical bonds is called

A

Compound

200
Q

Ionic compounds generally exist as individual ions

A

True

Biology 1 (11 decks)

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