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NAS2 Challenge Exam Prep > Unit 2: Chemistry > Flashcards

Unit 2: Chemistry Flashcards

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1
Q

What elements are most important to life? What elements should we still know?

A

Hydrogen, Carbon, Nitrogen, Oxygen
Sodium and Phosphorus

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2
Q

What is matter?

A

Anything that has weight and takes up space

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3
Q

What is an element?

A

A pure substance with a specific number of protons

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4
Q

What is an atom?

A

The smallest stable unit of matter. It has the same properties as every other atom in a particular element.

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5
Q

What are the charges of a:
Proton
Neutron
Electron

A

+
None
-

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6
Q

What’s the mass of:
Proton
Neutron
Electron

A

1 amu
1 amu
0 amu

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7
Q

What does the atomic number refer to?

A

The number of protons. This is a distinguishing characteristic between elements

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8
Q

What is an ion?

A

A charged atom (can be positively or negatively charged)

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9
Q

What’s a cation?

A

A positively charged ion. Has more protons than electrons

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10
Q

What’s an anion?

A

A negatively charged ion. Has more electrons than protons

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11
Q

How do you write a Hydrogen cation?

A

H^+

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12
Q

What is a molecule?

A

Two or more atoms that have been chemically joined (or “bonded”).
These can be the same atoms or different atoms.
H2O
SO4^2-

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13
Q

What’s a compound?

A

Different atoms held together by chemical bonds

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14
Q

What’s the chemical formula for
Glucose
Nitrogen gas?

A

C6H12O6
N2

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15
Q

Where does chemical bonding occur?

A

Within a molecule

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16
Q

What is covalent bonding?

A

Electrons are shared between two atoms. The electrons travel around both atoms’ nuclei. Sharing does not have to be equal

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17
Q

What is ionic bonding?

A

Electrons are transferred between two atoms

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18
Q

What is the outer/last used shell that electrons inhabit called?

A

Valence shell

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19
Q

Atoms are ______ with a full valence shell

A

Stable

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20
Q

_____ are stable when paired off (in twos)

A

Electrons

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21
Q

_____ are shared or transferred to fill or empty valence shells.

A

Electrons

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22
Q

What is equal sharing in a covalent bond called?

A

Nonpolar covalent bond
Electrons spend equal amounts of time at each nuclei

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23
Q

What is unequal sharing in a covalent bond called?

A

Polar covalent bond
Electrons spend more time at one nucleus than the other(s)

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24
Q

What symbol represents a covalent bond? How many can there be?

A

Lines between letters represent covalent bonds. Carbon for example is able to form single, double, and triple bonds (C-C, C=C, etc.)

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25
What element is assumed in a molecular drawing where lines meet?
Carbon
26
How many bonds can carbon form?
4. Carbon is element #6. It has two electrons in its first shell, and four in its second. This leaves four spots available in its valence shell
27
How many electrons can be in each shell, starting from the innermost?
2 8 32 https://www.lwtech.edu/campus-life/learning-lab/resources/docs/lwtech-learning-lab-science-atom-structure.pdf
28
Which are stronger, ionic or covalent bonds?
Ionic
29
Which chemical interactions occur within a molecule versus between separate molecules? Hydrophobic interactions Covalent bonds Hydrogen bonds Ionic bonds
Covalent and ionic bonds occur WITHIN a molecule Hydrophobic and hydrogen bonding occurs BETWEEN molecules
30
Polar molecules are hydrophobic or hydrophillic?
Hydrophilic ("water loving") Polar parts face towards a watery environment In the picture: hydrophilic head
31
Nonpolar molecules are hydrophobic or hydrophillic?
Hydrophobic ("water fearing") Nonpolar parts will face away from watery environments In the picture: hydrophobic tails
32
What bonding is not technically a chemical bond?
Hydrogen bonding There is no adjustment to the valence shells
33
Where does hydrogen bonding take place?
Between polar covalent bonds
34
Atoms move faster when hot or cold?
Atoms move fastest when heated
35
What property of water keeps its atoms from "jiggling" or vibrating too much?
Its hydrogen bonds
36
What is the transition of a liquid water to a gas called?
Evaporation
37
Evaporation requires ____ --> has a ____ effect
Evaporation requires heat --> has a cooling effect
38
What does polar solvent mean?
It will dissolve other molecules with polar or ionic bonds Hydrophilic molecules dissolve in water- "like dissolves like"
39
What is the difference between cohesion and adhesion?
Cohesion: water molecules sticking to each other (think capillary action...Water molecules stay close together and rise up the tube due to this sticky force) Adhesion: water molecules sticking to other things (think of water droplets sticking to the ends of leaves but not falling off even with gravity)
40
Solvents are ____ Solutes are what's ____ Solutions are what's ____
Solvents are substances that dissolve other substances Solutes are what is dissolved Solutions are what's created
41
What is the solute, solution, and and solvent in saltwater?
Solvent: Water Solute: Salt Solution: Salt water
42
What makes a molecule "organic"?
It has mostly carbon and hydrogen atoms
43
"Functional groups" are atoms that are ____ together
A specific combination of atoms bonded to a molecule that provide some new property; Frequently found together
44
-OH
Hydroxyl
45
-CH3
Methyl
46
-COOH
Carboxyl
47
-NH3
Amino
48
-PO4
Phosphate
49
What are reactants versus products in a chemical reaction?
Reactants (starting materials) --> products (resulting materials)
50
What does H2O dissociate to?
OH- and H+
51
Do acids or bases have a higher pH?
Acids are from -1 to 6 (-1 is strongest) 7 is neutral (water!) Bases are from 8 to 14 (14 is strongest)
52
Do acids have a higher H+ or OH- concentration?
Acids have a higher concentration of hydrogen ions (H+), greater than pure water. Bases have low H+ concentrations, less than pure water
53
What would adding HCl do to water?
HCL --> H+ and Cl- HCl increases the concentration of H+ That means the water would become more acidic. The normal pH of 7 would drop lower.
54
What would adding NaOH do to water?
NaOH --> Na+ and OH- NaOH increases the concentration of OH- This means the water would become more basic. The normal pH of 7 would rise higher.
55
Can strong acids/bases both dissociate and come back together?
No. Strong acids and bases can dissociate, but don't come back together. Weak acids/bases are able to both dissociate and easily come back together
56
What is a buffer?
A chemical that can add or take away H+ ions. They help maintain a steady pH.
57
What is maintaining a steady pH important for?
Maintaining the shape of molecules Maintaining bodily functions Proper chemical reactions
58
What is denaturing?
A shape change that causes a loss of function
59
What is energy?
The ability to do work (move matter)
60
How do cells get energy to perform their functions?
By breaking bonds in molecules. This releases energy
61
What is energy that is currently being used called?
Kinetic energy
62
What is energy that is not being used right now, but is ready to be used when necessary?
Potential energy
63
Combining molecules into a bigger molecule is called...
Synthesis
64
Breaking a molecule into smaller molecules is called...
Decomposition
65
Can molecules be exchanged?
Yes! It is represented by a double arrow. HCl + NaOH <--> NaCl + H2O
66
What does an endergonic reaction look like? Does it have a high or low activation energy?
In endergonic reactions, energy is absorbed and results in products that contain more energy than the reactants had The reaction is not spontaneous, and delta G is greater than 0 Activation energy is larger in endergonic reactions
67
What does an exergonic reaction look like? Does it have a high or low activation energy?
In an exergonic reaction, free energy is released. As energy is released instead of consumed, the products have less energy than the reactants. More energy is released in the form of heat
68
What groups are in ATP, and what are their charges?
3 negatively charged phosphate groups. They repel each other, so when the bonds holding them are broken, energy is released
69
What's happening here: ATP <--> ADP + P
Bonds of ATP are being broken, and energy is being released
70
What's happening here: ADP + P <--> ATP
Bonds are being formed, and energy is being consumed. A "recharge" of the energy supply
71
What do enzymes do? What are they made of?
Molecules that make a chemical reaction go faster thanks to lowering the activation energy; catalyzes a reaction Enzymes are made of protein, sometimes RNA Ends in "-ase"
72
What are enzyme reactants called?
Substrate
73
What are the steps enzymes take?
1. Substrate enters the active site 2. The enzyme changes shape slightly as the substrate binds (it has initiated a chemical reaction) 3. The reactants change into products 4. The products leave the active site
74
Will a higher substrate concentration raise or lower enzyme activity?
Higher substrate concentrations raise enzyme activity.
75
What happens when an enzyme is denatured?
The protein loses its shape and its subsequent function
76
Because chemical energy is stored, it is a type of ____ energy
Potential energy

NAS2 Challenge Exam Prep (5 decks)

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