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BIO MIDTERM > Lesson 1, Chapter 2 > Flashcards

Lesson 1, Chapter 2 Flashcards

(77 cards)

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1
Q

What is matter?

A

Anything that has mass and occupies space

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2
Q

What are all life forms composed of?

A

Matter

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3
Q

What can matter exist in?

A

3 states; solid, liquid or gas

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4
Q

What is an atom?

A

Smallest functional units of matter that form all chemical substances

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5
Q

Can atoms be further broken down?

A

No

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6
Q

What are molecules?

A

Two or more atoms bonded together

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7
Q

What is each specific type of atom called

A

Chemical element

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8
Q

What are the 3 subatomic particles?

A

Protons, neutrons, electrons

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9
Q

What type of charge do protons have and where they are found?

A

Positive; atomic nucleus

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10
Q

What is the charge of a neutron and where are they found

A

Neutral; atomic nucleus

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11
Q

What type of charge does an electron have and where is it found

A

Negative; orbitals

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12
Q

When would there be no net charge

A

When protons and electrons are present in equal numbers

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13
Q

Number of neutrons can __

A

vary

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14
Q

Where do electrons travel

A

Within regions surrounding the nucleus (orbitals) in which the probability of finding that electron is high

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15
Q

What are the 2 types of orbitals?

A

S and P

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16
Q

What shape are s orbitals

A

Spherical

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17
Q

What shape are p orbitals

A

Dumbbell

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18
Q

How many electrons can each orbital hold

A

2 per orbital; 8 total

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19
Q

How are electrons arranged in atoms with more electrons?

A

In atoms with more electrons, the electrons are arranged in layers or “shells” around the nucleus. Each new shell is farther from the center, and the more electrons there are, the more distant these shells become. Within each shell, electrons move in regions called orbitals.

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20
Q

What does the 1st shell look like

A

1 spherical orbital = 1s and holds 1 pair of electrons

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21
Q

What does the 2nd shell look like

A

1 spherical orbital = 2s - holds 1 pair of electrons
3 dumbbell orbitals = 2p - holds 4 pairs of electrons

can hold 4 pairs of electrons = 8 electrons

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21
Q

How do we distinguish one element from another

A

Number of protons

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21
Q

What is the atomic number

A

Equals number of protons
Also equal to the number of electrons in the atom so that the net charge is 0

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22
Q

What is the periodic table organized by

A

Atomic number
Rows = # of electron shells
Columns = # of electrons in the outer shell (valence electrons)

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23
Why do similar properties of elements within a column occur
Same number of electrons in their outer shells = similar chemical bonding properties
23
What does an atomic mass scale indicate
An atoms mass relative to the mass of other atoms
24
Most common form of carbon has # x and # x, is assigned to an atomic mass of exactly #
6 protons, 6 neutrons, 12
25
What is mass vs weight
Weight is derived from the gravitational pull on a given mass
26
What is the unit of measurement for atomic mass
Dalton (Da) or amu
27
What is a mole
1 mole of any element contains the same number of atoms - 6.022 x 10^23 (avogardro's number)
28
What is an isotope
Multiple forms of an element that differ in the number of neutrons
29
Atomic masses are _____ of the _____ of different _____ of an ______
averages, masses, isotopes, element
30
What are radioisotopes?
Used in medicine for cancer treatment, imaging Unstable and emit radiation as they decay
31
What elements make up about 95% of the atoms in living organisms?
Hydrogen, oxygen, carbon and nitrogen
32
Where do hydrogen and oxygen occur primarily?
In water
33
Where is nitrogen found
In proteins
34
What is the building block of all living matter
Carbon
35
What is a molecular formula
Contains chemical symbols of the elements in the molecule
36
What are the 3 types of bonds?
Covalent, hydrogen and ionic
37
What is a covalent bond
Electrons are shared to fill valence shells Can be polar or nonpolar covalent
38
What is a hydrogen bond
Hydrogen atom from 1 polar molecule is attracted to an electronegative atom from another molecule
39
What is an ionic bond
Electrons are transferred, forming ions that are attracted to each other
40
What can atoms share
Pair of electrons
41
What is the octet rule
Atoms are stable with their outer shell is full Many atoms = 8 electrons but exception is hydrogen with 2
42
How do polar covalent bonds form
Between atoms of different electronegativity
43
What causes polarity
Unequal distribution of electrons creates a difference in electric change across the molecule
44
How do nonpolar covalent bonds form
Between atoms with similar, electronegativities
45
What is the charge difference across molecules in nonpolar covalent bonds
No charge difference, equal sharing of electrons
46
How does a hydrogen bond form
Hydrogen atom from one polar molecule is attracted to an electronegative atom of another
47
What are enzymes?
Molecules that catalyze biologically important chemical reactions
48
What are the van der waals dispersion forces
Weak type of attraction between molecules. Happens because electrons move randomly within their obitals. A fleeting electrical attraction to other nearby molecules may arise. Collective strength can be quite strong.
49
How is the shape of a molecule determined
Arrangement and number of bonds between atoms
50
____ bonds are not ___ and ____ around single covalent bonds allows molecules to change ____
covalent, rigid, rotation, shape
51
What can the binding of one molecule to another cause the molecule to do
Change shape
52
What is a chemical reaction
When one or more substances are changed into other substances
53
What are some properties of chemical reactions?
1) Require a source of energy 2) Often require an enzyme as catalyst - speeds reaction rate 3) Proceed in a particular direction but will eventually reach equilibrium 4) Occur in liquid (water)
54
What are properties of water
1) 95% of the weight of certain plants comes from water 2) 60-70% of human weight comes from water 3) Most chemical reactions in nature involve molecules that are dissolved in water (including reactions inside cells)
55
What is a solution
Solutes in a solvent.
56
When is water the solvent?
Aqueous solution
57
What are hydrophilic
When ions and molecules with polar covalent bonds dissolve in water
58
What is the difference between hydrophilic and hydrophobic
Readily dissolve in water and do not dissolve in water
59
When is something amphipathic
- Both polar/ionized and nonpolar regions - May form micelles in water - Detergent is an amphipathic molecule
60
What is the concentration
Amount of a solute dissolved in a unit volume of solution
61
What is molarity
Molecular mass is the sum of all the atomic masses of all the atoms in the molecule
62
Changes in H2O three states of matter involves what?
Input or release of energy
63
What is the energy to boil?
Heat of vaporization
64
What is the energy to melt?
Heat of fusion
65
What are the colligative properties of water
Properties that depend strictly on the total number of dissolved solute particles, not on the type of solute
66
What is the temperature at which a solution freezes or boils influenced by
Amounts of dissolved solutes
67
What is antifreeze
Lowers the freezing point of the water and prevents it from freezing in cold weather
68
What happens to pure water to a very small extent into hydrogen ions and hydrogen
It was ionizes
69
What are acids
Molecules that released hydrogen ions in solution
70
What lowers the H+ concentration
Bases
71
Explain the pH scale
Acidic solutions are pH 6 or below pH 7 is neutral Alkaline solutions are pH 8 or above
72
What are the effects of pH
- shapes and functions of molecules - rates of many chemical reactions - ability of two molecule to bind to each other - ability of ions or molecules to dissolve in water
73
What can an acid-buffer system do
Shift to remove/release H+ to adjust for changes in pH
73
What do buffers do
Help to maintain a constant pH

BIO MIDTERM (4 decks)

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