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HESI > Chemistry > Flashcards

Chemistry Flashcards

(101 cards)

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1
Q

Scientific notation:

A

Scientific system of writing numbers

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2
Q

Scientific notation is composed of 3 parts:

A
  1. a mathematical sign (+ or -)
  2. Significand
  3. Exponential/logarithm
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3
Q

Basic measurements of the metric system:

A

Grams (weight)
Liters (volume)
Meters (distance)

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4
Q

3 common temperature systems:

A

Fahrenheit, Celsius, Kelvin

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5
Q

Fahrenheit:

A

A. Zero degrees (0 F) is the freezing point of sea water at sea level
B. 32 F is the freezing point of pure water at sea level
C. 212 F is the boiling point of pure water at sea level

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6
Q

Celsius:

A

A. Zero degrees (0 C) is the freezing point of pure water at sea level
B. 100 C is the boiling point of pure water at sea level
C. Most people have a body temp of 37 C

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7
Q

Kelvin:

A

A. Zero degrees (0 K) is -273.15 C and is the lowest temp achievable or absolute zero
B. The freezing point of water is 273 K
C. The boiling point of water is 373 K

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8
Q

Atom is composed of:

A

Protons and neutrons in the center and electrons orbiting the outside

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9
Q

The electrons orbit the nucleus at various energy levels called:

A

Shells or orbits

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10
Q

Charge of protons, electrons, neutrons:

A

Proton (+)
Electron (-)
Neutron (no charge)

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11
Q

When an atom is electrically charged, it’s called:

A

Ion

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12
Q

Cation:

A

Atom that has a positive charge

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13
Q

Anion:

A

Atom that has a negative charge

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14
Q

Rows in a periodic table are called:

A

Periods

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15
Q

Columns in a periodic table are called:

A

Groups

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16
Q

Atomic number:

A

Number or protons in the nucleus

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17
Q

Atomic mass:

A

The average mass of each of that element’s isotopes

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18
Q

Isotope:

A

Different kinds of the same atom that vary in weight

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19
Q

Compound:

A

Combination of atoms and other elements

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20
Q

Law of conservation of mass states:

A

Mass cannot be created or destroyed during a chemical reaction. Therefore, the equation must be rearranged and balanced.

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21
Q

Equilibrium:

A

A state in which reactants are forming products at the same rate that products are forming reactants (reversible).

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22
Q

4 ways to increase reaction rate:

A
  1. Increase in temp
  2. Increase in surface area of reactants
  3. Add a catalyst
  4. Increase concentration of reactants
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23
Q

Increasing the temp causes:

A

Particles to have a great kinetic energy that causes them to move around so fast that they collide

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24
Q

Increasing the surface area causes:

A

More opportunity for the particles to come in contact with one another

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25
Adding a catalyst:
Reduces the activation energy or amount of energy necessary for a reaction to occur
26
Examples of catalyst:
Metals and proteins (enzymes)
27
Increasing the concentration causes:
More chance of collisions between the reactants, which produces more products
28
Solution:
Homogenous mixture of two or more substances
29
Solute:
Parts being dissolved
30
Solvent:
Part doing the dissolving
31
4 types of solutions:
1. Compounds 2. Alloys 3. Amalgams 4. Emulsions
32
Alloys:
Solid solution of metals to make a new one (Ex. copper + tin= bronze)
33
Amalgams:
A specific type of alloy in which a metal is dissolved in mercury
34
Emulsions:
Mixtures of matter that readily separate such as water and oil
35
Concentration is expressed as:
Weight per weight Weight per volume Volume per volume
36
A mole is: AKA
6.02 x 10^23 Avogadro's number
37
5 types of chemical reactions:
1. Synthesis 2. Decomposition 3. Combustion 4. Single replacement 5. Double replacement
38
Synthesis:
Two elements combine to form a product
39
Decomposition:
Opposite of synthesis- breaking of a compound into its compound parts
40
Combustion:
Self-sustaining exothermic chemical reaction where oxygen and a fuel compound react
41
Single replacement:
Consist of an active metal reacting with an ionic compound containing a less active metal to produce a new compound
42
Double replacement:
- Involves two ionic compounds: the positive ion from one compound combines with the negative ion of the other compound - "Switching partners"
43
2 types of chemical bonding:
Ionic and covalent
44
Ionic bonding:
- Electrostatic attachment between two oppositely charged ions (or a cation and an anion) - Formed between metal and nonmetal
45
Covalent bonding:
- Formed when two atoms share a pair of electrons with one pair from each atom - Formed between two nonmetals - Strongest bond
46
Non-polar bond:
Electrons in a covalently bonded compound are shared equally
47
Polar bond:
The shared electron density is concentrated around one atom more than the other (not equal)
48
Intermolecular forces:
Weaker forces of attraction between whole molecules
49
List 3 intermolecular forces:
1. Hydrogen bonding 2. Dipole-dipole interactions 3. Dispersion forces
50
Hydrogen bond:
- The attraction for a hydrogen atom by a highly electronegative element - Strongest of all intermolecular forces
51
Dipole-dipole interactions:
The attraction of one dipole on one molecule for the dipole of another molecule
52
Dipole:
Separation of charges within a molecule between two covalently bonded atoms
53
Dispersion forces:
- When the electrons within an element or compound concentrate themselves on one side of an atom causing a temporary dipole - Weakest of all intermolecular forces
54
Stoichiometry:
Quantities and numeric relationships of the participants in a chemical reaction
55
Dimensional analysis:
Process used to determine the number of moles of oxygen needed to complete the reaction
56
Oxidation:
Loss of electrons
57
Reduction:
Gain of electrons
58
OIL-RIG:
Oxidation is loss (of an electron) | Reduction is gain (of an electron)
59
These elements, when they exist outside of a compound in their natural state, are always in pairs:
Hydrogen, bromine, oxygen, nitrogen, iodine, and fluorine.
60
Series of rules to identify the oxidation states of all elements in the compound:
1. The charge or number of any element in it's natural state is zero. 2. The oxidation number of any simple ion is the charge of the ion 3. The oxidation number for oxygen in a compound is (-2) 4. The oxidation number for hydrogen in a compound is (+1) 5. The sum of the oxidation numbers equals the charge on the molecules or polyatomic ions
61
Acids:
- Corrosive to metals - Change blue litmus paper red - Become less acidic when mixed with bases - Hydrogen or proton donors
62
Bases:
- AKA alkaline compounds - Denature proteins - Change red litmus paper blue - Become less basic when mixed with acids - Hydrogen or proton acceptors
63
Chemical reactions:
Atoms are trying to reach stable electron configurations
64
Nuclear reactions:
Concerned with reactions that take place in the nucleus to obtain stable nuclear configurations
65
Radioactivity:
The emission of particles and/or energy (radiation) from an unstable nucleus
66
3 types of radiation in nuclear chemistry:
Alpha, beta, gamma
67
Alpha radiation:
- Emission of helium nuclei consisting of 2 protons and 2 neutrons (+2 charge) - Can be stopped by sheet of paper
68
Beta radiation:
- Composed of high-energy electrons that are the product of the decomposition of a neutron or proton - Can be stopped by thin sheet of aluminum foil, lucite, or plastic
69
Gamma radiation:
- High-energy electromagnetic radiation | - Can go through concrete and lead
70
Unstable atoms decay until...
It finds a stable nuclear configuration by emitting radioactive particles
71
Biochemistry:
Study of chemical processed in living organisms
72
Function of carbohydrates:
To store and provide energy for the body
73
Monosaccharides:
- Simplest type of carbohydrate | - Contain carbon, hydrogen, and oxygen in a ratio of 1:2:1
74
2 types of monosaccharides:
- Glucose and fructose | - Both are a six-carbon sugar called a hexose
75
Disaccharides
Consists of 2 monosaccharides joined together
76
2 types of disaccharides:
Sucrose (glucose + fructose) | Lactose (glucose + galactose)
77
Oligosaccharides:
3-6 monosaccharides joined together
78
Polysaccharides:
More than 6 and up to thousands of monosaccharides joined together-> called a starch
79
2 common polysaccharides:
Cellulose (made by plants) | Glycogen (made by animals)
80
Glycolysis:
Chemical pathway in the body that metabolizes glucose
81
Net result of glycolysis:
2 pyruvate | 2 ATP
82
Anaerobic glycolysis:
Converts glucose to lactate instead of pyruvate as in aerobic glycolysis
83
Gluconeogenesis:
Process where the liver makes glucose from proteins and fats
84
Amino acids:
Composed of a carbon atom bonded with four other groups: amine, carboxyl, hydrogen, and an R group
85
Dipeptide:
Union of 2 amino acids using a peptide bond
86
Peptides/polypeptides:
Groups of fewer than 30 amino acids joined together
87
Fatty acids:
Consist of a hydrocarbon chain with an acid group ( the carboxyl group) at one end
88
Triglycerides:
Neutral fat that is joined by 3 fatty acids joined to a glycerol/backbone structure
89
Phospholipids:
Consists of 2 fatty acid chains and a phosphate group
90
Cholesterol:
Composed of a 4-ring structure and a side chain
91
Function of fats:
- Insulates body organs against shock - Maintain body temp - Keep skin and hair healthy - Promotes healthy cell function - Energy stores
92
Phospholipid function:
Essential component of cell membrane
93
Cholesterol:
Precursor for many important biological molecules such as steroids
94
Natural lipids are classified as:
Unsaturated, polyunsaturated, and saturated
95
Saturated fats:
No double bonds between carbon atoms of the fatty acid chains
96
Unsaturated fats:
One or more double bonds between carbon atoms of the fatty acids chains
97
Nucleic acids are found:
In all living cells and viruses
98
DNA structure:
Composed of deoxyribose and a phosphate
99
Amphoretic:
..
100
Pentose:
5 carbon sugar
101
Ribose:
5 carbon carbohydrate

HESI (18 decks)

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