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HESI > Chemistry > Flashcards

Chemistry Flashcards

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
Q

Adding a catalyst:

A

Reduces the activation energy or amount of energy necessary for a reaction to occur

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26
Q

Examples of catalyst:

A

Metals and proteins (enzymes)

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27
Q

Increasing the concentration causes:

A

More chance of collisions between the reactants, which produces more products

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28
Q

Solution:

A

Homogenous mixture of two or more substances

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29
Q

Solute:

A

Parts being dissolved

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30
Q

Solvent:

A

Part doing the dissolving

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31
Q

4 types of solutions:

A
  1. Compounds
  2. Alloys
  3. Amalgams
  4. Emulsions
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32
Q

Alloys:

A

Solid solution of metals to make a new one (Ex. copper + tin= bronze)

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33
Q

Amalgams:

A

A specific type of alloy in which a metal is dissolved in mercury

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34
Q

Emulsions:

A

Mixtures of matter that readily separate such as water and oil

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35
Q

Concentration is expressed as:

A

Weight per weight
Weight per volume
Volume per volume

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36
Q

A mole is:

AKA

A

6.02 x 10^23

Avogadro’s number

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37
Q

5 types of chemical reactions:

A
  1. Synthesis
  2. Decomposition
  3. Combustion
  4. Single replacement
  5. Double replacement
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38
Q

Synthesis:

A

Two elements combine to form a product

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39
Q

Decomposition:

A

Opposite of synthesis- breaking of a compound into its compound parts

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40
Q

Combustion:

A

Self-sustaining exothermic chemical reaction where oxygen and a fuel compound react

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41
Q

Single replacement:

A

Consist of an active metal reacting with an ionic compound containing a less active metal to produce a new compound

42
Q

Double replacement:

A
  • Involves two ionic compounds: the positive ion from one compound combines with the negative ion of the other compound
  • “Switching partners”
43
Q

2 types of chemical bonding:

A

Ionic and covalent

44
Q

Ionic bonding:

A
  • Electrostatic attachment between two oppositely charged ions (or a cation and an anion)
  • Formed between metal and nonmetal
45
Q

Covalent bonding:

A
  • Formed when two atoms share a pair of electrons with one pair from each atom
  • Formed between two nonmetals
  • Strongest bond
46
Q

Non-polar bond:

A

Electrons in a covalently bonded compound are shared equally

47
Q

Polar bond:

A

The shared electron density is concentrated around one atom more than the other (not equal)

48
Q

Intermolecular forces:

A

Weaker forces of attraction between whole molecules

49
Q

List 3 intermolecular forces:

A
  1. Hydrogen bonding
  2. Dipole-dipole interactions
  3. Dispersion forces
50
Q

Hydrogen bond:

A
  • The attraction for a hydrogen atom by a highly electronegative element
  • Strongest of all intermolecular forces
51
Q

Dipole-dipole interactions:

A

The attraction of one dipole on one molecule for the dipole of another molecule

52
Q

Dipole:

A

Separation of charges within a molecule between two covalently bonded atoms

53
Q

Dispersion forces:

A
  • 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
Q

Stoichiometry:

A

Quantities and numeric relationships of the participants in a chemical reaction

55
Q

Dimensional analysis:

A

Process used to determine the number of moles of oxygen needed to complete the reaction

56
Q

Oxidation:

A

Loss of electrons

57
Q

Reduction:

A

Gain of electrons

58
Q

OIL-RIG:

A

Oxidation is loss (of an electron)

Reduction is gain (of an electron)

59
Q

These elements, when they exist outside of a compound in their natural state, are always in pairs:

A

Hydrogen, bromine, oxygen, nitrogen, iodine, and fluorine.

60
Q

Series of rules to identify the oxidation states of all elements in the compound:

A
  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
Q

Acids:

A
  • Corrosive to metals
  • Change blue litmus paper red
  • Become less acidic when mixed with bases
  • Hydrogen or proton donors
62
Q

Bases:

A
  • AKA alkaline compounds
  • Denature proteins
  • Change red litmus paper blue
  • Become less basic when mixed with acids
  • Hydrogen or proton acceptors
63
Q

Chemical reactions:

A

Atoms are trying to reach stable electron configurations

64
Q

Nuclear reactions:

A

Concerned with reactions that take place in the nucleus to obtain stable nuclear configurations

65
Q

Radioactivity:

A

The emission of particles and/or energy (radiation) from an unstable nucleus

66
Q

3 types of radiation in nuclear chemistry:

A

Alpha, beta, gamma

67
Q

Alpha radiation:

A
  • Emission of helium nuclei consisting of 2 protons and 2 neutrons (+2 charge)
  • Can be stopped by sheet of paper
68
Q

Beta radiation:

A
  • 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
Q

Gamma radiation:

A
  • High-energy electromagnetic radiation

- Can go through concrete and lead

70
Q

Unstable atoms decay until…

A

It finds a stable nuclear configuration by emitting radioactive particles

71
Q

Biochemistry:

A

Study of chemical processed in living organisms

72
Q

Function of carbohydrates:

A

To store and provide energy for the body

73
Q

Monosaccharides:

A
  • Simplest type of carbohydrate

- Contain carbon, hydrogen, and oxygen in a ratio of 1:2:1

74
Q

2 types of monosaccharides:

A
  • Glucose and fructose

- Both are a six-carbon sugar called a hexose

75
Q

Disaccharides

A

Consists of 2 monosaccharides joined together

76
Q

2 types of disaccharides:

A

Sucrose (glucose + fructose)

Lactose (glucose + galactose)

77
Q

Oligosaccharides:

A

3-6 monosaccharides joined together

78
Q

Polysaccharides:

A

More than 6 and up to thousands of monosaccharides joined together-> called a starch

79
Q

2 common polysaccharides:

A

Cellulose (made by plants)

Glycogen (made by animals)

80
Q

Glycolysis:

A

Chemical pathway in the body that metabolizes glucose

81
Q

Net result of glycolysis:

A

2 pyruvate

2 ATP

82
Q

Anaerobic glycolysis:

A

Converts glucose to lactate instead of pyruvate as in aerobic glycolysis

83
Q

Gluconeogenesis:

A

Process where the liver makes glucose from proteins and fats

84
Q

Amino acids:

A

Composed of a carbon atom bonded with four other groups: amine, carboxyl, hydrogen, and an R group

85
Q

Dipeptide:

A

Union of 2 amino acids using a peptide bond

86
Q

Peptides/polypeptides:

A

Groups of fewer than 30 amino acids joined together

87
Q

Fatty acids:

A

Consist of a hydrocarbon chain with an acid group ( the carboxyl group) at one end

88
Q

Triglycerides:

A

Neutral fat that is joined by 3 fatty acids joined to a glycerol/backbone structure

89
Q

Phospholipids:

A

Consists of 2 fatty acid chains and a phosphate group

90
Q

Cholesterol:

A

Composed of a 4-ring structure and a side chain

91
Q

Function of fats:

A
  • Insulates body organs against shock
  • Maintain body temp
  • Keep skin and hair healthy
  • Promotes healthy cell function
  • Energy stores
92
Q

Phospholipid function:

A

Essential component of cell membrane

93
Q

Cholesterol:

A

Precursor for many important biological molecules such as steroids

94
Q

Natural lipids are classified as:

A

Unsaturated, polyunsaturated, and saturated

95
Q

Saturated fats:

A

No double bonds between carbon atoms of the fatty acid chains

96
Q

Unsaturated fats:

A

One or more double bonds between carbon atoms of the fatty acids chains

97
Q

Nucleic acids are found:

A

In all living cells and viruses

98
Q

DNA structure:

A

Composed of deoxyribose and a phosphate

99
Q

Amphoretic:

A

..

100
Q

Pentose:

A

5 carbon sugar

101
Q

Ribose:

A

5 carbon carbohydrate

HESI (18 decks)

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