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Summer 24 > Chem Chap 2 > Flashcards

Chem Chap 2 Flashcards

1
Q

What is chemistry?

A

Study of matter and changes it undergoes

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2
Q

What is physics?

A

Study of motion, matter and energy interactions

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3
Q

What is a Atom?

A
  • building block of matter
  • atoms are the smallest particle of an element that can enter into a chemical reaction
  • Composed of protons, neutrons, electrons
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4
Q

Chemical Properties

A

Characteristics that describe the chemical reactivity of a substance. Chemical reactions result formation of different compounds

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5
Q

Physical properties

A

Do not describe the chemical reactivity of a substance. A substance can display properties without a change in composition

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6
Q

The atomic number

A
  • The number of protons in the nucleus
  • determines the identity of the atom
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7
Q

The mass number

A
  • the sum of proton number (or atomic number) and the neutrons
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8
Q

What is the Atomic mass/ Atomic weight

A

average mass of an atom in a natural sample of the element

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9
Q

Isotope

A
  • atoms with the same atomic number but with different atomic weights
  • structural variations of an atom
  • have the same number of protons (and electrons) but a different number of neutrons
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10
Q

Radioisotopes

A
  • heavier, unstable isotopes of an element that spontaneously decompose into more stable forms
  • half life- time required to lose 1/2 of radioactivity
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11
Q

What is Daltons Theory

A
  • proposes three hypothesis to explain laws of conservation of mass and definite proportions
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12
Q

Daltons first theory

A
  • each element is composed of tiny, indivisible particles called atoms, which are identical for the element but are different (particularly their masses and chemical properties) from atoms of other elements
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13
Q

Daltons Second theory

A
  • Chemical combination is simply the bonding of a definite, small whole number of atoms of each of the combining elements in a fixed ratio to make one molecule of the formed compound. A given compound always has the same relative numbers and types of atoms
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14
Q

Daltons Third theory

A
  • no atoms are gained, lost, or changed in identity during a chemical reaction; they are just rearranged to produce new substances
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15
Q

Law of conservation of mass

A

no detectable change in the total mass occurs during a chemical reaction. This law was proposed by Antoine Lavoisier

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16
Q

Law of Definite proportions

A

different samples of pure compound always content the same elements in the same proportionably mass
- water always contains 11.2% hydrogen and 88.8% oxygen

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17
Q

Who was Dmitri Mendeleev

A
  • Russian who constructed the periodic table of elements, emphasizing that chemical and physical properties are repeated in a predictable way
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18
Q

Rows on periodic table are called _____?

A

periods

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19
Q

Columns are called ___?

A

Groups or families
(elements within a family have similar chemical and physical properties)

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20
Q

What is periodic law

A

properties of elements are periodic functions of their atomic numbers

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21
Q

What is a covalent bond

A
  • molecule is a group of atoms chemically bonded together into a discrete unit
  • Sharing electrons
  • Covalent = Close on the periodic table (generally rule formed by elements on the right side of periodic table)
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22
Q

What are ionic compounds

A

compounds that are held together by ionic bonds or the attraction or oppositely charged ions
- in solid states ionic compound form crystalline lattices
- cations are attracted to all the neighboring anions not just one
- there are no discrete ionic “molecules”
- transfer of electron

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23
Q

Chemical Bonds

A
  • an energy relationship between the electrons of the reacting atoms
  • bonds are formed using the electrons outermost energy level (valence shell)
24
Q

Valence Shell

A
  • outermost energy level containing chemically active electrons
25
Q

Octet Rule (rule of 8)

A

except of the first shell which is full with two electrons, atoms interact in a manner to have eight electrons in their valence shell

26
Q

Chemically Inert elements

A

have their outermost energy level fully occupied by electrons

27
Q

Chemically Reactive elements

A

elements that do not have either outermost energy level fully occupied by electrons

28
Q

Types of chemical bond

A
  • ionic
  • covalent
  • hydrogen
29
Q

Ionic Bonds

A
  • chemical bonds that form between two atoms that transfer one or more electrons from one atom to other
  • ions are charged particles
30
Q

Anion

A

electron acceptor carrying a net negative charge due to the extra electron
- formed by gain of electrons
- nonmetals tend to form anions
- electron acceptor

31
Q

Cation

A

electron donor carrying a net positive charge due to the loss of an electron
- formed by loss of electron
- metals tend to form cations

32
Q

Crystals

A

large structures of cations and anions held together by ionic bonds
Ex NaCl

33
Q

Nonpolar molecules

A
  • equal sharing of electrons
  • no poles
  • ex CO2
  • charge is balanced
34
Q

Polar molecules

A
  • unequal sharing of electrons
  • creates a charged particle
  • ex H2O
35
Q

Hydrogen bonds

A

weak attractions that form between partially charged atoms found in polar molecule
- common in dipoles (water)
- responsible for surface tension
- important as intramolecular bonds giving the molecule a three dimension shape
- hydrogen bonds tend to collapse the lung

36
Q

Ions

A
  • atom or group of atoms with a charge
  • cannot cross the cell membrane
37
Q

Molecular compounds

A

made of discrete units (molecules) and usually consist of a small number of nonmetals atoms held together by covalent bonds

38
Q

Hydrates

A
  • some ionic compounds incorporate a fixed number of water molecules into their formula unit
39
Q

Desiccants

A
  • the anhydrous form of a compound that has a strong tendency to form a hydrate and is used to scavenge the last traces of water from a system
  • most commonly used is silica gel (SiO2)
  • addition of water to a desiccant is a reversible process so saturated desiccants can be used as moisturizers
40
Q

Moles

A
  • amount of substance that contains exactly as many particles at 12.00 grams of carbon
  • this number is called Avogadros number (6.02x10^23)
  • particles can be molecules, atoms, ions or electrons
  • molecular mass is the sum of the masses of the component atoms
41
Q

Avogrados number

A

6.02x10 ^23

42
Q

water always contains ___% hydrogen

A

11.2%

43
Q

water always contains ____% oxygen

A

88.8%

44
Q

What are the big 4 elements? What percentage do they make up in our body?

A
  • oxygen
  • carbon
  • Hydrogen
  • Nitrogen
  • 96.1 %
45
Q

Ph is controlled by what element?

A

Hydrogen

46
Q

Fe++ (ferrous) vs Fe+++ (Ferric)

A
  • Ferrous is good
  • Ferric is bad form because it decreases the hemoglobin affinity for oxygen
47
Q

What clotting factor is calcium involved in?

A

Factor IV

48
Q

what percentage of the air does Nitrogen make up?

A

80%

49
Q

What percentage of Oxygen makes up the air?

A

20%

50
Q

What is the most abundant intracellular ion?

A

Potassium

51
Q

What is the most abundant extracellular ion?

A

Sodium

52
Q

How do you calculate molecular mass?

A

the sum of the masses of the component atoms

53
Q

Compare and contrast mixtures and compounds

A

No chemical bonding takes place in mixtures, most can be separated by physical means, and mixtures can be heterogeneous or homogeneous.
-Compounds cannot be separated by physical means and all compounds are homogeneous.

54
Q

What are the 4 major elements in the body and their percentage? Functions?

A

Oxygen-65% it is needed for cellular energy (ATP)
Carbon-18.5% a primary component of all organic molecules
Hydrogen-9.5% a component of all organic molecules, as a proton it influences the pH of body fluids.
Nitrogen-3.2% a component of proteins and nucleic acids (genetic material).

55
Q

What are the 9 lesser elements in the body and their percentage? Functions?

A

-Calcium-1.5% found as salt in bones and teeth, its ion form is required for muscle contraction, conduction of nerve impulses, and blood clotting.
-Phosphorus-1.0% part of calcium phosphate in teeth and bones, also present in nucleic acids and part of ATP.
-Potassium-0.4% most abundant ICF cation, required for conduction of nerve impulses and muscle contraction.
-Sulfur-0.3% component of proteins, particularly muscle proteins.
-Sodium-0.2% most abundant ECF cation, required for water balance, conduction of nerve impulses, and muscle contraction.
-Chlorine-0.2% most abundant ECF anion.
-Magnesium-0.1% present in bone, important cofactor in metabolic reactions.
-Iodine-0.1% needed to make thyroid hormones
-Iron-0.1% component of hbg and some enzymes

56
Q

What is methemoglobinemia? Treatment?

A

When ferrous (good form) is converted to ferric (bad form) it causes inability for O2 to be transported, pt will become hypoxic. Give IV methylene blue. Can be caused by some local anesthetics

57
Q

Role of surfactant in body?

A

Surfactant decreases surface tension in lungs for expansion during inhalation and prevents alveolar collapse during exhalation. Surfactant acts as a soap or detergent and breaks hydrogen bonds in lungs.

Summer 24 (17 decks)

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