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A & P - Chemisty > Elements and Atoms: Building Blocks of Matter > Flashcards

Elements and Atoms: Building Blocks of Matter Flashcards

1
Q

Matter

A

Anything that occupies space and has mass

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2
Q

Weight vs Mass

A

Mass - amount of matter contained in an object

Weight - an objects mass as affected by the pull of gravity

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3
Q

Element

A

A type of matter (pure substance) that cannot be created or broken down by ordinary chemical means (Carbon, Sulfur, Hydrogen, Oxygen, Nitrogen)

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4
Q

Compound

A

A substance composed of two or more (different) elements joined by chemical bonds. The elements that make up any given compound occur in the same relative amounts (ex. Glucose -> C6-H12-O6)

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5
Q

Atom

A

The smallest possible particle of an element that retains all of the properties of that element

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6
Q

Atomic Number

A

An atom of carbon is unique to carbon, but a proton of carbon is not. One proton is the same as another, whether it is in carbon, sodium, nitrogen (same for neutrons and electrons). The unique quantity of protons an element contains distinguishes it from other elements. No other element has exactly 6 protons in it’s atoms. Atomic number = number of protons.

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7
Q

Atomic Mass

A

Protons + Neutrons

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8
Q

Molecule

A

Two or more atoms chemically combined

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9
Q

Molecular Formula

A

A combination of symbols that indicates the number and type of atoms in a molecule (ex. H2O)

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10
Q

Structural Formula

A

Shows the arrangement of atoms/molecules

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11
Q

Valence Shell

A

An atom’s outermost electron shell. If the valence shell is full, the atom is stable and unlikely to be pulled away from the nucleus by the electrical charge of other atoms. If the valence shell isn’t full, the atom is reactive, meaning it will react with other atoms in ways that make the valence shell full.

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12
Q

Octet Rule

A

All atoms “want” to have a full outer shell which is 8 electrons (except for hydrogen and helium)

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13
Q

Bond

A

A weak or strong electrical attraction that holds atoms in the same vicinity

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14
Q

Ion

A

An atom that has an electrical charge - whether positive or negative.

Atoms typically have the same number of protons as electrons, however when an atom participates in a chemical reaction in order to have a full valence electron shell (octet rule) it’s number of protons and electrons will differ because it either donated or accepted electrons

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15
Q

Cation

A

A positively charged Ion

Ex. Potassium (K) has atomic number 19, just one electron in it’s valence shell. In chemical reactions it will lose an electron to have a full shell because that is easier than gaining 7. The loss of the negatively charged electron will cause the positively charged protons to be more influential than the remaining negatively charged electrons because there will be more protons than electrons. (K+)

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16
Q

Anion

A

A negatively charged Ion

Ex. Fluorine, atomic number 9, has 7 electrons in it’s valence shell. It is likely to bond with atoms in such a way that it gains one electron to have a full valence shell (octet rule) because that is easier than losing 7. When it does, it’s electrons will outnumber it’s protons by one, giving it an overall negative charge

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17
Q

Ionic Bond

A

An ongoing, close association between ions of opposite charge.

The opposite charges of cations and anions exert a moderately strong mutual connection that keeps atoms in close proximity forming an ionic bond. Ex. Sodium commonly donates an electron to chlorine, becoming Na+. When chlorine accepts the electron, it becomes Cl-. With their opposing charges, these two ions strongly attract each other (NaCl).

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18
Q

Electrolytes

A

Dissolved ions in a liquid state that produce electrical charges within the body

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19
Q

Covalent Bonds

A

Molecules formed by a covalent bond share electrons in a mutually stabilizing relationship

Electrons move back and forth between the elements. Because of the sharing of pairs of electrons (one electron from each of two atoms) covalent bonds are stronger than ionic bonds

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20
Q

Nonpolar Covalent Bonds

A

The sharing of the negative electrons between the atoms is relatively equal, as is the electrical pull of the positive protons in the nucleus of the atoms involved. That is why covalently bonded molecules that are electrically balanced in this way are described as non polar, that is, no region of the molecule is either more positive or more negative than any other

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21
Q

Polar Covalent Bonds

A

A molecule that contains regions that have opposite electrical charges. Polar molecules occur when atoms share electrons unequally.

Ex. Water (H2O) oxygen contains 8 protons and the two hydrogen atoms contain only 1. Because every proton exerts an identical positive charge, the nucleus that has 8 protons exerts a charge eight times greater than a nucleus that contains one proton. This means that the negatively charged electrons present in the water molecule are more strongly attracted to the oxygen nucleus than to the hydrogen nuclei. Each hydrogen atom’s single negative electron therefore migrated toward the oxygen atom, making the oxygen end of their bond slightly more negative than the hydrogen end of their bond

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22
Q

Hydrogen Bond

A

Formed when a weakly positive hydrogen atom already bonded to one electronegative atom is attracted to another electronegative atom from another molecule. Hydrogen bonds always include hydrogen that is already part of a polar molecule. Not an actual bond, an electrostatic attraction between two solar groups

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23
Q

Inorganic Compounds

A

A substance that does not contain both carbon and hydrogen

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24
Q

Organic Compound

A

A substance that contains both carbon and hydrogen

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25
Roles of Water
Lubricant and Cushion - just as oil lubricates the hinge on a door, water in synovial fluid lubricates the actions of body joints, helps the lungs expand and recoil, helps food flow through the digestive tract, endure abdominal organs are friction free Heat Sink - absorbs the heat generated by chemical reactions without greatly increasing in temperature. Can cool the body by allowing warm blood from the body’s core to flow to the blood vessels under the skin and transfer for it to the environment. Or, sweat glands can release water in sweat, carrying away heat from the body Component of Liquid Mixtures - works as a “universal solvent”, a water based liquid called a solution. Essentially all of the chemical reactions in the body occur among compounds dissolved in water
26
Dehydration Synthesis
Forms monomers into polymers. One reactant gives up an atom of hydrogen and another reactant gives up a hydroxyl group (OH) in the synthesis of a new product. In the formation of their covalent bond, a molecule of water is released as a byproduct, and the remaining monomers are left (Joins monomers into polymers). H——OH H——OH H——OH-H——OH ^ Forms water = H H2O OH
27
Hydrolysis
A molecule of water disrupts a compound, breaking its bonds. The water is itself split into H and OH. One portion of the severed compound then bonds with the hydrogen atom and the other portion bonds with the hydroxyl group
28
Polymer
A large molecule composed of many repeated subunits
29
Monomer
Small, simple molecules that are linked with other identical small, simple molecules to form polymers
30
Macromolecule
Large polymers Ex. Proteins, lipids, carbohydrates, nucleic acids
31
Salts
Formed when ions form ionic bonds (two groups of oppositely charged ions). A salt is a substance that when dissolved in water, dissociates into ions.
32
Acids and Bases
Like salts, dissociate in water into electrolytes. Acids and bases can very much change the properties of the solutions in which they are dissolved
33
Acid
A substance that releases hydrogen ions in solution. Because an atom of hydrogen has just one proton and one electron, a positively charged hydrogen ions is simply a proton. This solitary proton is highly likely to participate in chemical reactions. Strong acids, like hydrochloric acid, are compounds that release all of their H+ in solution, that is, they ionize completely. Weak acids do not ionize completely, some of their hydrogen ions remain bonded with a compound in solution.
34
Base
A substance that releases hydroxyl ions (OH-) in solution, or one that absorbs H+ already present in solution. The hydroxyl ions or other base combine with the H+ ions already present to form a water molecule, thereby removing H+ from the solution and reducing its acidity.
35
pH Scale
Measures relative acidity or alkalinity of a solution, or concentration of H+ (hydrogen ions). For example, a pH solution has a H+ concentration that is ten times greater than that of a pH 5 solutions (ten times more acidic). The lower the number below 7, the more acidic the solution, or the greater the concentration of H+. The higher the number above 7, the more basic (alkaline) the solution, or the lower the concentration of H+
36
Neutral pH
7 - pure water is pH 7
37
Buffer
A solution of a weak acid and it’s conjugate base. A buffer can neutralize small amounts of acids or bases in body fluids. Ex. If there is a slight decrease below pH 7.35 in the pH of a bodily fluid, the buffer in the fluid - in this case, acting as a weak base, will bind the excess hydrogen ions. In contrast, if pH rises above 7.45, the buffer will act as a weak acid and contribute hydrogen ions.
38
Carbohydrate
A molecule composed of carbon, hydrogen, and oxygen. Carbohydrates are referred to as saccharides, a word meaning “sugars”. Three forms are important in the body. Monosaccharides - monomers of carbohydrates. Disaccharides - made up of two monomers. Polysaccharides - polymers
39
Monosaccharides
Monomers of carbohydrates. Five are important in the body. ``` “Hexose sugars” -glucose -fructose -galactose “Pentose sugars” -ribose -deoxyribose ```
40
Disaccharides
A pair of monosaccharides. Formed via dehydration synthesis. Three are important: - sucrose - lactose - maltose
41
Polysaccharide
Contain a few to a thousand or more monosaccharides. Three are important: Starch- polymers of glucose. Plant based foods Glycogen- polymer of glucose, stored in the tissues of animals (muscles and liver) Cellulose- cell wall of green plants. Component of plant food referred to as “fiber”
42
Starch
Polymer of glucose - plants
43
Glycogen
Polymer of glucose - animals (tissues)
44
Cellulose
Polysaccharide that is primary component of cell wall in green plants, “fiber”
45
Functions of Carbohydrates
Energy/fuel - All body cells can use glucose for fuel. Nerve cells and red blood cells can ONLY use glucose for fuel. In the breakdown of glucose for energy, ATP is produced. ATP releases free energy when its phosphate bonds are broken, and thus supplies ready energy to the cells. Also present in cells. Some carbohydrate molecules bind with proteins to produce glycoproteins, others combine with lipids to produce glycolipids, both of which are found in the membrane that encloses the contents of body cells
46
Lipids
Fats, oils. Hydrophobic, do not dissolve in water.
47
Triglyceride
Glycerol (consists of 3 carbon atoms) + (bound by dehydration synthesis) 3 fatty acids =triglyceride - one of the most common dietary lipid groups
48
Phospholipid
A bond between the glycerol component of a lipid and a phosphorus molecule. Recall that triglycerides are nonpolar and hydrophobic. The same holds true for the fatty acid portion of the phospholipid, however the phosphate containing group at the head of the compound is polar and thereby hydrophilic. This is why they are components of the CELL MEMBRANE. They can interact with the watery interior of cells and the watery solution outside of cells. Also part of BILE
49
Steroid
Most important: cholesterol - hormones - vitamin D Also used in cell membrane (cholesterol)
50
Proteins
Organic molecules composed of one or more polypeptides chemically joined. Peptide Bond- bond between amino acids
51
Amino Acid
A molecule composed of an amino acid group and a carboxyl group, together with a variable side chain. 20 amino acids contribute to nearly all of the thousands of different proteins important in human structure and function
52
Peptide Bond
A covalent bond between two amino acids that forms by dehydration synthesis
53
Dipeptide
Two amino acids chemically joined by a peptide Bond
54
Tripeptide
Three amino acids chemically joined by a peptide Bond
55
Polypeptide
Multiple amino acids chemically joined by a peptide bond
56
Structural Proteins
H20 insoluble Fiberous Proteins -form structural material Ex. -Keratin - skin, hair, nails -collagen - tendons and ligaments, matrix of bone, connected tissue
57
Functional Proteins
Biochemically active a. Contractive Proteins (muscles) b. Messenger molecules (hormones) c. Immunity Proteins (antibodies) d. Transport Proteins - transport stuff around the body e. ENZYMES
58
Enzyme
A biological catalyst - (a substance that accelerates a chemical reaction without being consumed by the reaction) made of protein Substrate* - the material upon which an enzyme acts Hydrolysis Ex. Starch + H20 ————> glucose Amylase-enzyme (speeds up this reaction)
59
Nucleotide
Form energy carrying molecules - ATP: Adenosin Triphosphate - ADP: Adenosin Diphosphate P - S - B P: phosphate group S: 5 carbon sugar B: organic base
60
ATP
Holds energy that can be used by the cell P-P-P - S - B ——> “charged battery”
61
ADP
P-P | - S - B —> “dead battery”
62
Nucleic Acids
DNA + RNA - genetic material - protein synthesis

A & P - Chemisty (1 decks)

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