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Biology 2401 103 > Charter 2. Chemistry > Flashcards

Charter 2. Chemistry Flashcards

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1
Q

Matter

A

•Anything that has mass and occupies space.
-Matter can be seen, smelled and/or felt
-Weight is mass plusses effects of gravity

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2
Q

States of matter

A

Matter can exist in 3 possible states:
Solid:definite shape and volume
Liquid:changeable shape; definite volume
Gas:changeable shape and volume

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3
Q

Energy

A

•The capacity to do work or put matter into motion
•Energy does not have mass, nor does it take up space
•What gives each element its particular physical and chemical properties

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4
Q

Structure of Atoms

A

Atoms are composed of 3 subatomic particles (protons, neutrons and electrons).

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5
Q

Protons

A

▪︎Carry a positive charge (+)
▪︎Weigh an obituary 1 atomic massage unit (1amu)

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6
Q

Electrons

A

▪︎Carry a negative charge (-)
▪︎Are so tiny they have virtually no weight (0amu)

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7
Q

Types of chemical bonds

A

3 types if chemical bonds
-Ionic Bonds
-Covalent Bonds
-Hydrogen Bonds

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8
Q

Ionic bonds

A

Atoms that have gained or lost electrons and become charged
▪︎Number of protons does not equal number of electrons
-Involve the transfer of valence shell electrons from 1 atom to another, resulting in ions

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9
Q

Ionic bonds pt.2

A

1 becomes an anion (negative charge)
-Atom that gained 1 or more electrons
▪︎1 becomes a cation (positive charge )
-Atom that lost 1 or more electrons
-Attraction of opposite charges results in an ionic bond
▪︎Most ionic compounds are salts

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10
Q

Covalent bonds

A

Formed by sharing of 2 or more valence shell electrons between 2 atoms.
▪︎Sharing of 2 electrons results in single bond
▪︎Sharing of 4 electrons is a double bond
▪︎Sharing of 6 electrons is a triple bond
-Allows each atom to fill its valence shell to atleast part of the time
-2 types of covalent bonds
▪︎polar and nonpolar covalent bonds

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11
Q

Non polar covalent bonds

A

▪︎Equal sharing of electrons between atoms
▪︎Results in electronically balanced, non polar molecular such as co2

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12
Q

Polar covalent bonds

A

-Unequal sharing of electrons between 2 atoms
-Results in electronically polar molecules
▪︎Atoms have different electron-attracting abilities, leading to unequal sharing.
▪︎Atoms with greater electron-attraction ability are electronegative and those with less are electropositive

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13
Q

Hydrogen bonds

A

An attraction between 2 atoms that already participate in other chemical bonds. 1 of the atoms is hydrogen while the other may be an electromagnetic atom such as oxygen, chlorine or fluorine.

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14
Q

Water

A

•Polar solvent properties
-Dissolves and disassociates ionic substances
-Forms hydrogen (water) layers around large charged molecules
▪︎Example:proteins
-Body’s major transport medium

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15
Q

Carbohydrates

A

•Include sugars and starches
•Contain C,H and O
-Hydrogen and oxygen are in 2:1 ratio
•3 classes (Monosaccharides, disacharides and polysaccharides)
Monosaccharides have 1 single sugar (Monomers: smallest unit of carbohydrate)
Dissacharides: 2 sugars
Polysaccharides: many sugars

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16
Q

Lipids

A

•Contain C,H,O but less than in carbs and sometimes contain p
•Insulable water
•Maintypes:
-Triglycerides
-pHospHolipids
-Steroids
-Eicosanoids

17
Q

Proteins

A

•Comprise 20-30% of cell mass
•Have most varied functions of any molecules
-Structural, chemical (enzymes), contraction (muscles)
•Contain C,H,O,N and sometimes s and p
•Polymers and amino acid monomers held together by peptides bonds
•Shape and functions due to 4 Structural levels

18
Q

Nucleic acids

A

•Composed of C,H,O,N and P are the largest molecules in the body
•Nucleic acid polymers are made up of monomers called nucleic nucleotides
-Composed of nitrogen base, a pentose sugar and pHospHate group
•2 major classes
-Deoxyribonucleic acid (DNA)
-Ribonucleic acid (RNA)

19
Q

DNA

A

Holds genetic blueprint for the synthesis of all proteins
-Double stranded helical molecule (Double helix) located in cell nucleus
-Nucleotides contain a deoxyribose sugar, pHosPhate group and 1 or 4 nitrogen bases
▪︎purinesiodenine (A), guanine (G), pyrimidines, cytosine (C) and thymine (T)

20
Q

DNA pt.2

A

▪︎Follows complementary base-painting rules:
-A always pairs with T
-G always pairs with C

21
Q

RNA

A

Links DNA to protein synthesis and is slightly different from DNA
-Single stranded linear molecule is active mostly outside the nucleus
-Contains ribose sugar (not deoxyribose)
-Thymine is replaced with uracil
-3 varieties of RNA carry out DNA orders for protein synthesis
▪︎Messenger RNA (mRNA), transfer RNA (tRNA) and ribosomal RNA (rRNA)

22
Q

Inorganic compound/molecules (Water)

A

Most abundant inorganic compound
-Accounts for 60% -80% of the volume of living cells
•Most important important inorganic compound because of its properties
-High heat capacity, high heat vaporization, polar solvent properties, reactivity and cushioning

23
Q

Inorganic compound/molecules (Cations)

A

Negative oxygen regions of polar water molecules are attracted to Na+Cations (positively charged)

24
Q

Inorganic compound/molecules (Anions)

A

Positive hydrogen regions of polar water molecules are attracted to Cl-anions (negatively charged)

25
Q

Dehydration and hydrolysis

A

•Organic molecules contain carbon
-Exceptions: CO2 and CO, which are inorganic
•Carbon is Electroneutral
-Shares electrons ; never gains or loses them
-Forms 4 covalent bonds with other elements
-Carbon is unique to living systems
•Major organic compounds: carbohydrates, lipids, proteins and nucleic acids

26
Q

Dehydration synthesis

A

Monomers are joined ny removal of H from the other at the site of bond transformation

27
Q

Hydrolysis

A

Monomers are released by the addition of a water molecule, adding OH to 1 monomer and H to the other

28
Q

Water role in cellular metabolism

A

•Reactivity
-Necessary part of hydrolysis and dehydration synthesis reactions
•Cushioning
-Protects certain organs from physical trauma
▪︎Example: cerebrospiral fluid cushions nervous system organs
-Polar solvent properties: Dissolves and dissociates ionic substances and forms hydration (water) layers around large charged molecules
▪︎Example: proteins

29
Q

pH acid base concentration

A

pH scale is measurement of concentration hydrogen ions [H+] in a solution
-The more hydrogen ions in a solution, the more acidic that solution is
-Ph is negative logarithm of [H+] in moles per liter that ranges from 0-14
-pH scale is logarithmic, so each pH unit represents a 10-fold difference
▪︎Example: a pH 5 solutions is 10 times more acidic than a pH 6 solution

30
Q

pH acid base concentration (cont.)

A

-Acidic solutions have high [H+] but low pH
▪︎Acidic pH range is 0-6.99
-Neutral solutions have equal numbers of H+and OH- ions
▪︎All neutral solutions are pH7
▪︎Pure water is pH Neutral
-pH of pure water is pH7: [H+] = 10-7m
-Alkaline (basic) solutions have low [H+] but high pH
▪︎Alkaline pH range is 7.01- 14

31
Q

Protein role in cellular life

A

Compose 20%-30% of cell mass
•Have most varied functions of any molecular structure
-Structural, chemical (enzymes), contraction (muscles)
•Contain C,H,O,N and sometimes S and P
•Polymers of amino acids monomers held together by peptide bonds
•Shape and function due to 4 structural levels

32
Q

Protein role in cellular life cont.

A

•Structural protein function
-mechanical support
•Enzyme protein
-catalysis in protein enzymes are essential for virtually every biochemical reaction in the body
•Transport protein
-moving substances (In blood across plasma membranes)
•Communication proteins
-transmitting signals between cells. Can act as chemical messengers (e.g. hormones) or as receptors in plasma membranes
•Defensive proteins
-protect against disease

33
Q

Central dogma of molecular biology

A

A theory that genetic information flows only in 1 direction, from DNA, to RNA to protein or RNA directly to protein

Biology 2401 103 (2 decks)

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