Chapter 2 Flashcards
Matter
Anything that has matter and takes up space
Mass
the amount of matter a substance contains, whereas weight is the force of gravity acting on a mass
O
Oxygen
C
Carbon
H
Hydrogen
Na
Sodium
O, C, H, N
Make up the majority of elements in our body
Ca, P, K, S, Na, Cl, Mg and Fe
Make up lesser elements
Oxygen
65%
used to generate ATP, a molecule
used by cells to temporarily store chemical energy.
Carbon
18%
Forms backbone chains and rings of all organic molecules: carbohydrates, lipids (fats), proteins, and nucleIc acids (DNA and RNA)
Hydrogen
9.5%
Constituent of water and most organic molecules
Nitrogen
3.2%
Component of all proteins and nucleic acids
Atoms
the smallest units of matter that retain the properties and characteristics of an element
Subatomic particles in atoms
protons (p+), neutrons (n0) and electrons (e-)
Atomic number
the number of protons in the nucleus of an atom
Mass number
the number of protons and neutrons in an atom
Atomic mass/weight
the average mass of all its naturally occurring isotopes
Ion
an atom that has lost or gained an electron
Molecule
2 or more atoms sharing electrons
Compound
substance that can be broken down into 2 or more different elements
Free radical
is an atom or groups of atoms with an unpaired electron in the outermost shell
Antioxidants
substances that inactivate oxygen-derived free radicals
Chemical bond
Occurs when atoms are held together by forces of attraction
Cations elements
H+, Na+, K+, NH4+, Mg2+, Ca2+, Fe2+, Fe3+
Anions elements
F-, Cl-, I-, OH-, HCO3-, O2-, SO4 2-, PO4 3-
Ionic compounds exist as
Soilds
Ionic bonds are manly found in
Teeth and bones
Electrolytes form when
An ionic compound breaks apart in + or - ions in a solution
Covalent bonds
When 2 or more atoms share electrons rather than donating/receiving
Atoms form covalently bonded molecules by
Sharing one, two, or three pairs of valence electrons
What can covalent bonds form between
Two similar atoms or atoms of different elements
O=O
Total of 4 electrons will be shared
Nonpolar covalent bond
Atoms share electrons equally, hydrophobic
Polar covalent bond
Sharing of electrons between 2 atoms is unequal
Hydrogen bonds
Weak bonds that result from attraction of oppositely charges parts of molecules
Stabilize molecular structure of large molecules
Many hydrogen bonds together make them
Strong
Cohesion
the tendency of like particles to stay together
Hydrogen bonds between water molecules give
Water cohesion
Surface tension
a measure of the difficulty of
stretching or breaking the surface of a liquid
Created by hydrogen bonds
Chemical reactions occur when
new bonds are formed or old bonds are broken
Reactants
starting substances
Products
ending substances
Energy
the capacity to do work
Types of energy
❑ Potential energy
❑ Kinetic energy
❑ Chemical energy
Laws of conversation of energy
energy can neither be created nor destroyed but it can be converted from one form to another
Exergonic reactions
Release more energy than is consumes
Endergonic reaction
Use more energy than it produces
Activation reaction
Ensure more products will be formed, add energy
Types of chemical reactions
- Synthesis
- Decomposition
- Exchange
- Reversible
- Oxidation-reduction
Synthesis
A+B—>AB
Decomposition
AB—>A+B
Exchange
AC+BD—>AB+CD
Reversible
A+B<—>AB
Oxidation
Loss of electrons and energy release
Reduction
Gain of electrons and energy gain
Inorganic compounds
usually lack carbon and are simple molecules
Organic compound
always contain C, usually contain H, and always have covalent bonds
Water
the most important and abundant inorganic compound in all living things, has a high heat capacity, helps reduce friction as membranes
Hydrolysis reaction
Water is added to break bonds
Dehydration synthesis
Water is removed to break bonds
Mixture
combination of elements or compounds that are physically blended together but not bonded together
3 types of mixtures
- Solution
- Colloid
- Suspension
Acid
H+
1-6
Base
OH-
8-14
Salt
(+) + (-)
Buffer system
help to regulate pH by converting strong acids or bases into weak acids or bases
Helps maintain homeostasis
Enzymes
a catalyst in a living cell
Enzymes are:
❑ Highly specific
❑ Extremely efficient
❑ Subject to cellular controls
Organic compounds always contain
Carbon
Carbon compounds
do not dissolve easily in water
are a good source of energy
Carbohydrates
provide most of the energy needed for life
Monosaccharides
simple sugars that contain from 3 to 7 carbon atoms
Disaccharides
simple sugars formed from the combination of two monosaccharides by dehydration synthesis
Polysaccharides
from tens to hundreds of monosaccharides joined by dehydration synthesis
Glucose
The main blood sugar
Monosaccharides
Examples of monosaccharides
Glucose
Fructose
Galactose
Deoxyribose
Ribose
Examples of disaccharides
Sucrose
Lactose
Maltose
All steroids have
4 rings of carbon atoms, individual rings are designated by the letters A, B, C, D
Proteins
Give structure to the body, regulate processes, provide protection, assist in muscle contraction, transport substances, and serve as enzymes
Structural
Form structural framework of various parts of the body
Regulatory
Function as hormones that regulate various physiological processes; control growth and development; as neurotransmitters, mediate responses of nervous system
Contractile
Allow shorting of muscle cells, which produces movement
Immunological
Aid responses that protect body against foreign substances and invading pathogens
Transport
Carry vital substances throughout the body
Catalytic
Act as enzymes that regulate biochemical reactions
Amino acids
Proteins are formed by combining various amino acids
Peptide bonds
Help you determine what kind of protein it is
Primary structure
Amino acid sequence
Secondary structure
Twisting and folding of neighbouring amino acids, stabilized by hydrogen bonds
Tertiary structure
Three dimensional shape of polypeptide chain (final stage)
Quaternary structure
Arrangement of 2 or more polypeptide chains
DNA
Forms the genetic code in the nuclei of the body cells and it regulates most of the cells activities
RNA
Guides protein formation
DNA components
Cytosine
Thymine
Adenine
Guanine
RNA components
Cytosine
Uracil
Adenine
Guanine
Pentose sugar
A five carbon sugar called deoxyribose attaches to each base in DNA
Phosphate group
Alternate with pentose sugars to form the backbone of DNA strand
