Download Chapter 2 pp 31-38 Anatomy Notes more complete

Anatomy Notes
Chapter 2 pp 32-38 to Acids and Bases
Chemistry Review- completed for class 9/19 and 9/21/14
Trace elements:
Trace elements in the human body: Cr,Co,Cu,F,I,Fe,Mn,Zn- together less that 0.1%
Trace element
Zn
RDA or safe daily intake
12 mg
(-)
poor growth, skin
rash,enlarged liver and
spleen, lethargy
Fe
15mg
anemia, low levels
hemoglobin
I
150mg
Goitre(Fxn-syn of
thyroid hormone)
Acrodermititus
Cu
1.5-3.0 mg/day
anemia/poor wound
healing,dep. Collagen
synthesis
F
1.4-4.mg/day
tooth decay
Mn
2.0-5.0mg/day
abnormal growth of
bone/conn tissue
Cr
50-100 micrograms/day
fxn; acts as a cofactor to
insulin
Mo
70-200 micrograms/day
no clear cut symptoms
Fxn;agent for electron
transfer
Food Sources
Zn, Cu,:
dairy, meat,fish,eggs, potatoes,grains,lentils
Mn:
nuts, unrefined grains
Mg:
whole grain cereals,green veg
Mo
dried legumes,grains,cereal prods, organ meats
F:
drinking water,seafish,tea
I;
iodized salt, seafood
2.1 Introduction
Prefix meanings
di-2
gly-sweet
lip-fat
lyt-dissolvable
mono-1
poly-many
sacchar-sugar
syn-together
iso-equal
nucle-kernel
valent-having power
Human body composed of chemicals
Salts
Water
Proteins
Carbohydrates
Nucleic acids
All food, liquids, medications-chemicals
Elements and Atoms
2.2 Matter
Matter-anything that has weight and takes up space, s,l,g in surroundings and inside
the body.
Element-Pure chemical substance made of only one type of atom.
Living organisms requires about 20 elements; O, C, H and N- make up more
than 95% by wt of the human body.
Atom- The smallest particle of an element that has the properties of that element.
Chemical bonds-The attractive forces between atoms.
Atomic Structure
Nucleus- The central portion of an atom. It contains protons and neutrons.
Electron- Extremely small particle; carries a negative charge and is in constant
motion around the nucleus of an atom.
Proton- Relatively large particle; carries a positive charge and is found within the
nucleus of an atom.
Neutron- Relatively large particle; uncharged and thus electrically neutral; found
within the nucleus of an atom.
Electron-Extremely small particle; carries a negative electrical charge and is in
constant motion around the nucleus of an atom.
Because the nucleus contains the protons- it is always (+) charged.
The # of electrons outside the nucleus = the # of protons, therefore the complete
atom is electrically neutral or uncharged.
Atoms of different elements have different #of protons.
Atomic #- the # of protons in a particular element.
Atomic weight-the atomic weight of an atom of an element is = to approximately
the number of protons + number of neutrons in it’s nucleus; electrons have very
little weight.
All atoms of the same elements have the same number of protons and electrons.
However….atoms of an element may vary in the number of neutrons n their nuclei
and therefore have different atomic weights…. Isotopes.
Isotopes
Isotope-Atoms with the same atomic # but different atomic weights.
Ex. All Oxygen atoms have 8 protons but some may have 8,9,or 10 neutrons,
therefore their weights would be 16,17,18.
Atoms reactivity depends upon the # of electrons.
Characteristics of isotopes:
Isotopes have the same # of electrons so reactivity is the same.
Isotopes may be stable or unstable
Unstable isotopes- has atomic nuclei that decompose, releasing energy
or pieces of themselves.
Unstable isotopes are called radioactive because they emit energetic particles, and
the energy or atomic fragments they give off are called radiation.
3 forms of radiation:
Alpha- particles from nuclei consist of 2P and 2N, travel slowly and are weak.
Beta- consists of electrons that travel more rapidly and penetrate more deeply.
Gamma- similar to x-rays- most penetrating form.
Each kind of radioactive isotope produces 1 or more forms of radiation and each
becomes less radioactive at a particular rate.
Half-life- the time required for an isotope to lose one half of it’s radioactivity.
Bonding of Atoms
Bonds
Covalent- share electrons
Single
Double
Triple
Polar- uneven sharing- one end of the molecule has more of its
share of electrons. Typically H bonds to O or N called a
Hydrogen bond. Weak, particularly at room T. At 0 degrees
form ice, as the T rises molecular movement begins and the Hbonds are broken, ice turns back into water.
Hydrogen bonds are very important in protein and nucleic acid
structure.
Ionic- gains or loses electrons-anions (-) and cations (+).
Atoms attach to one another forming chemical bonds.
The chemical behavior of atoms results from interactions among their electrons.
When atoms form chemical bonds- they gain, lose or share electrons.
Electrons occupy shells around the nucleus.
Each shell can hold a certain number of electrons: remember electron
configurations?????? Electron capacity=2n2 where n= the energy level.
Level 1-2electrons
Level 2-8 electrons
Level 3-18 electrons
Level 4-32 electrons
Level 5-50 electrons
Level 6-72 electrons
Electrons in the outermost level or shell determine the atoms behavior.
Atoms, whose outermost shell is filled, have stable structures and are chemically
inactive- noble gases.
Atoms such as H or Li tend to gain, lose or share electrons to fill their shells.
Ions-atoms that gain or lose electrons become electrically charged are called ions.
Because oppositely charged ions attract, ex. Na+ and Cl- ions react to form a type of
chemical bond- ionic bond.
From here Notes are skipping pp 36-38…. I will go back and pick them up!
Acids and Bases
When ionically bonded substances dissolve in water, the slightly + and – ends of the
water molecule cause the ions to leave each other and interact with the water
molecules instead.
The polarity of the water dissociates the salts in the internal environment
(decomposition reaction).
NaClNa+ +ClSince the resulting solution contains electrically charged particle (ions) it will
conduct an electrical current.
Substances that release ions in water are called electrolytes.
Acids- electrolytes that release (H+) in water.
HClH++ClBase-electrolytes that release hydroxide ions. (OH-).
NaOHNa+ +OHThe hydroxide ions in turn can bond with H+ to form water.
The concentrations of H+ and the OHIn body fluids greatly affects the chemical reactions that control certain
physiological functions.
Since their concentrations are inversely relates…that is…as one goes up, the other
goes down, we need to keep track of one of them.
The pH scale measures H+ content.
Measures from 0-14, 7 being neutral (equal H+ and OH-).
0-------------------------14
Acid
Base
Each whole number on the pH scale represents a 10-fold difference in H+
concentration.
Human blood: pH 7.35-7.45
If pH goes down below 7.35-acidosis (can’t survive below 6.9)
If pH goes up above 7.8 alkalosis.
Homeostatic mechanisms maintain blood pH
MOLECULES AND COMPOUNDS
Molecule:
Compound:
FORMULAS
Structural:
Molecular:
REACTIONS
Synthesis;
Decomposition:
Exchange:
Reversible:
What is a catalyst?