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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). NaClNa+ +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. HClH++ClBase-electrolytes that release hydroxide ions. (OH-). NaOHNa+ +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?