Chapter 2. Life s chemical basis
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1 Chapter 2 Life s chemical basis
2 Start With Atoms CHARACTERISTICS OF ATOM Atom Building blocks of all substances They consist of 3 subatomic particles- Protons, Electrons, Neutrons Protons - positive charge Electron - negative charge Neutrons - neutral charge All atoms have a nucleus
3 Atoms
4 nucleus electron
5 Start With Atoms Element They are pure substances Each element is made up of atoms of the same type Example : Element Oxygen is made up of Oxygen atoms
6 Start With Atoms Atomic Number The number of protons,which is unique to that element Example: Element Carbon has six protons in its nucleus, so the atomic number is 6 Mass Number Total number of protons and neutrons
7 Start With Atoms Isotopes All atoms of that element that differ in their number of neutrons Example: Periodic table 13 6 C, 6C, C Dmitry Mendeleev arranged the periodic table based on the chemical properties. Symbol for each element is an abbreviation of its name (1or 2 letters of the element Elements in the far right column of the table are inert gases.
8 Periodic Table of Elements
9 Putting Radioisotopes To Use Radioisotopes The atoms of radioisotopes spontaneously emit subatomic particles or energy when their nucleus break This decay can transform one element to another Example Radioactive carbon decays to form nitrogen. Uses To estimate the age of rocks and fossils Researchers and clinicians use radioactive isotopes in living organisms Radioisotopes have uses in medicine, PET scan.
10 Why Electrons Matter Electrons and energy levels Electrons occupy in different orbital around the nucleus Shells and electrons Help us to check an atom for vacancies. Represent the orbital energy level as successively larger circles or shells Used to view an atoms electron structure.
11 electron Third Shell - Greatest Energy sodium chlorine 11p+, 11e - 17p+, 17e - argon 18p+, 18e - Second shell- More energy carbon oxygen 6p+, 6e - 8p+, 8e - neon 10p+, 10e - First shell- Lowest energy hydrogen 1p+, 1e - helium 2p+, 2e -
12 Why Electrons Matter Atoms and Ions Atoms An atom with equal number of protons and electrons has no net charge. Ions An atom that have gained or lost electrons. An ion is an atom that carries a charge, it acquires a negative charge by pulling an electron away from other atom or it acquires a positive charge by losing an electron.
13 Ion Formation
14 Why Electrons Matter Electronegativity It is the measure of atom s ability to pull electrons from other atoms. From atoms to molecules A chemical bond is an attractive force that arises between two atoms when their electrons interact Molecule - It is formed when two or more atoms of same or different element join in chemical bonds.
15 Why Electrons Matter Compounds- They are molecules that consist of two or more different elements in proportions that do not vary. Example Water(H2O), It has 1 Oxygen atom bonded to 2 Hydrogen atoms. Mixtures-Two or more substances intermingle, but do not bond with each other. Example - Sugar and water.
16 What Happens When Atoms Interact?
17 What Happens When Atoms Interact? Types of Bond Ionic bond Covalent bond Hydrogen bond
18 Ionic Bonds Strong association between a positive ion and a negative ion (attraction of opposite charges)
19 What Happens When Atoms Interact? Covalent bond two atoms share a pair of electrons Polar covalent bond two atoms do not share electrons equally (oxygen is partial negative and hydrogen is partial positive) Example - Water molecule Non-polar covalent bond atoms share electrons equally Example - molecular Hydrogen, Oxygen
20 Molecular hydrogen (H H) Two hydrogen atoms, each with one proton, share two electrons in a single nonpolar covalent bond. Molecular oxygen (O O) Two oxygen atoms, each with eight protons, share four electrons in a nonpolar double covalent bond.0 Water molecule (H O H) Two hydrogen atoms each share an electron with an oxygen atom in two polar covalent bonds. The oxygen exerts a greater pull on the shared electrons, so it has a slight negative charge. Each hydrogen has a slight positive charge.
21 What Happens When Atoms Interact? Hydrogen Bond Formed Between a Hydrogen atom and an electronegative atom Example - Bond between two water molecules, and between water and ammonia
22 Hydrogen Bonds
23 Water s Life Giving Properties Polarity of water molecule polarity of each molecule attracts other water molecules Hydrophilic substance (water-loving) - any substance that has an affinity for water Example - Water forms hydrogen bonds with sugar and other water molecules Hydrophobic substance (water-dreading) - substances that do not have an affinity for water Example - Salad oil
24 Polarity of water molecule
25 Water s Life Giving Properties Water s temperature-stabilizing effects Temperature It is a way to measure of energy of molecular motion Evaporation heat energy converts liquid water to a gas Water s solvent property Solvent substances that dissolve other substances Solute the substance that is dissolved
26 Water s Life Giving Properties Sphere of hydration clustering of water molecules around a solute Example - Pour table salt into a cup of water Water s cohesion molecules resist separating from one another Example - Tossing a pebble into a pond
27 Water s Solvent Properties Solvents dissolve solutes (spheres of hydration)
28 Water s Cohesion
29 Acids and bases The p H scale measures Hydrogen ion concentration in a solution greater the H+ concentration less is the p H, and vice versa At p H 7 (neutral) H + and OH concentrations are equal The difference between acids and bases Acids donate Hydrogen ions Example - Lemon juice, coffee Bases accept Hydrogen ion as they dissolve in water Example - Seawater, egg white
30 Red Dots-Hydrogen (H +) battery acid gastric fluid acid rain lemon juice cola vinegar orange juice tomatoes, wine bananas beer bread black coffee urine, tea, typical rain corn butter milk pure water blood, tears egg white seawater baking soda phosphate detergents Tums Blue Dots-Hydroxyl (OH-) toothpaste hand soap milk of magnesia household ammonia hair remover bleach oven cleaner drain cleaner
31 Acids and bases Salt and water Salt any compound that dissolves easily in water and releases ions other than H + and OH -. Example: NaCl HCl + NaOH NaCl + H 2 O It is formed when acid interacts with base
32 Acids and bases Buffers substances that minimize changes in concentrations of H + and OH - in a solution Buffering system set of chemicals that keeps the p H of a solution stable
33 Functions of Buffer Systems Buffers help maintain homeostasis Most biological processes proceed only within a narrow p H range, usually near neutrality Acidosis Alkalosis
34
35
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