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Chemistry of Life

Explore the fundamental concepts of inorganic chemistry in relation to the chemistry of life. Learn about elements, atoms, isotopes, compounds, covalent and ionic bonds, molecules, mixtures, solutions, pH scale, polar and non-polar molecules, and the unique characteristics of water.

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Chemistry of Life

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  1. Chemistry of Life Inorganic Chemistry

  2. What is an element? • A Pure substance that contains on one type of atom. • There are 92 naturally occurring elements. • They are put together in the form of “The Periodic Table of the Elements”

  3. 96% of the mass of a human is made up of the following four elements: • Carbon (C) • Hydrogen (H) • Oxygen (O) • Nitrogen (N) • The one or two letter abbreviation is called the chemical symbol. • Sodium (Na) • Chlorine (Cl)

  4. What is an atom? • An atom is the basic unit of matter. • It includes a central nucleus which includes protons and neutrons. • Protons have a positive (+) charge and neutrons have a neutral charge.

  5. An electron cloud surrounds the nucleus. It is comprised of energy levels that contain electrons. • Electrons have a negative (-) charge.

  6. Each energy level can only hold a certain amount of electrons. • 1st : 2 electrons • 2nd : 8 electrons • 3rd : 8 electrons

  7. Atomic number: # of protons • Mass Number: # of protons + # of neutrons • Symbol: one or two letters representing the element

  8. Isotope- Same element but with a different number of neutrons • Protons stay the same, neutrons change. This means the mass number changes.

  9. Atoms of 2 or more different elements chemically joined together form a compound. • Examples of compounds: • Water (H2O) – hydrogen and oxygen bonded together • Table salt (NaCl) – Sodium and chloride bonded together

  10. Covalent bonds share electrons. • Example of covalent bonds is water (H2O). • Ionic bonds transfer electrons • Example of ionic bonds: table salt (NaCl).

  11. Molecule • Smallest particle of a substance; it retains its properties through composed of one or more atoms positively (+) or negatively (-) charged. • Ion: a charged particle (pos or neg)

  12. Mixture: substances or combined, but each keeps its own properties. • Example: saltwater, big mac • Solution: mixture of one or more substances (one being dissolved and the other does the dissolving) • Solute: substance being dissolved in a solution • Solvent: substance doing the dissolving in a solution

  13. Example of parts of a solution: • Lemonade=solution • Solvent=water • Solute=sugar/lemon juice

  14. pH • A measure of how acidic or basic a solution is. • 1-6 Acidic • 7 neutral • 8-14 Basic

  15. Acid • Below 7, More H+ than OH- • Ex: Lemon juice, milk, HCl

  16. Base • Above 7; less H+ than OH- • Ex: ammonia, drain – o , eggs, soap

  17. Neutral • pH = 7; equal amount of H+ and OH- • Ex: pure water.

  18. pH scale • Ranges from 0-14 • 0=strongest acid • 14=strongest base

  19. Polar molecule • Atoms in covalent bond that do not share electrons equally (has positive and negative ends) • Typically disolves in H2O. • Ex: Water, H2O

  20. Hydrogen bond • Weak bond created by a hydrogen atom attracted to oppositely charged atoms • Ex: Water, 2 hydrogens (+) + 1 oxygen (-) = H2O

  21. Non-polar molecule • Electrons are equally shared by atoms • Ex: O2, H2, CH4 (methane)

  22. Characteristics of Water: • Water is polar • Water resists temperature changes • Water expands when it freezes • Water is cohesive – it sticks to itself • Water is adhesive – it sticks to other stuff • Water has surface tension – Ex: a bug walks on water.

  23. Surface Tension • Water’s ability to stick to itself. • This causes some insects to walk on water, causes rain to form droplets and small objects to float on water. • It is a cohesive force between the molecules of water.

  24. Let’s draw an atom… • Remember atoms include a nucleus with protons and neutrons. • An electron cloud surrounds the nucleus. • Using three colors, draw this atom in the empty space in your notes.

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