2. Chemical Fundamentals Review Living things are composed of matter. Matter has mass, occupies space. Atoms composed of: – Small nucleus Proton (positive charge) Neutron (no charge) – Orbited by Electrons in arranged in shells (negative charge)

3. What is the PERIODIC TABLE? oShows all known elements in the universe. oOrganizes the elements by chemical properties.

4. How do you read the PERIODIC TABLE?

5. What is the ATOMIC NUMBER? oThe number of protons found in the nucleus of an atom Or oThe number of electrons surrounding the nucleus of an atom.

6. What is the SYMBOL? oAn abbreviation of the element name.

7. What is the ATOMIC WEIGHT? oThe number of protons and neutrons in the nucleus of an atom.

8. How do I find the number of protons, electrons, and neutrons in an element using the periodic table? o# of PROTONS = ATOMIC NUMBER o# of ELECTRONS = ATOMIC NUMBER o# of NEUTRONS = ATOMIC _ ATOMIC WEIGHT NUMBER

9. Example Atomic Mass – 12 Atomic Number - 6 Protons (6) Electrons (6) Neutrons (12-6 = 6)

10. Bohr Rutherford Diagrams 1.Write how many protons and neutrons are in the nucleus. 2.Draw electrons in rings (energy shells) around the nucleus. Ex. Fluorine 19 F 9 9p+ 10 n

11. Bohr- Rutherford Diagrams 1.Write the # of protons and neutrons in the nucleus. 2.The 1 st electron energy shell has a maximum of 2 electrons. 3.The 2 nd electron energy shell has a maximum of 8 electrons. 4.The 3 rd electron energy shell has a maximum of 8 electrons. 18p + 22n 0 Argon

12. Why are Electrons so Important? The chemical behaviour of an atom depends mostly on the number of electrons in its outermost shell. valence electrons/shell All atoms with incomplete valence shells are chemically reactive and are responsible for the formation of chemical bonds between atoms.

13. Octet Rule = atoms tend to gain, lose or share electrons so as to have 8 electrons C would like to N would like to O would like to H would like to Gain 4 electrons Gain 3 electrons Gain 2 electrons Gain 1 electron

14. Atoms bond to form compounds Compounds are made up of at least 2 different kinds of atoms (e.g., H 2 O) Bonds are formed by the sharing or transfer of electrons 2 Types of Chemical Bonds Ionic Bonds Covalent bonds

15. Ionic Bonds – occur when one atom donates or gives up one or more electrons - metal and non metal Ionic Compound ( Na + Cl - ) Salt crystals Opposite charges attract to form ionic bonds

16. Covalent Bonds – involve a sharing of a pair of valence electrons between atoms between two non-metals

17. Single covalent bond Double covalent bond Four single covalent bonds Two single covalent bonds

18. 2 Types of Covalent Bonds Polar CovalentNon-polar covalent Equal sharing of electrons Unequal sharing of electrons Determined by the atoms ELECTRONEGATIVITY E.g. H 2 O 2 E.g. H 2 O

19. Electronegativity The measure of an atom’s attraction for additional electrons Polar Covalent Bond - unequal sharing of electrons between two atoms with different electronegativity results. Non-Polar Covalent Bond – equal sharing of electrons between two atoms. Electronegativity = Stronger pull of shared electrons

20. The electronegativity difference ( ∆ En) is the difference in electronegativity number between two atoms participating in a covalent bond.

21. Electronegativity Differences

22. Molecular Polarity Depends on – Distribution of charges – Molecular shape Symmetrical molecular shapes produce non-polar molecules (whether bonds are polar or not) Asymmetrical molecular shapes produce polar molecules Balanced charges produce non-polar molecules Non-balanced charges produce polar molecules

23. Polar Molecules Align themselves to other polar molecules Soluble in water Exclude non-polar molecules (oils and fats)

25. VSEPR Valence shell electron pair repulsion Electrons repel one another forming the shape of the molecule Includes both bonded electron pairs and non- bonding electron pairs (lone pairs)

26. VSEPR