1. Take out 6.1 Notes and Periodic Table!
Tuesday Nov 4th-Week 13
TOPIC: Atoms, Elements, & Compounds  OBJ : 1-4
DO NOW:
EXT: DUE DATE:
DW: 6.1 Notes
EXIT: Fill in your level of understanding AND Explain what an enzyme is and how it is used in biology/chemistry. (use your book pages)
Science of Life
Take out 6.1 Notes and Periodic Table!
-6.1 Notes
HANDOUTS to PICK-UP:
-6.2 Book Pages
TURN IN to ABS box:
SEMINAR 2:
BEFORE/AFTER SCHOOL:
DW-None
ABSENT
AGENDA

2. TUESDAY DO NOW Q: What is an ionic bond? What is a covalent bond?
Tuesday: ___11__/__4___
OBJECTIVE…#_1-4_____
TOPIC:
Atoms, Elements, & Compounds
Daily Work Grade- NONE
DW GRADE: 2 1 0
DO NOW
Q: What is an ionic bond? What is a covalent bond?
A: Covalent bonds share electrons, and ionic bonds donate electrons.

3. Today’s Objectives 1---IDENTIFY / DIAGRAM parts of an atom
2---DIFFERENTIATE & RECOGNIZE relationships of atoms,
elements, molecules, compounds
3---UTILIZE the periodic table to identify atomic structures of elements (CHOPN- characteristics)
4---COMPARE / CONTRAST covalent bonds and ionic bonds

4. These should be done by test day!
Vocabulary
-atom
-nucleus
-proton
-neutron
-electron
-element
-compound
-molecule
-covalent bond
-ion
-ionic bond
These should be done by test day!

5. Matter is composed of tiny particles called atoms
MAIN IDEA:
Matter is composed of tiny particles called atoms

6. ATOMS: smallest unit of matter
-2 parts: nucleus & orbitals 1-NUCLEUS: made of protons & neutrons 2-ORBITALS: area surrounding the nucleus -where electrons spin at amazing speeds

7. ATOMS / STRUCTURE
PROTONS: -p+ -located inside the nucleus -positive electric charge -relative size = 1 -ATOMIC # = # protons -unique to each element

8. ATOMS / STRUCTURE
NEUTRONS: -n -located inside the nucleus -no electric charge -relative size = 1 -n= atomic mass – atomic #

9. ATOMS / STRUCTURE
ELECTRON: -e- -located inside orbitals around the nucleus -negative electric charge -relative size = 1/1836 -has virtually no mass -#e = #p (in a stable atom)

10. ATOMS / STRUCTURE
electron e- proton nucleus neutron orbitals e p+ n

11. ATOMS / ORBITALS
-electrons orbit the nucleus in energy levels -electrons are constantly spinning like fan blades -electrons switch places in energy levels -each energy level can hold a certain # of electrons level 1 – 2 electrons level 2 – 8 electrons level 3 – 18 electrons level 4 – 32 electrons

12. ATOMS / BOHR MODEL
energy levels/# e-
1 - 2
2 - 8
3 - 18
4 - 32

13. ATOMS / ORBITALS No-it has 6 but can hold up to 8
IDENTIFY the # of electrons in the outermost energy level of the oxygen atom.____
DETERMINE: Is the 2nd energy level of the oxygen atom full?
EXPLAIN:
No-it has 6 but can hold up to 8

14. ATOMS / VALENCE ELECTRONS
-electrons in outer energy level
-# valence electrons same as representative group
-electrons involved in chemical bonds
SEE PERIODIC TABLE
1-NUMBER the REPRESENTATIVE GROUPS (FAMILIES)
- 1A thru 8A
*GROUP # = # of valence electrons (e-)
2-NUMBER the PERIODS
1 thru 7
*PERIOD # = # of energy levels needed for the electrons

15. PERIODIC TABLE of ELEMENTS
Representative groups #1-8

17. ATOMS / LEWIS DOT DIAGRAMS
-represent valence electrons -use element symbol -dots represent valence electrons Cl Na P N

18. ELEMENTS: pure substance
-can not be broken down into other substances
-not physically / not chemically
-atoms of the SAME element
-same atomic #
-same # p+ and e-
#p = #e overall neutral charge (NO charge)
-PERIODIC TABLE
-see handout
-atoms of same element:
-same ATOMIC #
-same p /e
atomic # = p = e

19. ELEMENTS / ISOTOPES
-ISOTOPES -atoms of same element that have different # n -different ATOMIC MASS -EX OXYGEN

20. ELEMENTS / RADIOACTIVE ISOTOPES
-RADIOACTIVIE ISOTOPES -still no charge -changing # n affects the stability of nucleus -causes decay/break apart -Carbon-14 is radioactive- -C-14 is found in all living things -½ life: time for ½ to decay -Calculate the age of an object by finding how much C-14 remains APPLY: Another carbon isotope has 6 protons and 8 neutrons in its nucleus. What is this carbon isotope called? ___________________
carbon-14

21. -Specific combination of elements -fixed ratio
COMPOUNDS-
pure substance / 2 > elements combine
-Specific combination of elements
-fixed ratio
-chemically/physically different
-than elements they are made of
-can NOT be broken down by physical means
-CAN be broken down chemically
DRAW CONCLUSIONS: Table salt is a compound made of sodium and chlorine. Could you separate the sodium from the chlorine by crushing the salt crystals? ______
EXPLAIN: NO
compound cannot be broken down by physical means

22. CHEMICAL BONDS
VIDEO CLIP- chemical bonds

23. O + C + O  C O CHEMICAL BONDS / COVALENT
*GOAL: 8 e- in the outer shell of each atom
-electrons are SHARED between 2 atoms
-NON-METALS bond with NON-METALS
(neither non-metal wants to give up e-)
-forms a MOLECULE
Example:
O C O  C O

24. Na + Cl  NaCl CHEMICAL BONDS / IONIC
*GOAL: 8 e- in the outer shell of each atom
-electrons are TRANSFERRED between 2 atoms
-METALS bond with NON-METALS
(metals give up e- easily)
-forms a MOLECULE
Example:
Na Cl  NaCl

25. IONS: atom that TRANSFERS electron
lose an electron  positive charge
gain an electron  negative charge
CATION (+)Element gives up e- in the outer shell
-atom becomes a positively charged ion
ANION (-)Element gains the e- in their outer shell
-atom becomes a negatively charge ion

26. REVIEW / PRACTICE
p + n

27. REVIEW / PRACTICE

28. EXIT
FILL-IN: level of understanding of today’s objective
  
EXIT: Explain what an enzyme is and how it is used in biology/chemistry. (use your book pages)