1. Unit 2: Matter, Chemical Trends, and Chemical Bonding 1) Review: M________, E__________________, A__________ Structure (B________-Rutherford Diagrams), P_________ table of elements 2) Compounds and Bonding (ionic and covalent): naming, structural representation, chemical formula.

2. What is Chemistry Chemistry: the study of m_______ and e___________ and the i_______________ between them. The study of how the c_________________ of matter relates to its p_______________.

3. Chemistry is responsible for solving several societal issues Environmental issues: Preventing release of dangerous toxins from manufacturing sites, preventing corrosion (rust) on buildings and important monuments. Health Issues: Developing drugs to fight dangerous diseases,

4. The Basics of chemistry What is matter? Matter: is anything that occupies s________ and has a m____________ (e__________ is not matter) Examples of matter: __________________

5. Classifying Matter Review

6. Does Homer occupy space? Does homer have a mass?

7. Matter Pure Substance: Substance made up of only o_____ kind of matter (p______________). Element: Contains only o____ kind of atom. The chemical symbol has o_______ capital l________. Compound: A pure substance that is made of ________ or more different elements that are combined together chemically. The chemical symbol has ____ or more capital l_________. Ex: NaClEx: Na

8. All matter is made of tiny particles called atoms: Atom: S____________ part of an element that has all the element’s properties. E.g. G______ (Au) and Silver (____) are elements. Elements: Substance that c______________ be broken down into any simpler substance.

9. Structure of the Atom: Atoms are composed of 3 subatomic particles. 1) Electrons: have a charge of ____. Orbit around the center of the atom in energy levels called s__________. 2) Protons: have a charge of _____. Are located at the center (n________) of the atom with the neutrons. 3) Neutrons: do ____ have a charge. Are located at the center (n________) of the atom with the Protons.

10. Electrons are in orbit around the nucleus just like planets are in orbit around the sun P+ N e- Electron Shell Note: The center of the atom is composed of protons and neutrons. The center is called the nucleus. It is in the nucleus where most of the mass resides. Electron Nucleus Proton Neutron

11. Properties of the subatomic Particles NameSymbolRelative massChargeLocation Proton1836 Neutron1837 Electron1

12. Location of electrons: The electrons are located around the nucleus in shells. The first innermost shell can hold up to _____ electrons. The next two shells can hold up to _______ electrons each. Valence shell: The o______ most shell of an atom. The electrons in this shell are called the valence electrons. The valence electrons determine the chemical and physical p______________ of elements.

13. It is the number of subatomic particles that determine what element you have: the atoms of every element have the same number of protons Hydrogen atoms always have one proton. Lithium atoms always have 3 protons. Sample problem: An element has 2 protons. The element is ______________?

14. Case Study: Sulfur – A typical atom A Bohr diagram: an illustration of an a_______ that shows the a__________ and n__________________ of electrons in each shell. All sulphur atoms have ____ p_________. All sulphur atoms have ____ e______________ (to match the number of protons). Sulphur

15. Steps to Drawing a Bohr-Rutherford Diagram – Sulfur 16 electrons, 16 protons, and 16 neutrons 1) Draw a small center circle to represent the nucleus. 2) Write the number of protons and neutrons within this circle. 3) Draw slightly larger circle around this center circle to represent the inner shell. 4) Add electrons (2 max) to this shell (represent the electrons as dots). 5) Draw slightly larger circle around this circle to represent the next shell. 6) Add electrons (8 max) to this shell (represent the electrons as dots). 7) If this shell gets filled, draw another shell and add up to 8 electrons to it. p = 16 n = 16 Note: Adding electrons should be done in an organized fashion.

16. So, how can we tell how many protons, electrons, and neutrons an element has? THE P__________ T________ OF E____________!THE P__________ T________ OF E____________!

17. The Periodic Table of Elements: created by Dmitri Mendeleev All of the known elements are organized in the periodic table of elements. The horizontal rows are called p____________ (there are ___). 1 2 3 4 5 6

18. The period in which an element belongs tell us how many electron shells that element has! Period 1: ___ shell Period 2: ___ shells Period 3: 3 shells Period 4: 4 shells Period 5: 5 shells Period 6: 6 shells Period 7: __ shells

19. The Periodic Table of Elements: created by Dmitri Mendeleev The vertical columns are called f___________ or g________. There are 18 groups. Elements in the same family (group) of the periodic table have similar physical and chemical p________________. 1 21314151617 18 Groups 3 - 12

20. The Group in which the element belongs tells us the number of v___________ e___________ & the i__________ it will form. Group 1 elements: ____ valence electron. Group 2 elements: ____ valence electrons. Group 3-12 are weird Group 13: 3 valence electrons Group 14: 4 valence electrons Group 15: 5 valence electrons Group 16: 6 valence electrons Group 17: 7 valence electrons Group 18: Complete valence shell (2 for He and 8 for rest)

21. The categories The elements are organized in three categories: the m_______ (left and centre of the periodic table), the n________________ (on the right side of the periodic table), and the m___________ (the staircase of elements).

22. The categories CategoryPropertiesLocation in P.T.Examples Metals-Good conductors of heat and electricity -Shiny and silver coloured. -Ductile and malleable -All solid at room temperature (except for Hg) -Left and center of periodic table. Li, ___________ ___________ ___________ MetalloidsProperties in between those of metals and non-metals. -In between the metals and non- metals (separated by a staircase). B, ___________ ___________ Non-metals-Not metals -Poor conductors -At room temperature: some are solid, some are liquid, and some are gases. -Right hand-side of the table. He, ___________ ___________

23. The families: Further division of the 3 major categories

24. FamilyPropertiesLocation in P.T.Examples A____________ Metal -Soft, silver-grey metals. -React easily with H 2 O and O 2 in the air. -Group 1 (except H) Li and Na Alkaline Earth Metals -Silver grey metals. -Harder than alkali metals. -Reactive but less reactive than alkali metals. -Group 2 Be and Mg H_____________-Coloured non-metals that are very reactive. -Group 17F, Cl, Br, I, At N_____________ Gases -Non-metal gases -Colourless, odourless, and very unreactive. -Group 18He, Ne, Ar T_____________ metals -Metals with a range of reactivity and a wide range of properties. -In general: shiny and good conductors of heat and electricity. They also have higher densities and melting points than groups 1 & 2. (1 or 2 outer level electrons) -Groups 3-12 (including lanthanides and actinides) Cu, Fe