1. STRUCTURES & BONDING Title 04/10/2015 NextMATTER

2. MATTER is anything that has mass and takes up space.

3. STRUCTURES & BONDING ATOMS 04/10/2015 NextBack “WHAT IS MATTER MADE FROM?” A question which has been asked from the ancient Greeks up to 19 th century. In 530 B.C., Democritus, a Greek philosopher proposed that any matter could be halved continuously until small indivisible units could be reached.

4. STRUCTURES & BONDING ATOMS 04/10/2015 NextBack “WHAT IS MATTER MADE FROM?” The ideas proposed by the Greeks were generally unaccepted until in 1808, John Dalton (a teacher!) proposed the modern ATOMIC THEORY. From his experiments he found that only elements combined to form compounds. He soon realised that elements were made up of tiny indivisible spheres he called ATOMS. ATOM

5. STRUCTURES & BONDING ATOMS 04/10/2015 NextBack Atoms are the building blocks of matter. They are so small you cannot see them with normal microscopes Try cutting a strip of paper as small as you can…. An atom would be another 40 cuts from the smallest possible cut…at least! ATOM

6. STRUCTURES & BONDING ELEMENTS 04/10/2015 NextBack “WHAT IS AN ELEMENT?” An element is a substance which is only made up of one type of atom. Example, Carbon is made up of Carbon atoms.

7. STRUCTURES & BONDING STRUCTURE OF THE ATOM 04/10/2015 NextBack All matter is made up of atoms, but…. “WHAT ARE ATOMS MADE FROM?” Atoms are made up of even smaller subatomic particles called: ELECTRONS PROTONS NEUTRONS - +

8. + + + + + + + + + + + + + Nucleus STRUCTURES & BONDING STRUCTURE OF THE ATOM 04/10/2015 NextBack In the middle of an atom, the NUCLEUS can be found. In nucleus, PROTONS and NEUTRONS can be found. Orbiting the nucleus in SHELLS, ELECTRONS can be found. - - -- - - - - - - NOT TO SCALE!. -- - - - - - - ATOM

9. STRUCTURES & BONDING STRUCTURE OF THE ATOM 04/10/2015 NextBack The gap between electron shells and nucleus is very large on a subatomic scale. If an atom was the size of a stadium… …the nucleus would be the size of a pea on the centre spot!!

10. STRUCTURES & BONDING THE SUBATOMIC PARTICLES 04/10/2015 NextBack Each subatomic particle has a MASS and a CHARGE. ATOMIC PARTICLERELATIVE MASSRELATIVE CHARGE PROTON1 Unit +1+1 NEUTRON1 Unit 0 ELECTRON1/1840 (NOTHING!) -1 - + (Masses and Charges are RELATIVE which means in comparison to each other e.g. 1840 electrons will weigh the same as 1 proton.)

11. STRUCTURES & BONDING CHARGES 04/10/2015 NextBack In an atom, the number of electrons is equal to the number of protons. This means that since there is a balance between the number of positive and negative subatomic particles there is NO OVERALL CHARGE. An atom must be electrically neutral + + - - - - - + + + BORON ATOM No Charge 5 Electrons (5 Negatives) 5 Protons (5 Positives)

12. The structure of the atom MASS NUMBER (Atomic Mass) = number of protons + number of neutrons Atomic SYMBOL Atomic NUMBER = number of protons = number of electrons

13. STRUCTURES & BONDING COMPOUNDS 04/10/2015 NextBack “WHAT IS A COMPOUND?” A compound is a substance which is only made up of two or more elements chemically bonded. Example, Sodium Chloride is made up of Sodium and Chlorine Atoms.

14. Bohr-Rutherford Diagram 1. Calculate the number of protons and neutrons. 2. Write the number of p+ and n0 in the nucleus with a circle around them. 3. Draw the number of shells (circles) the atom has – the period number tells you the number of shells. 4. Calculate the number of electrons the atom (same as the number of protons) or ion) has. 5. Place in the electrons into the shells. Shell1 – 2 e-, Shell 2 onwards gets 8.

15. Periodic Table The periodic table is an arrangement of the elements according to: The number of protons, neutrons, and electrons Physical Properties - The way they look Chemical Properties - The way they act

16. 80% of the elements in the periodic table are metals A smaller group consists of non-metals Separating the two are a set of elements called metalloids. Periodic Table

17. The Periodic Table Shows the mass number and atomic number Gives the symbol of the element mass number 23 Na atomic number 11

18. Groups of Elements Vertical (up and down) columns on the periodic table Indicates the number of electrons on the outer most shell called valence electrons.

19. Periods on the Periodic Table The different rows of elements in the periodic table are called periods. Numbered 1-7 The period number of an element indicates the number of orbitals or shells the element has.

20. Periods on the Periodic Table 123456123456

21. Using The Periodic Table In your notes, use your periodic tables to determine the following for the elements at the bottom. –The number of protons –The number of neutrons –The number of shells –The number of electrons on the outer most shell (valence electrons) –Draw the atoms for each Calcium (Ca), Magnesium (Mg), Chlorine (Cl)

22. Isotopes: atoms of the same element that have a different number of neutrons. Atomic mass is the average mass of all isotopes of a particular element Family is a group of elements with similar properties arranged together in columns. Alloys are a mixture of two or more metals. Important Terms

23. The Periodic Table HHe LiBeBCNOFNe NaMgAlSiPSClAr KCaFeNiCuZnBrKr AgIXe PtAuHg Alkali metals Noble gases Halogens These elements are metals This line divides metals from non- metals These elements are non-metals

24. Most are solid at room temperature Most have a shiny appearance (lustrous) Their shape can be changed (malleable) Can be stretched and drawn into thin wires (ductile) Most conduct electricity and heat well Usually have high densities (ie. Sink in water) Properties of Metals

25. Poor conductors of heat and electricity or are insulators (don’t conduct at all). Low melting and boiling points (usually liquids or gases at room temperature). Brittle - if a solid. Do not possess metallic luster (so dull) Properties of Non-Metals

26. Behave mostly like non-metals But do have some metallic properties, most importantly they can conduct electricity. Metalloids

27. Group of elements that rarely react and are stable. Noble Gases (or inert gases)

28. 1.Group VIII – The Noble Gases All are colourless gases Occur naturally in the atmosphere Very stable Helium is safe and light, but the gases get heavier and more dense the further you go down the group. Families of Importance

29. 2.Group VII – The Halogens Form ions with a charge -1 Found in nature as salts Have coloured and poisonous vapours Form diatomic molecules As you move down the group, the atoms get bigger and less reactive Families of Importance

30. 3.Group I – Alkali metals Form +1 ions Extremely reactive Found in nature only as mineral salts Have typical metallic properties All alkali metals react violently with water, producing an basic solution and hydrogen gas. Families of Importance

31. 4.Group II – The Alkaline Earths Act in a similar but less reactive way as the Group I elements Families of Importance