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STRUCTURES & BONDING Title 05/05/2017 MATTER Next MATTER is anything that has mass and takes up space. STRUCTURES & BONDING ATOMS 05/05/2017 “WHAT IS MATTER MADE FROM?” A question which has been asked from the ancient Greeks up to 19th century. In 530 B.C., Democritus, a Greek philosopher proposed that any matter could be halved continuously until small indivisible units could be reached. Back Next STRUCTURES & BONDING ATOMS 05/05/2017 “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 Back Next STRUCTURES & BONDING ATOMS 05/05/2017 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 Back Next STRUCTURES & BONDING ELEMENTS 05/05/2017 “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. Back Next STRUCTURES & BONDING STRUCTURE OF THE ATOM 05/05/2017 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 Back Next STRUCTURES & BONDING STRUCTURE OF THE ATOM In the middle of an atom, the NUCLEUS can be found. - - - - + + + +++ + + Nucleus ATOM ++ ++ + - In nucleus, PROTONS and NEUTRONS can be found. - 05/05/2017 - - - Orbiting the nucleus in SHELLS, ELECTRONS can be found. - - - - NOT TO SCALE!. Back Next STRUCTURES & BONDING STRUCTURE OF THE ATOM 05/05/2017 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!! Back Next STRUCTURES & BONDING THE SUBATOMIC PARTICLES 05/05/2017 Each subatomic particle has a MASS and a CHARGE. ATOMIC PARTICLE PROTON + NEUTRON ELECTRON - RELATIVE MASS RELATIVE CHARGE 1 Unit +1 1 Unit 0 1/1840 (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.) Back Next STRUCTURES & BONDING CHARGES 05/05/2017 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 + + 5 Electrons 5 Protons No Charge (5 Negatives) (5 Positives) Back Next 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 STRUCTURES & BONDING COMPOUNDS 05/05/2017 “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. Back Next 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. 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 Periodic Table • 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. The Periodic Table Shows the mass number and atomic number Gives the symbol of the element mass number 23 Na atomic number 11 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. 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. Periods on the Periodic Table 1 2 3 4 5 6 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) Important Terms • 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. The Periodic Table Alkali metals Li Be Na Mg K Ca Halogens These elements H are metals Fe Ni He Cu Zn Ag Pt Noble gases Au This line divides metals from nonmetals B C N O F Ne Al Si P S Cl Ar Br Kr I Xe Hg These elements are non-metals Properties of Metals • 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 Non-Metals • 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) Metalloids • Behave mostly like non-metals • But do have some metallic properties, most importantly they can conduct electricity. Noble Gases (or inert gases) • Group of elements that rarely react and are stable. Families of Importance 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 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 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 4. Group II – The Alkaline Earths • Act in a similar but less reactive way as the Group I elements