Preliminary Course: Atomic Structure - Trinity College Dublin Course/Atomic structu… · Atomic...
Transcript of Preliminary Course: Atomic Structure - Trinity College Dublin Course/Atomic structu… · Atomic...
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Preliminary Course: Atomic Structure Lankani Wijesinghe
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Outline
PART 1
• What is Matter?
• History of the atomic structure
• Atomic model
PART 2
• Introduction to the periodic table
• Properties of some main group elements
• Ions
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Why learn atomic structure ?
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Classification of matter
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Classification of matter
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Classification of matter
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Different kinds of Atoms: The Elements
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To Democritus, atoms were small, hard particles that were all made of the same
material but were different shapes and sizes. Atoms were infinite in number, always
moving and capable of joining together.
Atomic Theory of Matter
To Democritus, atoms were small,
hard particles that were all made of
the same material but were different
shapes and sizes.
Atoms were infinite in number,
always moving and capable of
joining together.
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Atomic Theory of Matter
The billiard ball
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Law of Multiple Proportions
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The atomic theory makes sense!
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Atomic Structure: Electrons
• J.J.Thompson (1897) applies
voltage to gas in a sealed tube
•Cathode rays are negatively
charged
•The charged particles which are
produced are found to have a
mass 1800 times smaller than
hydrogen
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Plum pudding model
Thompson postulated that the negative particles reside within atoms,
balanced by a “delicious cake” of positive charge.
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Beyond the Plum Pudding
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Beyond the Plum Pudding
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Rutherford's conclusions
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Bohr’s Atom
Neils Bohr (1885–1962) refined Rutherford's
model in 1913 by proposing that electrons:
- orbit the nucleus without losing energy;
- could move only in fixed orbits of specific
energies.
- electrons with low energy would orbit closer to
the nucleus while electrons with high energy
orbit further from the nucleus.
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Rutherford's –Bohr’s Atom
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The neutron is discovered
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The Atomic Model
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The Nuclear Atom
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Atomic Number
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Mass Number
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Isotopes
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An example: Heavy water
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Birth of the Periodic Table
Also took in to consideration
• density
• melting point
• reactivity
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Mendeleev’s Periodic Table (1869)
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Mendeleev’s Periodic Table (1871)
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The Modern Periodic Table
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The Modern Periodic Table
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Metals, Non-Metals and Semi-Metals
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Metals • conducts electricity • has a metallic lustre • malleable and ductile
Non-metals
• lack metallic lustre • does not conduct electricity - good insulators • brittle
Semi-metals (metalloids)
• It has some properties like a metal and some properties are like a non-metal
Na Au
C
Hg
Br
Si Ge
Metals, Non-Metals and Semi-Metals
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Group 1: Alkali metals
• Soft, silvery metals
• Low melting points
• Very reactive with air and water
• Produces H2 when reacted with water
• Reactivity increases down the group
• One electron in the valence shell
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Group 2: Alkaline earth metals
• Silvery metals
• Less reactive than alkali metals
• Produces H2 when reacted with water
• Reactivity increases down the group
• Two electrons in the valence shell
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Group 17: Halogens
Cl Br I
• Chemically reactive
• Found in salts
• Used as disinfectants (eg. Cl, Br, I)
• Form acids when bonded to hydrogen (eg. HCl, HF)
• 7 electrons in the valence shell
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Group 18: Noble gases
• Colourless, ordourless gases
• Highly unreactive
• Only heavier noble gases undergo some chemical
reaction
• Electronically stable
Electron discharge colour
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Transition metals
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Transition metals
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Chemistry is all about electrons
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Sodium wants to lose an electron!
(Na+)
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Metals generally form CATIONS
Cu+, Cu2+ etc.
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Chlorine wants an electron!
(Cl-)
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Non-metals generally form ANIONS
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Cations and Anions stick together
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GOOD LUCK WITH YOUR FIRST YEAR AT TRINITY COLLEGE DUBLIN !!