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Science 10 NotesChemistry
Atom: All matter is made up of small particles called atoms
Proton: Positively charged atom that gives weight to the nucleus
Neutron: Neutrally charged atom that gives weight to nucleus
Electron: Negatively charged atom that does not give much weight and moves fast
Nucleus: Centre of an atom (Protons + Neutrons)
Mass Number: Number of Protons + Number of Neutrons (Weight)
Atomic Number: Number of protons in an atom
Atomic Mass: Average mass of more than one type of atoms of the same element
Compound: 2 or more elements together
Development of the Atomic Theory
Aristotle (300BC) Believed matter was composed of different proportions
of four basic elements: Fire, Earth, Water, Air
Democritus (400BC) Theorised how many times matter could be broken down
until it reached its smallest component. He reasoned that
the smallest particle possible should be called atoms,
which is Greek for “indivisible”.
, John Dalton 1808 Presence of difference types of atoms.
Fundamentals of elements and compounds:
1. All matter is made up of atoms
2. Atoms cannot be created or destroyed or divided
into smaller parts
3. All atoms of the same element are identical in
mass and size
4. Compounds are formed when atoms of different
elements combine in fixed proportions
J.J. Thompson 1897 Discovery of charged particles (protons and electrons)
- Atoms were no longer the smallest things
- Electrons scattered through a cloud of positive
charges
Ernest Rutherford (1908) Presence of nucleus. Electrons around nucleus.
i. Atoms have small dense positively charged core
that reflects protons; while the rest must be empty
space for electrons to float around
Niels Bohr (1913) Electron shell exists. Electrons move around the nucleus.
Heisenburg Uncertainty Principle (No idea where the electron is)
Modern Atomic Theory
i. All matter is made up of tiny particles called atoms
ii. An atom is the smallest piece of an element that still retains the same properties of
that element
iii. Atoms are electrically neutral, they do not have a charge
iv. Atoms are composed of 3 subatomic particles: protons, neutrons, and electrons
Particle Location Charge Relative Mass
(amu)
Protons Nucleus + 1
Neutrons Nucleus O 1
Electrons Electron Cloud - 0 (1/1840)
Isotopes
Elements that have the same number of protons and the same chemical reactivity but
have different masses
This is due to the different amounts of neutrons
Periodic Table
, Founder: Dmitri Mendeleev
Purpose: A way to organise known elements (Organised in increasing atomic mass)
Total known elements: 118 (94 Naturally occurring, 24 synthetic -> produced in laboratories
but not found in nature)
Mendeleev noticed that as mass increased, certain chemical and physical properties started
to repeat. These were put in the same group
Period: Horizontal Row
Group: Vertical Column
Alkali Metals (Group 1)
i. Soft, shiny, malleable, ductile metals, easily cut with a knife
ii. Low density
iii. Highly reactive
iv. All react with water and create alkaline solutions
Alkali Earth Metals (Group 2)
i. Somewhat reactive
ii. Reacts with water but less than group 1
iii. Reacts with hydrochloric acid to form hydrogen gas
iv. Denser than group 1
v. Gain 2 electrons to become stable
Transition Metals (Group 3 – 12)
• Higher density than group 1 and 2 + hardness
• Conductors of electricity and heat
• High melting points
• Malleable and ductile
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