The study of atoms reveals that all matter consists of tiny, constantly moving particles, as described by the kinetic theory. Diffusion illustrates how particles spread from high to low concentrations, with gases moving faster due to larger spaces between them. Atoms are made up of subatomic partic...
Atoms - Summary
The Kinetic Theory - Matter consists of many, very small particles which are
constantly moving or in a continual state of motion.
Diffusion - Is the movement of particles from a high concentration to a low
concentration. (Ex. Potassium manganate)
- In liquids: Is slow as particles move slightly and have
small spaces between them
- In gases: Is fast as particles move rapidly and have large
spaces between them.
Volatile - liquid @ room temperature but when opened to air fumes show
Diffusion experiment - Ammonia is lighter than hydrogen chloride ->
travels farther -> fumes form nearer to hydrogen chloride -> small light
particles diffuse faster than large heavy ones
Brownian Motion - Random motion of visible particles caused by the
bombardment of much smaller, invisible ones.
Atomic number = Protons = Neutrons
Mass number = Atomic number + Neutrons
Neutrons = Mass number - Atomic number
Isotopes - atoms of the same element with the same number of protons
and neutrons but different number of electrons
Finding the RAM - percentage of abundance x mass number of both
isotopes added together, then the answer is divided by 100.
Electronic Configuration - 1st shell: Can hold up to 2 electrons
2nd shell: Can hold up to 8 electrons
3rd shell: Can hold up to 8 electrons
Periodic Table - Group 1: Alkali metals
Group 2: Alkali Earth metals
Group 3, 4, 5, 6: No name
Group 7: Halogens (produce salt)
Group 8/0: Noble gases (don’t react due to a full outer shell)
Group Number - Is found by the number of electrons in the outer shell
Period Number - Is found by the number of shells in the element
Aim of atoms - to achieve noble gas electronic configuration
- Metals lose electrons while non-metals gain them
Valency - number of electrons gained, shared or lost.
Ionic Bonding - bond between metals and non-metals by transfer of
electrons
- Metals lose electrons = positive ions = cations
- Non-metals gain electrons = negative ions = anions
- Ion = a charged particle as it consists of an equal amount
of protons and electrons
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