chapter three. dalton’s atomic theory: every element is made of tiny, unique particles called...
TRANSCRIPT
Chapter Three
Dalton’s Atomic Theory:
Every element is made of tiny, unique particles called atoms that cannot be subdivided
Atoms of the same element are exactly alike
Atoms of different elements can join to form molecules
Because of new technology, we have discovered
some holes in Dalton’s Atomic Theory
Breaking Down the Atom
1. Nucleus-center of an atom, all the mass of the atom is here
it has a positive charge
made up of protons and neutrons
Breaking Down the Atom
2. Protons-a positively charged particle It’s a subatomic particle has an atomic mass of 1 AMU
1. Neutrons-a neutral charged particle = NO CHARGE
Subatomic particle same mass and size as a protons In reality, it is basically a proton that has
neutralized its positive charge by absorbing an electron.
To Sum up the Nucleus
The nucleus is made up of protons and neutrons. Protons and neutrons are both relatively the same mass and size but protons have a positive electrical charge and neutrons have no electrical charge.
Outside the Nucleus
1. Electron-a negative charged particle Very small mass (.000001 AMU)
Move around the nucleus because of the attraction btwn + and – charges
Creates a “cloud” because the electrons are moving very fast.
Outside the Nucleus
2.Energy-level-this is a location where electrons can be found based on their energy.
The more energy they have, the further away they are from the nucleus.
Electrons can only be found in certain energy levels
Outside the Nucleus3. Orbital-a region in an atom where there is
a high probability of finding electrons. Electrons may occupy 4 distinct orbitals
within atoms.
*** Since all electrons are negatively charged, they repel each other, therefore they will always be as far away from each other and still fill an electron cloud.
- Opposite Charges Attract, Like Charges Repel
Understanding the PTE
Valence Electron- an electron in the outermost energy level of an atom
Periodic Table of the Elements *This is a tool used by scientists to classify
elements *It is not to be memorized, just applied
Periodic law- properties of elements tend to change in a regular pattern when elements are arranged in order of increasing atomic number, or number of protons each has.
Periodic Table of the Elements Period- a horizontal row of elements in the
periodic table. - 7 total rows - each represents the number of electron
clouds in that element Group (family)-a vertical column of elements in
the periodic table - All elements in a family have similar properties - All have the same number of valence electrons.
- All usually will bond to the same cation(s) or anion(s)
Learning from the PTE
Ionization-the process of adding electrons or removing electron from an atom
-Atoms that do not have filled outer electron clouds can undergo a process called ionization.
- This process results in a more stable atom.
- Based on the position of the atom on the PTE.
Becoming Stable Ion-an atom or group of atoms that has lost or
gained one or more electrons therefore has a net electric charge
Cation-an ion with a positive charge - it loses an electron
- it now will have more protons than electrons making it positive
Anion-an ion with a negative charge - it gains electrons - it now has more electrons than protons
Information from the PTE Atomic number -the number of protons in the
nucleus of an atom - The atomic number also equals the number of
electrons it has. - Each element has a different atomic number
Mass number -the total number of protons and neutrons in the nucleus of an atom - represents average of all the different atoms of an elements
- The mass number includes only the number of protons and neutrons because protons and neutrons provide most of the atoms mass.
Exceptions to Daltons Rule Isotopes-any atoms having the same number of
protons but different number of neutrons- Most elements have at least one different isotope- Hydrogen has three:
1.Normal- Hydrogen 1 2.Deuterium- Hydrogen 2 = 1 proton & 1 neutron 3.Tritium- Hydrogen 3 = 1 proton & 2 neutron ** this one is radioactive- glows in the dark
Finding out about the Atoms
Atomic mass unit- represents the amount of mass of one proton of an element
Average atomic mass- the weighted average of the masses of all naturally occurring isotopes of an element
Elements on the PTE Metals- the elements that are good conductors
of heat and electricity - Most are shiny solids that can be stretched
and shaped - are malleable- can be easily bent - Families 1-12 - can only loses electrons to form + ions
Nonmetals- the elements that are not good conductors of heat and electricity - groups 13-18(approximately)
- Nonmetals may be solids, liquids, or gases.
Metals Semiconductors- the elements that are
intermediate conductors of heat and electricity
Ex: Metalloids
Alkali metals- the highly reactive metallic elements located in group 1 of the periodic table
Ex. H, Na, Li, K, lose 1 e- to have a full valence shell
** most are dangerously explosive
Metals continued Alkaline earth metals- the reactive metallic
elements located in group 2 of the periodic table Ex. Mg, Ca- Lose 2 e-s to fill their outer
Electron cloud
Transition metals- the metallic elements located in groups 3-12 of the periodic table
* Have overlapping electron clouds * They are much less reactive then sodium or
calcium, but they can lose electrons to form positive ions
**VERY IMPORTANT – they cannot gain e-s
Halogens
Halogens-the highly reactive elements located in group 17 of the periodic table
- They gain 1 electron to have a full electron cloud
- React very fast with group 1 metals
Ex. Cl, Fl, Br and I
Kings of the PTE Noble gasses- the un-reactive gaseous
elements (Group 18)* have full valence shells* happy atoms* Because these atoms have filled outer electron
clouds, they do not need to lose or gain electrons to become stable.
Counting Atoms
Mole-the SI base unit that describes the amount of substance * Mole day 10-23
Avogadro's number- the number of particles in 1 mole equals 6.022x 10to the 23rd /mol Particles
Molar mass- the mass in grams of 1 mole in a substance Conversion factor-a ratio equal to one that expresses the
same quantity in two different ways 1 mole = 6.02*10to the 23rd particles