section 2.1. four classical atomic models quantum mechanical model
TRANSCRIPT
The Periodic Table and Atomic Structure
Section 2.1
Four classical atomic models Quantum Mechanical Model
Review
Distinguish between metals, non-metals, and metalloids in terms of distinguishing properties
Explain the structure of the periodic table Identify important families and elements Describe atomic theory in terms of subatomic particles and
location (nucleus, energy levels) Define atomic number, mass number, isotope, and atomic
molar mass and be able to identify these for a given element Determine numbers of protons, neutrons and electrons for a
given element Describe the process of ionization and formation of cations and
anions Identify patterns in the periodic table for valence electrons and
energy levels Relate ionization to the octet rule
Objectives
Antoine Lavoisier Mass is neither created or destroyed The total mass of the reactants equals the
total mass of the products
Law of Conservation of Mass
115: basic building blocks 90 naturally occurring, 25 synthetic Split into 3 classes
◦ Metals◦ Non-metals◦ Metalloids
◦ https://www.youtube.com/watch?v=GFIvXVMbII0
The Elements
Most elements (75%) Silver/grey and shiny Conductors of heat and electricity Malleable and ductile Most solid at room temperature Reactivity varies
◦ Most reactive is francium (left and down)◦ Inert= unreactive
Metals
17 elements Grouped based on their different from
metals Vary is state, color and reactivity
◦ Highly reactive= fluorine (right and up ◦ Inert= noble gases
About half will appear at molecules (more than one atom)
Non-Metals
Remaining elements Properties intermediate between metals and
non-metals Along the staircase (except aluminium) Ex. Silicon, arsenic, boron
Metalloids
The Periodic Table
Organizes elements based on chemical properties◦ Metals on left side and centre◦ Non-metals on far right
Exception hydrogen (learn more later)◦ Metalloids between two
Shows name and symbol for element◦ Get to know the symbols!
http://periodictable.com/
The Periodic Table
For the following, identify as being a metal, non-metal or metalloid
Hydrogen Sulfur Calcium Tin Gold Boron Aluminum Xenon
The Element Game
For the following, give the element’s name or symbol:◦ Calcium◦ Hydrogen◦ Sulfur◦ Phosphorus◦ Mg◦ Na
Pre-test
Vertical columns Groups of elements with similar
chemical/physical properties Group 1: alkali metals
◦ Soft, shiny, silver, very reactive with water◦ Compounds white and soluble in water
Group 2: alkali earth metals◦ Shiny, silver◦ White compounds but not as soluble
Important Families/ Groups
Group 17: halogens◦ Non-metals◦ Very reactive
React with alkali metals to make salts Group 18: noble gases
◦ Non-metals◦ Very unreactive
Important Families cont…
Horizontal rows Have the same number of levels of
electrons
Periods
Crossword What’s in a Name? ELEMENTary My Dear Watson
To Do
Atoms are very small (10-10 m in diameter) What are three kinds of subatomic particles?
◦ Protons, Neutrons and Electrons Where are they found?
◦ Protons and Neutrons- inside the nucleus◦ Electrons- outside the nucleus
Protons and neutrons are over 99.9% of total mass◦ Imagine this: our classroom filled with iron. If we take
out the nuclei for all the iron atoms and place them side by side, they would be as big as a period in a book. But that period would almost equal the mass of the room full of iron
Atomic Theory
Has a positive charge (p+) Mass of 1.67x10-27 kg The number of protons defines the element
and is called the atomic number
All helium atoms have a 2 p+ and every atom with 2 p+ is helium
Protons
No charge (n0) Mass of 1.67x10-27 kg The number of protons and neutrons
together make the atomic mass of the atom◦ If an atom has 8 protons and 10 neutrons, its
atomic mass is 18◦ If an element has an atomic number of 24
(protons) and an atomic mass of 52 (protons and neutrons) it has 28 neutrons
Neutrons
Charge of 1- (e-1) Mass of 9.11x10-31kg Electrons are so small that they are not
factored into the atomic mass In an atom the number of protons = the
number of electrons
Electrons
Number of protons Determines the element
Atomic Number
Can you find the atomic number of the following elements?PbHgtinchlorineplatinumCumanganeselithium
As we move through the periodic table, what do you notice about the ordering of atomic numbers?
Isotope- atoms of same element with different number of neutrons◦ Ex. Common form of hydrogen has one proton
and no neutrons. 1/10 000 hydrogen atoms have a neutron, called deuterium (“heavy” hydrogen)
Each isotope given a mass number◦ Equals total number of protons and neutrons
(don’t include electrons- too small)◦ # of neutrons= mass number – atomic
number
Mass Number and Isotopes
Can be shown as:
◦ Mass number
element symbol atomic number
Ex. Oxygen-16
What would be the symbols for oxygen-17? Oxygen-18?
Mass Number and Isotopes cont…
Mass number and isotopes
Name:#p = _____#n = _____#e = _____
Name:#p = _____#n = _____#e = _____
Practice: Fill in the chart!Element Name
Mass Number
Number of Protons
Number of Neutrons
calcium 41
uranium 238
aluminum 14
9 5
20 10
iron 30
Shown in the periodic table Average mass of element’s isotopes Number of electrons equals number of
protons (in neutral atoms)
Atomic Molar Mass
Atomic molar mass
Neils Bohr- proposed that electrons moved around a nucleus at a specific fixed distance◦ Energy level
Electrons could move up levels by absorbing energy
Electrons could move down levels by losing energy
BUT each energy level can only have a certain maximum number of electrons
Bohr Model of the Atom
Electrons occupy energy levels◦ Region around nucleus either empty or contain
electrons◦ Increase energy when get further from the
nucleus Specific number of electrons/level
◦ First level- 2 electrons◦ Next levels- 8 electrons
Energy level can be empty, partly or completely filled
Energy Levels
Drawings include:◦ Number of protons (in nucleus)◦ Number of neutrons (in nucleus)◦ Electrons in correct energy levels (how many electrons can be in each
level?) Ex. Hydrogen Lithium Sodium Oxygen Sulfur Helium Neon Argon Calcium
Drawing Atoms
Electrons in the outermost energy level Valence number- number of electrons an
element can lose/gain to combine with other elements
How many valence electrons do each of the following elements have?◦ Oxygen?◦ Magnesium?◦ Chlorine?◦ Argon?◦ Carbon-14?
Valence Electrons
For understanding how atoms bond Atoms want to have eight electrons in their
valence shell (which shell is this?) More stable when have full energy levels What are these elements like with full energy
levels?◦ Noble gases!◦ Gain/lose electrons to be like their closest noble gas◦ Ex. Chlorine will gain one electron to be like argon◦ Exception: hydrogen, lithium and beryllium. Why?
Who do they want to be like?
The Octet Rule
When we gain/lose electrons from an atom, what happens to its charge?◦ Ex. Fluorine gains one electron to fill its outer
octet. What is its electrical charge now? Gaining/losing electrons process called
ionization◦ Results in positively charged or negatively
charged ions
What Now?
Elements can lose or gain outermost (valence) electrons◦ Called ionization◦ Makes ions (positively or negatively charged)◦ Allows metals and non-metals to form
compounds◦ http://www.youtube.com/watch?
v=xTx_DWboEVs&feature=related
Formation of Ions
Positively charged ions Metal ion loses electrons Where do the electrons go?
◦ To another atom Why would the atom be positively charged if
it loses electrons? Ex Magnesium
◦ Loses 2 electrons◦ What would the diagram look like before? After
ionization? Put charge as a superscript: ex. Mg2+
Cations
Negatively charged ions Non-metal gains electrons Where do the electrons come from?
◦ From atoms that lose electrons (cations) Why is it negatively charged? Ex. Oxygen
◦ Gains two electrons◦ What is the diagram before? After ionization?
How would you write it as a symbol?
Anions
Cations:◦ Element name + ion◦ Ex. sodium ion◦ Ex. magnesium ion
Anions:◦ First part of element name and change ending to
“ide”◦ Ex. nitride ◦ Ex. oxide◦ Ex. fluoride
Naming Ions
For each of the following ions, draw with nucleus and electrons and give appropriate name or symbol:
Hydrogen ion Cl- Nitride Be2+
sulfide
Practice
group 1 = 1+ group 2 = 2+ group 3-12 labeled on table group 15 = 3- group 16 = 2- group 17 = 1- group 18 not ions B, C, Si do not form ions
Ion Trends in Periodic Table
Why do atoms gain or lose electrons?◦ To have full energy levels and be more stable like
closest noble gas Once ions are formed:
◦ Electrically charged◦ What would happen when I bring a cation and an
anion together?◦ Form a bond! How we make compounds between
metals and non-metals◦ Need to form the ion first before a bond can
be formed
Why form ions?
Building an Atom Assignment
TO DO