periodic table r08
DESCRIPTION
This is a first draft of a PowerPoint I put together for my HS chemistry 9 class on the periodic table in 2008.TRANSCRIPT
![Page 1: Periodic Table R08](https://reader034.vdocument.in/reader034/viewer/2022052410/556155aed8b42a8a7d8b5373/html5/thumbnails/1.jpg)
The Periodic Table
Elements & Families of Elements
![Page 2: Periodic Table R08](https://reader034.vdocument.in/reader034/viewer/2022052410/556155aed8b42a8a7d8b5373/html5/thumbnails/2.jpg)
Unit Outcomes
Number the periods (electron shells) Number the groups (valence number) Draw the line that separates the metals from
the nonmetals Write the oxidation numbers Identify atoms that are solid, liquid and gases
at room temperature
![Page 3: Periodic Table R08](https://reader034.vdocument.in/reader034/viewer/2022052410/556155aed8b42a8a7d8b5373/html5/thumbnails/3.jpg)
Unit outcomes, continued
Learn names and symbols of the elements shown below.
![Page 4: Periodic Table R08](https://reader034.vdocument.in/reader034/viewer/2022052410/556155aed8b42a8a7d8b5373/html5/thumbnails/4.jpg)
Unit Outcomes, continued
Identify trends across the periodic table Identify key properties of metals and nonmetals Locate the families
Alkali metals, Alkaline earth metals, transition metals, metalloids, Halogens, Noble gases
Identify key properties of families Learn key vocabulary—solid, liquid, gas, ‘full’,
reactive, conductor, brittle, melting point, etc.
![Page 5: Periodic Table R08](https://reader034.vdocument.in/reader034/viewer/2022052410/556155aed8b42a8a7d8b5373/html5/thumbnails/5.jpg)
Periodic Table
![Page 6: Periodic Table R08](https://reader034.vdocument.in/reader034/viewer/2022052410/556155aed8b42a8a7d8b5373/html5/thumbnails/6.jpg)
Elements Defined
Elements are substances that cannot be broken down into simpler substances by ‘ordinary’ chemical means such as by heat, light, electricity, or reaction with other substances special equipment, such as a particle
accelerator, or temperatures like those inside the sun can break down elements
![Page 7: Periodic Table R08](https://reader034.vdocument.in/reader034/viewer/2022052410/556155aed8b42a8a7d8b5373/html5/thumbnails/7.jpg)
Periods and Groups
![Page 8: Periodic Table R08](https://reader034.vdocument.in/reader034/viewer/2022052410/556155aed8b42a8a7d8b5373/html5/thumbnails/8.jpg)
Periods
Horizontal Rows are called PERIODSPeriod number = # of electron shells of
atoms in each row Period 1 atoms all have 1 electron shell Period 2 atoms all have 2 electron shells … etc. Period 7 atoms all have 7 electron shells
![Page 9: Periodic Table R08](https://reader034.vdocument.in/reader034/viewer/2022052410/556155aed8b42a8a7d8b5373/html5/thumbnails/9.jpg)
Groups
Vertical Columns are called GROUPS Group number = # of electrons in the outermost
shell of atoms in each column Group 1 atoms have 1 electron in their outermost shell Group 2 atoms have 2 electrons in their outermost shells … etc. Group 8 atoms all have ‘full’ outermost shells
e.g., Helium has 2 e- in outermost shell e.g., Neon and argon have 8 e- in the outermost shell
![Page 10: Periodic Table R08](https://reader034.vdocument.in/reader034/viewer/2022052410/556155aed8b42a8a7d8b5373/html5/thumbnails/10.jpg)
Group Number/Valence Electrons
Group number = number of valence electrons Valence electrons—electrons in the outermost
shell determine how an atom combines with other atoms
its chemical properties
Group numbers can be written with Arabic (1, 2, 3, etc.) or Roman numerals (I, II, III, etc.) Use Roman numerals to avoid confusion
![Page 11: Periodic Table R08](https://reader034.vdocument.in/reader034/viewer/2022052410/556155aed8b42a8a7d8b5373/html5/thumbnails/11.jpg)
Ions
ION (definition) — an atom (or group of atoms) that is positively or negatively charged; a charged particle
Na+1 Na ---> Na+ + 1e- Be? Atom + ion donates an e-
B 11 p+ 11 p+
N 11 e- 10 e-
O F Cl + 1e- --- > Cl-
Atom accepts an e- - ion
17 p+ 17 p+
17 e- 18 e-
![Page 12: Periodic Table R08](https://reader034.vdocument.in/reader034/viewer/2022052410/556155aed8b42a8a7d8b5373/html5/thumbnails/12.jpg)
Electropositivity
the ability of an atom to lose electrons and form positive ions.
http://www.meta-synthesis.com/webbook/35_pt/pt.html
![Page 13: Periodic Table R08](https://reader034.vdocument.in/reader034/viewer/2022052410/556155aed8b42a8a7d8b5373/html5/thumbnails/13.jpg)
Electronegativity
the ability of an atom to gain electrons and form negative ions the stronger an atom pulls electrons, the higher its
electronegativity
![Page 14: Periodic Table R08](https://reader034.vdocument.in/reader034/viewer/2022052410/556155aed8b42a8a7d8b5373/html5/thumbnails/14.jpg)
Oxidation Numbers
The number of electrons donated (lost) or accepted (gained) by an atom Donate 1 to 4 electrons
Oxidation # +1, +2, +3, +4 Form positive ions (+1 ion, +2 ion, +3 ion, etc.)
Accept 1 to 4 electrons Oxidation # -4, -3, -2, -1 (-1 ion, -2 ion, -3 ion, etc.) Form negative ions
Do not donate/accept electrons Oxidation # 0
Atoms become stable (get ‘full’ outer shells) by donating or accepting valence electrons!
![Page 15: Periodic Table R08](https://reader034.vdocument.in/reader034/viewer/2022052410/556155aed8b42a8a7d8b5373/html5/thumbnails/15.jpg)
Oxidation Numbers
![Page 16: Periodic Table R08](https://reader034.vdocument.in/reader034/viewer/2022052410/556155aed8b42a8a7d8b5373/html5/thumbnails/16.jpg)
The Elements (1955)—A Song
Read the ‘lyrics’ as the song plays.
Pay attention to the pronunciation of the elements.
Can you sing along? Give it a try!
animation
by Tom Lehrer, Maths professor at Harvard
![Page 17: Periodic Table R08](https://reader034.vdocument.in/reader034/viewer/2022052410/556155aed8b42a8a7d8b5373/html5/thumbnails/17.jpg)
Solids, Liquids, Gases
![Page 18: Periodic Table R08](https://reader034.vdocument.in/reader034/viewer/2022052410/556155aed8b42a8a7d8b5373/html5/thumbnails/18.jpg)
Solids, Liquids, Gases
Liquids: Br, Hg
Gases: H, N, O, F, Cl, He, Ne, Ar, Kr, Xe, Rn
Solids: All other elements
![Page 19: Periodic Table R08](https://reader034.vdocument.in/reader034/viewer/2022052410/556155aed8b42a8a7d8b5373/html5/thumbnails/19.jpg)
Elements
Synthetic (man-made) Atomic numbers 43, 61, 93-118
Naturally occurring (found in nature) All other elements
![Page 20: Periodic Table R08](https://reader034.vdocument.in/reader034/viewer/2022052410/556155aed8b42a8a7d8b5373/html5/thumbnails/20.jpg)
Metals () and Nonmetals ()
![Page 21: Periodic Table R08](https://reader034.vdocument.in/reader034/viewer/2022052410/556155aed8b42a8a7d8b5373/html5/thumbnails/21.jpg)
Metals and NonMetals
Different electron cloud configurations of elements create (result in) different properties
Metals: outer shells with few electrons Tend to lose electrons, form positively charged
ions, in chemical reactions
Nonmetals: outer shells are nearly full Tend to gain electrons, form negatively charged
ions, in chemical reactions, OR share electrons and form a covalent bond
![Page 22: Periodic Table R08](https://reader034.vdocument.in/reader034/viewer/2022052410/556155aed8b42a8a7d8b5373/html5/thumbnails/22.jpg)
Metals VS Nonmetals
Metalsgood conductors of heat &
electricity
ductilecan be drawn out into wires
malleable (bendable)can be forced (hammered)
into different shapes
high melting points so solid at room temperature
form positive ions, cations
form basic oxides
NonmetalsGood electrical insulators;
nonconductors of electricity
brittle & crumbly in solid form
relatively low boiling points form negative ions, anions
form acidic oxides
![Page 23: Periodic Table R08](https://reader034.vdocument.in/reader034/viewer/2022052410/556155aed8b42a8a7d8b5373/html5/thumbnails/23.jpg)
Acids and Bases
![Page 24: Periodic Table R08](https://reader034.vdocument.in/reader034/viewer/2022052410/556155aed8b42a8a7d8b5373/html5/thumbnails/24.jpg)
Metals and Nonmetals
Metalsreact with nonmetals
to form compounds
Nonmetals (Group 7)very reactiveform ionic bonds with
metalsform covalent bonds
with other nonmetals
![Page 25: Periodic Table R08](https://reader034.vdocument.in/reader034/viewer/2022052410/556155aed8b42a8a7d8b5373/html5/thumbnails/25.jpg)
Trends: Metallic Properties
![Page 26: Periodic Table R08](https://reader034.vdocument.in/reader034/viewer/2022052410/556155aed8b42a8a7d8b5373/html5/thumbnails/26.jpg)
Metalloids and Diatomics
7 metalloids B, Si, Ge, As, Sb, Te, Po Intermediate (in between) physical and chemical
properties (metals and nonmetals) silicon and germanium, are semi-conductors (computers)
7 diatomics H, N, O, F, Cl, Br, I
H2, N2, O2, F2, Cl2, Br2, I2
![Page 27: Periodic Table R08](https://reader034.vdocument.in/reader034/viewer/2022052410/556155aed8b42a8a7d8b5373/html5/thumbnails/27.jpg)
Trends across the Periodic Table
as you move down a group ( )Atomic number, mass, density and size
(radius) increasesMelting points decrease (metals)/ increase
(nonmetals)Reactivity increases (metals)/ decreases
(nonmetals)
*Fr and F are 2 most reactive elements*
![Page 28: Periodic Table R08](https://reader034.vdocument.in/reader034/viewer/2022052410/556155aed8b42a8a7d8b5373/html5/thumbnails/28.jpg)
Trends across the Periodic Table
as you move across a period ( )Atomic number and mass increasesSize (radius) decreasesHardness and melting points increase
(metals) Reactivity decreases (metals)/ increases
(nonmetals)
![Page 29: Periodic Table R08](https://reader034.vdocument.in/reader034/viewer/2022052410/556155aed8b42a8a7d8b5373/html5/thumbnails/29.jpg)
Atomic Number and Mass
![Page 30: Periodic Table R08](https://reader034.vdocument.in/reader034/viewer/2022052410/556155aed8b42a8a7d8b5373/html5/thumbnails/30.jpg)
Size (atomic radii)
“Atoms with more
electrons will be bigger.”
top to bottom
X left to right
Why?
Protons (+)
AND
electron shells (-)
![Page 31: Periodic Table R08](https://reader034.vdocument.in/reader034/viewer/2022052410/556155aed8b42a8a7d8b5373/html5/thumbnails/31.jpg)
Summary of P.T. Trends
Metal Atoms: relatively large atoms with weak attraction for electrons
more metallic
Nonmetal Atoms: relatively small atoms with strong attraction for electrons
more nonmetallic
![Page 32: Periodic Table R08](https://reader034.vdocument.in/reader034/viewer/2022052410/556155aed8b42a8a7d8b5373/html5/thumbnails/32.jpg)
Mendeleev’s Periodic Table (1869)
Increasing atomic weight/mass Repeating chemical properties/reactivity in rows Left empty spaces…why?
Big Difference?
![Page 33: Periodic Table R08](https://reader034.vdocument.in/reader034/viewer/2022052410/556155aed8b42a8a7d8b5373/html5/thumbnails/33.jpg)
Other Possibilities?
![Page 34: Periodic Table R08](https://reader034.vdocument.in/reader034/viewer/2022052410/556155aed8b42a8a7d8b5373/html5/thumbnails/34.jpg)
Galaxies
![Page 35: Periodic Table R08](https://reader034.vdocument.in/reader034/viewer/2022052410/556155aed8b42a8a7d8b5373/html5/thumbnails/35.jpg)
Spirals
![Page 36: Periodic Table R08](https://reader034.vdocument.in/reader034/viewer/2022052410/556155aed8b42a8a7d8b5373/html5/thumbnails/36.jpg)
Which is your favorite?
Check out this website:
http://www.meta-synthesis.com/webbook/35_pt/pt.html
![Page 37: Periodic Table R08](https://reader034.vdocument.in/reader034/viewer/2022052410/556155aed8b42a8a7d8b5373/html5/thumbnails/37.jpg)
Families
![Page 38: Periodic Table R08](https://reader034.vdocument.in/reader034/viewer/2022052410/556155aed8b42a8a7d8b5373/html5/thumbnails/38.jpg)
Families
Definition: groups of elements that have similar chemical properties Chemical properties: valence number, reactivity
(with water, a base, an acid), behavior in solvents, radioactivity
Physical properties: state, color, m.p. and b.p., hardness, malleablility, density, conductivity, etc.
Examples of Families Alkali Metals, Alkaline Earth Metals, Transition
Metals, Halogens, the Noble Gases Found in columns and/or series (rows)
![Page 39: Periodic Table R08](https://reader034.vdocument.in/reader034/viewer/2022052410/556155aed8b42a8a7d8b5373/html5/thumbnails/39.jpg)
The Top and the Middle
![Page 40: Periodic Table R08](https://reader034.vdocument.in/reader034/viewer/2022052410/556155aed8b42a8a7d8b5373/html5/thumbnails/40.jpg)
Hydrogen, Helium and Transition Metals Hydrogen—properties of both group I and VII
sometimes missing an electron +1; sometimes with an extra electron -1; doesn’t belong to any family
Helium—placed in group VIII yet unlike all other elements, it can only have two
electrons in its outer shell
Transition Metals —in center section have special electron rules +2 (unless otherwise noted)
Cu I, Cu IV, etc.
![Page 41: Periodic Table R08](https://reader034.vdocument.in/reader034/viewer/2022052410/556155aed8b42a8a7d8b5373/html5/thumbnails/41.jpg)
Alkali Metals (Li, Na, K, Rb, Cs, Fr) Most reactive family of metals
Group I: only 1 e- in outer shell More reactive as move down the group, as size increases
Never found free in nature Kept under oil in lab
Metals (but not always typical metals*) Good conductors of heat/electricity Malleable and ductile All soft (can be cut with a knife) and shiny and lighter
(less dense) than other metals (float on water)* Solid at room temperature*
M.P and B. P are positive/lower than most metals
![Page 42: Periodic Table R08](https://reader034.vdocument.in/reader034/viewer/2022052410/556155aed8b42a8a7d8b5373/html5/thumbnails/42.jpg)
Alkali Metals
Form ionic compounds (+1 positive ion, cation) Compounds formed are white metallic solids Dissolve in water --> colourless solutions
Sodium chloride (NaCl) table salt
Very reactive with water (and chlorine and oxygen) React with water to form bases (alkaline solutions) …
‘Alkali’ metals
Sodium and potassium ions are important parts of body fluids (electrolytes)
Rb, Cs and Fr are dangerous (Fr is radioactive)
![Page 43: Periodic Table R08](https://reader034.vdocument.in/reader034/viewer/2022052410/556155aed8b42a8a7d8b5373/html5/thumbnails/43.jpg)
Alkali Earth Metals(Be, Mg, Ca, Sr, Ba, Ra) 2nd most reactive family of metals
Group II: 2 e- in outer shell Lose valence electrons and form positive ions, +2 charge
Never found free in nature
Metals Similar properties to alkali metals
Electrical conductors; malleable and ductile Silvery but harder and more dense, w/ higher M.P and B.P Form ionic compounds, react with water to form alkaline
suspensions Na and K, and Ca and Mg ions are important in our
bodies
![Page 44: Periodic Table R08](https://reader034.vdocument.in/reader034/viewer/2022052410/556155aed8b42a8a7d8b5373/html5/thumbnails/44.jpg)
Transition Metals
21 (Scandium) through 29 (Copper)
39 (Yttrium) through 47 (Silver)
57 (Lanthanum) through 79 (Gold)
89 (Actinium)
and all higher numbers
![Page 45: Periodic Table R08](https://reader034.vdocument.in/reader034/viewer/2022052410/556155aed8b42a8a7d8b5373/html5/thumbnails/45.jpg)
Transition Metals
able to put more than 8 e-
(up to 32 electrons) in the shell that is one in from the outermost shell gold (Au) 2-8-18-32-18-1
can use the two outermost shells to bond with other elements allows them to bond with many elements in a
variety of shapes
range of oxidation states
![Page 46: Periodic Table R08](https://reader034.vdocument.in/reader034/viewer/2022052410/556155aed8b42a8a7d8b5373/html5/thumbnails/46.jpg)
Transition Metals
Very good conductors of heat/electricity Malleable and ductile Hard, tough, strong High M.P. and density Low reactivity (compared to Group I and II Metals)
Most form brightly colored compounds Uses: building structures, electric cables,
radiators, colored paints, catalysts for industrial reactions, etc.
![Page 47: Periodic Table R08](https://reader034.vdocument.in/reader034/viewer/2022052410/556155aed8b42a8a7d8b5373/html5/thumbnails/47.jpg)
The Halogen Family(F, Cl, Br, I, At) Group XVII: 7 e- in their outer shell
Very reactive—with many different elements (especially Group I and II metals)
Form both ionic and covalent compounds (-1 anion) Never found free in nature; always in compounds
Nonmetals See: diatomics Electrical insulators Crumbly and brittle (solid) Characteristic colors and odors M.P. and B. P. are low solid (I2), liquid (Br2) or gaseous (F2 , Cl2) at R.T. Can be poisonous Used in bleaches, insecticides, dry cleaning, toothpaste
![Page 48: Periodic Table R08](https://reader034.vdocument.in/reader034/viewer/2022052410/556155aed8b42a8a7d8b5373/html5/thumbnails/48.jpg)
The Noble Gases(He, Ne, Ar, Kr, Xe, Rn) Group VIII: All have full outer shells (2 e- for
Helium, 8 e- for all others) Unreactive, ‘stable’ or ‘inert’ (no need to react!) Always found free in nature; monatomic
Nonmetals Colorless gases at R.T. (Earth’s atmosphere) Low B.P.
Uses: advertising signs and fluorescent lighting (neon), light bulbs (argon), car headlights (xenon), balloons and airships (helium), lasers (krypton)