1. The Periodic Table

2. History of the Table Dmitri Mendeleev (Russia)
The 1st chemist to arrange the newly found elements into a table/usable manner
Arranged them according to atomic mass
This caused gaps or periodic intervals being out of order
History of the Table

3. History of the Table Henry Moseley (England)
Used X-ray spectra to prove the existence of the protons
Arranged the table by atomic number (# of protons)
Gaps are now gone
Modern day periodic table
History of the Table

4. Elements in the periodic table are periodic functions of their atomic number
Periodic Law

5. 1. as you move down a group (column), you add 1 principal energy level or electron shell
2. as you move across a period (row), you add 1 proton to the nucleus, and 1 electron to the valence shell
Periodic Law

6. 3. the maximum number of valence electrons any element can have is eight
Any element with 8 valence electrons signifies the end of a period
The next element will be the start of a new period with 1 valence electron
PERIOD ( ROW)
Periodic Law

7. 4. the number of valence electrons determines the number of bonds an atom can form
Periodic Law

8. 5. the number of bonds an element can form determines the element’s chemical properties
6. all elements in the same group have the same number of valence electrons
They also have similar chemical properties
Group (column)
Periodic Law

10. Arrangement of the Periodic Table
The table is made up of periods and groups
Periods= horizontal rows (run left to right)
Groups= vertical columns (run up & down)
Octet= full valence shell (8 electrons)
Except for period 1 elements 2 electrons make a full valence shell
Arrangement of the Periodic Table

11. The Groups Group 1 Alkali metals (Family)
All have 1 valence electrons
Easily lose their one electron to become +1 ion
Extremely reactive  never found alone in nature
Contains most reactive metal
Francium-which is very rare
Cesium is the second most reactive
The Groups

12. The Groups Group 2 Alkaline Earth Metals (Family)
All have 2 valence electrons
Prefer to lose their two electrons to become +2
Fairly reactive-never found alone in nature
The Groups

13. The Groups Groups 3-12 Transition Metals
Found in the middle of the table (D block)
Form colored ions in solution
Tend to be unpredictable almost every transition metal can form different #s of bonds depending on what other elements or polyatomic ions are present
Have multiple oxidation states
Least reactive group of metals
Most likely to be found uncombined in natured
Ex. Cu is bright blue when dissolved in water
Polyatomic ion- molecular ion
two or more atoms bonded together
Oxidation state- the degree of oxidation (how many electrons an atom can lose)
The Groups

14. The Groups Groups 13-16 BCNO (not a single group)
Miscellaneous groups
Metals, nonmetals, & metalloids found along the staircase
Many different properties
The Groups

15. The Groups Group 17 Halogens (family) 7 valence electrons
Like to gain 1 electron to become ions with -1 charge
Form salts/compounds called halides
Contains the most reactive nonmetal: Fluorine (F)
All nonmetals
Three states of matter found in group:
Solid, liquid, gas
The Groups

16. The Groups Group 18 Noble Gases (Family) Unreactive or inert Octet
Most stable group: exist alone in nature
Exception to the octet is He ) only has 2 valence electrons
The Groups

17. The Groups Hydrogen not officially part of a group
Both a nonmetal and a gas
Can be seen as H2 or H+ or H-
The Lanthanide/Actinide Series- two rows on bottom of the table
Detached
Elements 58-79
Belong to nonmetals
Lanthanide Rare earth elements
Actinide- radioactive due to instability
The Groups

18. The Periodic Table The Staircase 1. metals: make up most of the table
Left of or below “staircase”-except H
All solids (except Hg)
Must have all four properties of a metal
1. malleable (can be hammered/molded into sheets)
2. ductile (can be drawn/pulled into wire)
3. have luster (are shiny when polished)
4. good conductors (allow heat & electricity to flow through them)
Due to sea of mobile valence electrons
Like to lose electrons to form positive ions
The Periodic Table

19. The Periodic Table 2. Nonmetals Right of or above the staircase
Mostly gases and Br
Not malleable/ductile; brittle (shatter easily)
Lack luster (dull)
Non or poor conductors
Like to gain electrons to form negative ions
May have one or zero properties of a metal
The Periodic Table

20. The Periodic Table 3. Metalloids (aka semi metals)
Have two properties of a metal
Along staircase (between metals and nonmetals )
Except Al
The Periodic Table

22. Phases of Matter at STP Solids (s)- most elements are solids at STP
Definite volume
Definite shape
Phases of Matter at STP

23. 2. Liquids (l) only two elements at STP (Br & Hg)
Definite volume
Takes the shape of the container
Phases of Matter at STP

24. Phases of Matter 3. Gases (g)- H, N, O, F, Cl & noble gases
no definite volume
Fill their container
4. Aqueous (aq) a STATE of matter which one substance (a solute) is dissolved in another (solvent); a solution
Not a phase
Homogenous mixture
Ex. Na Cl
Phases of Matter

25. Elements that are unstable alone in nature pair up in order to fill their valence shells
Both need the same number of electrons to fill the valence shell
Diatomic Elements

26. Diatomic Elements Contain 2 identical atoms 7 of them
Include N2, O2, F2, Cl2, Br2, I2 and H2
Diatomic Elements

27. 1 of 2 or more different forms of an element in the same phase, but with different formulas and different physical/chemical properties
Ex. O2 (oxygen) and O3 (ozone)
Carbon graphite (pencils) and diamonds
Allotrope

28. Periodic Trends As you move across a period
1. nuclear charge increases
a. additional proton
b. Pulls electron cloud in more tightly
2. shielding does not increase
a. kernel electrons interfere with attraction between protons in the nucleus and the valence electrons
b. Every element in the same period/row has the same number of kernel electrons
Shielding draws the electrons toward the nucleus
Periodic Trends

29. Periodic Trends As you move down a group
1. nuclear charge increases but
2. Shielding increases
Additional orbital/energy level means more kernel electrons (-) to interfere with the attraction between the protons and the valence electrons
Valence electrons are able to drift further from the nucleus
Periodic Trends

30. Atomic Radius ½ the distance between neighboring nuclei of a given element
Periodic Trends

31. Periodic Trends Moving down a group Moving across a period
Atomic radius increases
Adding energy levels to the outside of the atom take up more space
Moving across a period
Atomic radius decreases
Nuclear charge is increasing
Same # of energy levels, no increase in shielding
Periodic Trends

32. Periodic Trends Ionic Radius- radius of ions
Nonmetals gain electrons radius increases
Same nuclear charge pulling on more e-
Electrons outnumber protons
Electrons drift further away from the nucleus
Periodic Trends

33. Periodic Trend Metal lose electrons  radius decreases
Same nuclear charge pulling on less electrons
Protons outnumber electrons
Electrons are pulled closer to the nucleus
Periodic Trend

34. Isoelectronic series: atoms and ions that have the same number of total electrons
Elements gain or lose electrons in order to attain the electron configuration of the nearest noble gas
All members of an isoelectronic series have the same noble gas configuration
Periodic Trends

35. Periodic Trends Electronegativity Desire to gain electrons
Nonmetals gain electrons to achieve full octet  high electronegativity
Metals lose electrons to achieve full octet low electronegativity
Periodic Trends

36. Periodic Table Electronegativity 0.0 to 4.0
Most electronegative element Fluorine
Least electronegative element cesium or francium
Periodic Table

37. Periodic Trend Going across a period, electronegativity increases
Increased nuclear charge
Shielding does not increase
Going down a group, electronegativity decreases
Increased shielding
Periodic Trend

38. Ionization Energy amount of energy needed to remove the most loosely bound electrons from an atom/ion (in the gas phase)
X + energy  X+ + e-
Periodic Trends

39. Periodic Trends Going across a period, ionization energy increases
Increased nuclear charge
Shielding does not increase
Going down a group, ionization energy decreases
Increased shielding
Periodic Trends

40. Ability or tendency of an element to go through a chemical change or (react with another element)
Metals are loser when it comes to electrons
Nonmetals gain when it comes to electrons
Reactivity

41. Reactivity Metals (francium most reactive)
Going across a period, reactivity decreases
Increased nuclear charge
Shielding does not increase
Going down a group, reactivity increases
Increased shielding
Reactivity

42. Reactivity Nonmetals most reactive Fluorine
Going across a period, reactivity increases
(until you reach the noble gases)
Increased nuclear charge
Shielding does not increase
Going down a group, reactivity decreases
Increased shielding
Reactivity