Unit 3 Periodic Table Have your Periodic Table

Unit 3: Periodic Table Have your Periodic Table out everyday for this unit Mr. Mellon General Chemistry

I. Historical Development of the Table 1860’s A. Dmitri Mendeleev (_____) • Arranged elements into table based on PHYSICAL and similarities in the _____________ CHEMICAL properties • thought similarities were function ATOMIC MASS of _______ • Noticed that some elements seemed out of order Mendeleev Video Clip

I. Historical Development of the Table 1913 A. Henry Moseley (_____) • Established that properties of elements were ATOMIC NUMBER functions of ______ 1. Present table based on ATOMIC NUMBER ________ 2. Elements’ properties depend on STRUCTURE OF ATOM ________ 3. Properties of elements vary systematically throughout the table

II. Period (or Rows) HORIZONTAL ROWS • __________ • Number at the beginning of the period principle energy level in which indicates the ___________ valence _______ electrons are located 1 PEL 2 PEL 3 PEL Periods

II. Period (or Rows) Example: 4 A) What period is potassium and bromine in? ____ B) Based on the period, how many principal energy levels do potassium and bromine have? ________ 4 • ______ PROPERTIES change as you _____ ACROSS a period

III. Groups(or Families) VERTICAL COLUMNS • _________ SIMILAR chemical properties • Each group has _____ because each group has same number of VALENCE ELECTRONS ____________(except groups 3 – 12) 1 2 3 4 5 6 7 8 # of valence e- Groups

II. Period (or Rows) Example: 2 A) What group is magnesium and calcium in? ______ B) Based on the group, how do the properties of magnesium and calcium compare? Why? Similar because they both have same number of valence electrons (2)

II. Period (or Rows) Sample Questions: 1) Which sequence of atomic numbers represents elements which have similar chemical properties? A) 19, 23, 30, 36 C) 9, 16, 33, 50 B) 3, 12, 21, 40 D) 4, 12, 38, 88 ______ 1) Which two elements have the most similar chemical properties? A) Aluminum and Barium C) Nickel and Phosphorous B) Chlorine and Sulfur D) Sodium and Potassium _________

IV. Metals e- and become • Metal atoms lose _____valence ____ positive _____ ions when bonding. After they lose smaller their electrons they become _______ mixture of metals Homogenous • Alloy: ________ made by _____ them together melting

IV. Metals • Properties of Metals: 1. ____ ionization energy and electronegativity Low 2. _____ conductors of heat and electricity Good metallic luster (shine) 3. Exhibit ____________ 4. Malleable - can be _____ hammered into __________ thin sheets pulled into 5. Ductile - can be _____ thin wires _________ 6. More than _______ 2/3 of the elements are ____ metals High densities 7. _____ Mercury (Hg) a metal which a _____ 8. ________is liquid at room temperature and STP (Hg and Fe anvil video) (Francium) 9. Most reactive metal (bottom left corner): Fr ____ (easiest to lose it valence electrons)

IV. Metals CHECKS FOR UNDERSTANDING 1. Which element is malleable and can conduct electricity in the solid phase? A) Iodine B) Phosphorous C) Sulfur D) Tin 2. What happens to metals when they bond? What would happen to their atomic size? Lose electrons; become smaller 3. Where are the most reactive metals located? What about their atomic structure makes them so reactive? Bottom left corner; the electrons are far away (big atomic radius), so electrons can be easily removed (low ionization energy/electronegativity)

V. Nonmetals gain e- and become • Nonmetal atoms _____valence ____ negative ions when bonding. After they gain _____ larger electrons they become _______

V. Nonmetals • Properties of Nonmetals: High ionization energy and electronegativity 1. ____ Poor 2. _____ conductors of heat and electricity 3. 4. Brittle, soft _______________ Low _______ densities F (Fluorine) (top right corner) 5. Most active nonmetal: ____ (easiest to GAIN electrons) Graphite is an allotrope of carbon (nonmetal). It is used in pencils (brittle, soft, and low density)

V. Nonmetals CHECKS FOR UNDERSTANDING 1. Which element is brittle and not a conductor of electricity? A) Sulfur B) Sodium C) Potassium D) Helium 2. What happens to the number of electrons when nonmetals bond? What happens to their atomic radius when they bond? Gain electrons; become larger 3. Where are the most reactive nonmetals located? What about their atomic structure that makes them so reactive? Top Right corner (Group 17); small atomic radius so they attract electrons (High electronegativity/ ionization energy

VI. Metalloids • Atoms that _____________and form ions gain or lose ewhen bonding metal and nonmetals • Have properties of both _____________ staircase (see periodic • Can be located using the “______” table)

VI. Metalloids CHECKS FOR UNDERSTANDING 1. Which element has both metallic and nonmetallic properties? A) Rb B) Rn C) Si D) Sr 2. Which list of elements contains 2 metalloids? A) B, Ge, Po, Pb C) As, Bi, Br, Kr B) Si, P, S, Cl D) Po, Sb, I, Xe

VII. Periodic Properties A. Atomic Radius: Distance between the center of the ______ to the most outer nucleus shell electron _______ (orbital)

VII. Periodic Properties S - Periodic Trend (See Reference Tables – Table _____): (SIMULATION) ↓ Atomic Radius _____ as you move from left to period right across a __________ Explanation: # of energy levels remains the same _________ and outer e- gets pulled _______ to the nucleus closer ↑ group Atomic Radius _______ as you move down a _______ Explanation: # of energy levels remains the ____ increases

VII. Periodic Properties Atomic Radius Snowman

VII. Periodic Properties B. Ionic Radius: a loss or gain of ecauses an increase or reduction in an atom’s size lose • Metals: _____ electrons when they form positive ______ ions and ionic radius is _____ smaller than neutral atom 2 -8 -1 2 -8

VII. Periodic Properties B. Ionic Radius: gain negative ions • Nonmetals: _____ electrons when they form _____ and ionic radius is _____ bigger than neutral atom 2 -8 -7 2 -8 -8

IV. Periodic Properties Sample Questions: 1) Which element has an atomic radius that is greater than its ionic radius? A) S B) K C) F D) O 2) Explain what happens, in terms of valence electrons and size, when Mg becomes an ion. It loses valence electrons and its radius becomes smaller

VII. Periodic Properties C. Ionization Energy: remove Amount of energy needed to ______ the most loosely bound electron, specifically a valence _______ electron

VII. Periodic Properties - Periodic Trend for Ionization Energy (See Reference Tables – Table _____): S ↑ Ionization Energy _____ as you move from left to right across a _______ period Explanation: number of protons and valence electrons increases and size decreases, so electrons are held tighter ↓ Ionization Energy _____ as you move down a group ____________ Explanation: valance electrons are farther away and shielded by kernel electrons, so they are easier to remove

VII. Periodic Properties D. Electronegativity: measurement of an electrons attraction for _______when atom’s _____ bonded gain Desire of an atom to _____ electrons

VII. Periodic Properties - Periodic Trend for Electronegativity (See Reference Tables – Table _____): S ↑ Electronegativity_____ as you move from left to right across a _______ period Explanation: atomic size decreases, so electrons are closer to the positive nucleus ↓ Electronegativity _____ as you move down a group _________ Explanation: atomic size increases, so outer electrons are not as attracted to positive nucleus

IV. Periodic Properties Check for Understandings • What are the electronegativities for group 18 elements? Why do you think they have “this” electronegativity? They do not have electronegativity numbers. Why? Because they already have their 8 valence electrons (octet) • Which element attracts electrons the most when bonding? A) Ca C) Br B) Sr D) I • Which element gives off its valence electrons the easiest? A) Ca C) Br B) Sr D) I

VIII. Groups within Groups Alkali Metals A. Group 1: ________ soluble (dissolves) water and strongly basic • All ___________in Hydrogen • _________ is the exception on the periodic table – it belongs to no group : ( _______ Brainiac – Alkali Metals MYTHBUSTERS – ALKALI METALS Part 2 (start at 1: 50)

VIII. Groups within Groups Alkaline Earth Metals B. Group 2: ___________ 2 • Have ______valence electrons 2 charge when they bond • Form ______ In general for Groups 1 and 2: reactive As you move down, they become more _______

VIII. Groups within Groups Checks for Understanding 1. As you move down groups 1 and 2 elements become more reactive. Explain why this happens based on atomic size and ionization energy/electronegativity. As atomic size increases, ionization energy decreases (easier to remove e-) so they become more reactive 2. What will be the charge on a Ca ion when it bonds? +2 3. Based on your answer to question 2, what happens to the atomic size once it becomes an ion? Smaller (loses last energy level)

VIII. Groups within Groups Transition Metals C. Groups 3 -12: ________ • dense ____ metals and ____ high melting points • Form ______ multiple ions and _______ less reactive than Groups ______ 1 and 2 color • Form ions that have ______ Copper (II) Sulfate Solution (Cu 2+ ions) Cobalt (II) Chloride Solution (Co 2+ ions)

VIII. Groups within Groups Checks for Understanding 1. Identify the metal that has multiple oxidation states. A) K B) Ba C) Be D) Pd 2. Which compound forms a green aqueous solution? A) Rb. Cl B) Ca. Cl 2 C) Ni. Cl 2 D) Be. Cl 2 3. Which set of properties is most characteristic of transition elements? A) Colorless ions in solutions, multiple positive oxidation states B) Colorless ions in solutions, multiple negative oxidation states C) Colored ions in solutions, multiple negative oxidation states D) Colored ions in solutions, multiple positive oxidation states

VIII. Groups within Groups Halogens D. Group 17: ________ 7 valence e-, become ____ - 1 charged ion • Have ______ • Mostly ________ nonmetallic elements

VIII. Groups within Groups Noble Gases E. Group 18: ________ 8 valence electrons (or _____ 2 for He) • Have _____ full outer energy level • Have a _______ react(easily) because their outer shell is • Do not _______________ full (8 valence e-) stable (do not react easily because their • They are ______ out shell is full) • ALL OTHER ELEMENTS WANT TO BE LIKE THEM BECAUSE THEY HAVE 8 VALENCE ELECTRONS

VIII. Groups within Groups Checks for Understanding 1. Which halogen is most reactive? Explain why, based on atomic size, electronegative/ionization energy. F: smallest in size so attraction for electrons is very high (electronegativity) 2. Explain why noble gases don’t typically react with other elements? Their outer energy level is completely full. They do not want to gain anymore e-

IX. Phases of Matter of Elements • All of the information on the Periodic Table is given at STP ____ and ground state • STP - Standard Temperature and Pressure ( 0 o. C and 1 atm/101. 3 k. Pa (sea level pressure)) H, N, O, F, Cl and Noble gases Br, Hg Everything else

X. Other Categories 2 identical • Diatomics - Molecule containing ________ atoms - They are : H, O, F, Br, I, N, Cl (7 -H club) • Radioactive – nucleus is _______ and unstable breaks down spontaneously (all isotopes are ________ radioactive, but less than the ones mentioned below) - They are : Atomic # greater than 84 and 43 (Technitium), 61 (Promethium)

X. Other Categories man-made elements (all are radioactive, • Synthetic – _______ as well, but disintegrate in milliseconds) - They are : Atomic # greater than 93 and 43 (Technitium), 61 (Promethium) • (NOVA: How they are made)

X. Other Categories 2 or more structural • Allotropes- _______ different _______ forms of an element in the same phase that have different properties _______ Examples: O (g): O 2 – Dioxygen - what we inhale to live O 3 – Ozone - Toxic Carbon (s) Diamond Graphite Coal Buckminster

Eight Allotropes of Carbon Diamond Graphite (pencil “lead”) Lonsdaleite C 60 (buckyball) Amorphous carbon Single-walled carbon nanotube (buckytube)