IIIIII SMP, Periodic Table Notes 20141 The Periodic Table- Topic 5 Click for song Bellwork: Using your RB (pgs 78-83), define the following words in your

I II IIISMP, Periodic Table Notes 2014 1

The Periodic Table- Topic 5

Click for song

Bellwork: Using your RB (pgs 78-83), define the following words in your notebook: family, group, periodic law, period, metal, metalloid, nonmetal

Searching For an Organizing Principle

Chlorine, bromine, and iodine have very similar chemical properties.

Mendeleev’s Periodic Table (1869) How did Mendeleev organize his periodic table? The Abbreviated History of the Periodic Table for

Regents Chemistry

6.1

SMP, Periodic Table Notes 2014 3


A. Dmitri Mendeleev (1869, Russian) Organized elements by

increasing ATOMIC MASS.

Elements with similar chemical properties were grouped together.

There were some discrepancies.

I. HISTORY


B. Henry Moseley

ORGANIZED ELEMENTS BY INCREASING ATOMIC NUMBER.

Resolved discrepancies in Mendeleev’s arrangement.

The Periodic LawIn the modern periodic table, elements are arranged in order of increasing atomic number.

6.1

Mendeleev’s original table was according to mass. This was changed when Moseley discovered atomic number.


When elements are arranged in order of INCREASING ATOMIC #, elements with similar chemical properties appear at regular intervals.

The properties of the elements within a period change as you move across a period from left to right.

The pattern of properties within a period repeats as you move from one period to the next.

0

50

100

150

200

250

0 5 10 15 20Atomic Number

Ato

mic

Ra

diu

s (

pm

)



1. Horizontal rowsCalled PERIODSAll elements in the same period have the same number of ENERGY LEVELS in their atomic structure

A. Arrangement of Table

II. ORGANIZATION OF THE ELEMENTS


2. Vertical Columns

a) Called GROUPS OR FAMILIESb) All elements in the same group have the

same number of VALENCE ELECTRONS, therefore lose or gain the SAME number of electrons, form similar CHEMICAL FORMULAS and have similar CHEMICAL PROPERTIES

ex. XCl2 Group 2:

Be +2 Cl -1 = BeCl 2

Mg +2 Cl -1 = MgCl2

When writing

formulas, use the

criss-cross rule to

cancel out

oxidation states


Elements can be classified by their properties and located on the Periodic Table as metals, nonmetals, metalloids or semimetals

Metals on the left

Nonmetals on the rightMetalloids or semimetals

III. Comparing Metals, Nonmetals & Metalloids

SMP, Periodic Table Notes 2014

Elements on the Periodic Table are divided into three subgroups called METALS, NONMETALS and METALLOIDS

(semimetals).

Decrease metallic properties

Decrease metallic propertiesIncrease Increase

metallic metallic

propertiespropertiesIncrease Increase

nonmetallic nonmetallic

propertiesproperties


METALS: located on the LEFT SIDE of the periodic table (except H); MORE THAN 2/3 of all elements

1. Chemical properties tend to LOSE ELECTRONS EASILY (form + ions

with smaller radii) have LOW IONIZATION ENERGY (energy

needed to remove electrons) Metallic character INCREASES as ionization

energy decreases. have LOW ELECTRON AFFINITY (attraction for

electrons) form POSITIVE IONS when combining with

other atoms FRANCIUM most reactive metal: See Table J

http://castlelearning.com/review/reference/chem%20table%20j.htm


2. Metals Physical Properties

good conductors of heat and electricity due to their mobile valence electrons

LUSTROUS - reflect light, shine when they are polished

MALLEABLE - can be rolled or hammered into sheets

DUCTILE - can be drawn into wires are SOLIDS at room temperature

except for MERCURY (liquid)


B. NONMETALS- located on the right side of the periodic table (except for Noble gases)

1. Chemical properties tend to GAIN electrons to form

negative IONS with radii larger than their atoms

have high electron affinities (electronegativity)

produce COVALENT bonds by SHARING electrons with other nonmetals

FLUORINE most reactive nonmetal: see Table J


2. Nonmetals Physical Properties exist as gases, molecular solids, or

network solids at room temperature except BROMINE (liquid)

BRITTLE - (shatters when struck) DULL - does not reflect light even when

polished POOR CONDUCTORS of heat and

electricity Allotropes: Different SHAPE & PROPERTIES

forms from the same element.CARBON: coal; diamond, graphite OXYGEN: O2; O3 (OZONE)

Know the definition & examples

C. METALLOIDS (semi-metals)

Found lying on the jagged line between metals and nonmetals flatly touching the line (except Al and Po).

B,Si,Ge,As, Sb, & Te Exhibit properties of both

metals and nonmetals Behave as nonmetals but

their conductivity is like metals

SEMICONDUCTORS – Si and GeSMP, Periodic Table Notes 2014 16

Class/Home work - Trends

Complete pg 7 of guide by reading pgs 85-87 in RB (preferably in pencil)

Complete guide pgs 8-9 On pg 8, only collect trend data for

groups 1 and 7, and periods 2 and 4

Quiz Friday



Trends in the Periodic TableMany properties of the elements change in a predictable way as you move through the periodic table – these systematic trends are called periodic trends. (use reference Table S for data comparison)


1

2

3

4 5

6

7

INCREASES

DECREASES

Definition: AMOUNT OF ENERGY NEEDED TO REMOVE AN e- FROM AN ATOM.

TRENDs in a PERIOD as you move across left to right, values generally INCREASES Why?: AS THE #PROTONS (AKA: NUCLEAR CHARGE) INCREASES,

THERE IS A GREATER PULL ON THE E’S REQUIRING MORE NRG TO REMOVE THEM

TRENDs in a group: IE generally DECREASES from move top to bottom? Why?: Atom size increases making the outermost electron

farther away from the nucleus therefore making it easier to remove; Nuclear Shielding increases

1.IONIZATION ENERGY (IE)


© 1998 LOGAL

2. Atomic Radii

DEFINITION: ½ THE

DISTANCE BETWEEN 2

ADJACENT NUCLEI


TRENDs in a PERIOD as you move

across left to right, values

generally DECREASES

Why? THE GREATER THE

#PROTONS (NUCLEAR CHARGE),

THE STRONGER THE PULL ON THE

e’S BRINGING THEM CLOSER INTO

THE NUCLEUS (SHIELDING)

TRENDs in a group: AR generally

INCREASES from the top of the to

the bottom of the table.

Why? AS EACH ELEMENT GOES

DOWN A GROUP, YOU ADD

ANOTHER NRG LEVEL INCREASING

THE SHIELDING


3. ELECTRONEGATIVITY (EN)

DEFINITION: MEASURE OF AN ATOM’S ABILITY TO ATTRACT ELECTRONS

Atoms with a HIGH Electronegativity have a STRONGER attraction for bonded electrons

Atoms with a LOW Electronegativity have a WEAKER attraction for bonded electrons

Based on a scale of 4, Fluorine has the greatest EN


EN TRENDs in a PERIOD as you move across left to right, values generally INCREASES Why?: THERE ARE MORE PROTONS (INCREASED

ATOMIC NUMBER) WHICH INCREASES THE ELECTRONS ATTRACTION

EN TRENDs in a group: EN generally DECREASES from the top of the to the bottom of the table. Why?: AS YOU GO DOWN A GROUP THERE ARE MORE

ELECTRONS AND MORE NRG LEVELS SO THE ATTRACTION GETS WEAKER


IONIC RADIUS

Definition: A LOSS OR GAIN

IN ELECTRONS BY AN ATOM WILL

CHANGE THE SIZE OF THE

RESULTING ION

Ionic Radii

Metals Nonmetals


METALS:

LOSE electrons and form CATIONS (and get smaller)

ACROSS A PERIOD Explanation: METALS LOSE

ELECTRONS FROM THEIR valence SHELL

Trend: ionic size DECREASES

DOWN A GROUP Explanation: AS YOU MOVE

DOWN A GROUP, YOU ADD ANOTHER ENERGY LEVEL THEREBY INCREASING THE SIZE DUE TO THE INCREASED # OF ELECTRONS

Trend: ionic size INCREASES


NONMETALS: tend to GAIN electrons and form

ANIONS (and get larger).

ACROSS A PERIOD Explanation: NONMETALS GAIN

ELECTRONS WHICH ARE ATTRACTED TO THE PROTONS IN THE NUCLEUS

Trend: ionic size decreases.

GOING DOWN A GROUP Explanation: YOU ADD

ANOTHER ENERGY LEVEL THEREBY INCREASING THE SIZE DUE TO THE INCREASED # OF ELECTRONS

Trend: ionic size INCREASES© 2002 Prentice-Hall, Inc.


Periodic Trends Summary(use reference Table S for data comparison)

Trend Across a Across a period period

Down a Down a groupgroup

Ionization energy

increasesincreases decreasesdecreases

Electronegativity

increasesincreases decreasesdecreases

Atomic radii decreasesdecreases increasesincreases

Metallic properties

decreasesdecreases increasesincreases

Click on for video clip


IV. Classification

Alkali MetalsAlkaline Earth MetalsTransition MetalsHalogensNoble Gases

Click for

song


Group 1: Alkali Metals

extremely reactive (not found free in nature) -form stable ionic compounds

react with water to form a basereact with air to form oxidesreact with acids to form salts

Click on for video clip (2:56 min)


Group 2: Alkaline Earth Metals

reactive (not found free in nature) - form stable ionic compounds

react with water to form a basereact with air to form oxides react with acids to form salts

Click on for video clip


Groups 3-11: Transition Metals

multiple positive oxidation statesLose electrons from two outermost

energy levelsIons form colored solutions

Ex. CuSO4 (due to the Cu 2+ ion)


Group 15 – unique features

Members range from typical nonmetals (nitrogen and phosphorus) through metalloids (arsenic and antimony) to metals (bismuth)

NitrogenForms stable diatomic molecules with a triple

bondComponent of proteinForms some unstable compounds that are used as

explosives

PhosphorusComponent of nucleic acids (DNA, RNA)More reactive than nitrogen at room temperature


Group 16 – unique Features

Members range from typical nonmetals (oxygen and sulfur) through metalloids (selenium and tellurium) to metals (polonium)

Solids except oxygen Oxygen can exist as O2 and O3 (it is an allotrope)

Polonium is radioactive


Group 17: Halogens

very reactive nonmetals - high electronegativity

not found free in natureform diatomic molecules when

freereact with metals to form salts

(halides)Found in all three phases (s, l,

g) due to differences in Van der Waals forces (these are weak)


Group 18: Noble Gases

Have complete outer shellsAlmost inert (not reactive);

stableKrypton, xenon, and radon

form compounds with oxygen and fluorine

Referred to as monatomic gases

Documents

IIIIII SMP, Periodic Table Notes 20141 The Periodic Table- Topic 5 Click for song Bellwork: Using your RB (pgs 78-83), define the following words in your