I II IIISMP, Periodic Table Notes 2017 1

The Periodic Table- Topic 5

Click for song

1. Check your HW answers on the side board

2. Homework: Read pages 78-83 in RB & complete # 1-29

on separate paper (read carefully)

3. Take out guide & turn to pg 5 for notes

Mendeleev’s Periodic Table (1869)

How did Mendeleev organize his periodic table?The Abbreviated History of the Periodic Table for Regents Chemistry

6.1

2

Searching For an Organizing Principle

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

4

B. Henry Moseley

ORGANIZED

ELEMENTS BY

INCREASING ATOMIC

NUMBER.

Resolved discrepancies

in Mendeleev’s

arrangement.

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

Created the Modern Periodic Table known as the Periodic Law

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

Atom

ic Ra

dius

(pm)

The Periodic Law

In 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.

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1. Horizontal rows

Called PERIODS

All 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

SMP, Periodic Table Notes 2015 8

2. Vertical Columnsa) Called GROUPS OR FAMILIES

b) 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 =

Mg+2 Cl-1 = = Remember: When writing

formulas, use the criss-

cross rule to cancel out

oxidation states

BeCl2

MgCl2

SQUARES IN THE PERIODIC TABLE

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S M P , P E R I O D I C T A B L E N O T E S 2 0 1 5

Metals on

the left

Nonmetals

on the right

Metalloids (touch the staircase)

III. Comparing Metals, Nonmetals & Metalloids

Group 18 are

Noble Gases

• Elements on the Periodic Table are divided into three

subgroups called METALS, NONMETALS and

METALLOIDS (semimetals).

Decrease metallic properties

Increase

metallic

properties

Increase

nonmetallic

properties

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Periodic Metallic Properties – click on PT

to watch video

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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 to form

positive ions with smaller radii

❑ have LOW IONIZATION ENERGY (energy needed to remove electrons)

❑ Metallic character INCREASES as ionization energy decreases.

❑ have a low electronegativity (attraction for electrons)

❑ form POSITIVE IONS (cations) when combining with other atoms

❑ FRANCIUM most reactive metal

See Table J

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2. Metal Physical Properties❑ good conductors of heat and electricity due to the

mobility of their 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) & most have densities greater than water (alkali

metals will float)

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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 (anions) 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

© 2002 Prentice-Hall,

Inc.

SMP, Periodic Table Notes 2015 15

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 & CHEMICAL &

PHYSICAL PROPERTIES forms from the same element.

CARBON: coal; diamond,

graphite

OXYGEN: O2; O3 (OZONE)

phosphorus

2. Nonmetals Physical Properties

Carbon Allotropes

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, & At

Exhibit properties of BOTH metals

and nonmetals

Behave as nonmetals but their

conductivity is like metals

SEMICONDUCTORS – Si and Ge

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BELLWORK

1) Turn in your Meticulous Metals lab

2) Take out your colored PT–QUIZ . Turn

quiz in when finished.

3) Open RB and read pages 85-87 (UP TO

PROPERTIES OF GROUPS).

4) Be prepared to take notes – pg 9 of guide

5) HW: pgs 7-8

18

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Trends in the Periodic Table

Many 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)

20

IONIZATION ENERGY (IE)

Energy needed to remove the most loosely

bound electron from a neutral gaseous atom

X + energy X+ + e-

ATOMS WITH A HIGH IONIZATION ENERGY HOLD ONTO ELECTRONS

MORE EASILY AND ARE LESS LIKELY TO GIVE THEM UP.

ATOMS WITH A LOW IONIZATION ENERGY HOLD ONTO ELECTRONS

LOOSELY AND ARE MORE LIKELY TO LOSE ELECTRONS

SMP, Periodic Table Notes 2015

21

IE TRENDS IN A PERIOD: as you move across left to right on the table, values generally INCREASES

Why: AS THE #PROTONS INCREASES, THERE IS A GREATER PULL ON THE e’S REQUIRING MORE NRG TO REMOVE THEM

IE TRENDS IN A GROUP: Ionization energy generally DECREASES from the top of the table to the bottom of the table.

Why: Atom size increases making the outermost electron farther away from the nucleus therefore making it easier to remove

Shielding of the nucleus increases

Trends in Ionization Energy

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Trends in Ionization Energy

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Atomic Radii

one half of the distance between the nuclei of two atoms of the same element when the atoms are joined.

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AR TRENDS IN A PERIOD: As you move across left to right on the

table, values generally DECREASES

Why: THE GREATER THE #PROTONS (atomic #), THE STRONGER

THE PULL ON THE E’S BRINGING THEM CLOSER INTO THE

NUCLEUS

http://education-portal.com/search/text/academy.html

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AR TREND in a GROUP: Atomic radii generally INCREASES from the top of the table to the bottom of the table

Why? Due to electron shielding –As you move

down, YOU ADD ANOTHER NRG LEVEL

INCREASING THE SHIELDING (KERNEL E-

BLOCK)

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ELECTRONEGATIVITY: MEASURE OF AN ATOM’S

ABILITY TO ATTRACT ELECTRONS

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

Atoms with a HIGH Electronegativity have a STRONGER attraction

for bonded electrons

Atoms with a LOW Electronegativity have a WEAKER attraction for

bonded electronsSMP, Periodic Table Notes 2015

28

EN TRENDS in a PERIOD: as you move across left to

right on the table, values generally INCREASES

Why: THERE ARE MORE PROTONS (INCREASED

ATOMIC NUMBER) WHICH INCREASES THE

ELECTRONS ATTRACTION

EN TRENDS IN A GROUP: Electronegativity generally

DECREASES from the top of the table 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 (write on a separate sheet of paper)

A LOSS OR GAIN IN ELECTRONS BY AN ATOM WILL

CHANGE THE SIZE OF THE RESULTING ION

Metals lose e’s resulting in smaller ionic radius

Nonmetals gain e’s resulting in larger ionic radius

SMP, Periodic Table Notes 2015 29

Periodic Trend practice

1) Complete Guide pg 10 (do this for periods 1-3 and groups 1 and 2)

• Use colored pencils

2) On loose leaf paper, copy the info below:

3) HW: Complete guide pgs 13-14 30

Trend Across a period Down a group

Ionization energy increases decreases

Electronegativity increases decreases

Atomic radii decreases increases

Metallic properties

decreases increases

Periodic Trends Summary (click on title for video)

(use reference Table S for data comparison)