Chemistry Chapter 5 the Periodic Table

Chemistry Chapter 5Chemistry Chapter 5the Periodic Tablethe Periodic Table

In 1860, Stanislao In 1860, Stanislao Cannizzaro Cannizzaro presented a presented a method for method for accurately accurately measuring the measuring the relative atomic relative atomic masses of the masses of the elements.elements.

Chemistry Chapter 5Chemistry Chapter 5The Periodic LawThe Periodic Law

In 1869, Dmitri Mendeleev published his In 1869, Dmitri Mendeleev published his first “periodic table”. first “periodic table”. – He started by placing the known elements in He started by placing the known elements in

order using their atomic masses.order using their atomic masses.– He recognized that certain properties repeated He recognized that certain properties repeated

themselves “periodically”.themselves “periodically”.– He then rearranged the elements so that He then rearranged the elements so that

elements with similar properties appeared elements with similar properties appeared together in his table.together in his table.

– His procedure left empty spaces for elements His procedure left empty spaces for elements that had not been discovered. that had not been discovered.

Moseley & the Periodic LawMoseley & the Periodic Law

In 1911, Henry Moseley discovered that In 1911, Henry Moseley discovered that the periodic table fit better when the the periodic table fit better when the elements were placed in order elements were placed in order according to their increasing positive according to their increasing positive charge.charge.

This led to the principle of chemical This led to the principle of chemical periodicity known as the:periodicity known as the:– periodic law-periodic law- The physical and chemical The physical and chemical

properties of the elements are periodic properties of the elements are periodic functions of their atomic numbers.functions of their atomic numbers.

The Modern Periodic TableThe Modern Periodic Table

The The periodic tableperiodic table is an is an arrangement of the elements in arrangement of the elements in order of their atomic numbers so that order of their atomic numbers so that elements with similar properties fall elements with similar properties fall in the same column, or group.in the same column, or group.– group (or family)-group (or family)- the vertical the vertical

columns of the periodic tablecolumns of the periodic table– period-period- the horizontal rows of the the horizontal rows of the

periodic tableperiodic table

The Modern Periodic TableThe Modern Periodic Table noble gases-noble gases- the group 18 elements which the group 18 elements which

are not reactive (inert)are not reactive (inert) lanthanides (rare earth elements)-lanthanides (rare earth elements)-

elements 58-71 at the bottom of the periodic elements 58-71 at the bottom of the periodic table that are very similar in properties and table that are very similar in properties and represent the 4represent the 4thth energy level “f” orbital energy level “f” orbital block elements from period 6.block elements from period 6.

actinides-actinides- elements 90-103 are all elements 90-103 are all radioactive and represent the 5radioactive and represent the 5thth energy energy level “f” orbital block elements from period level “f” orbital block elements from period 7.7.– Do section review #3 & 5 on page 137.Do section review #3 & 5 on page 137.

Section Review- page 137Section Review- page 137

3-3- The noble gases, the The noble gases, the lanthanides , and lanthanides , and the actinides have been the actinides have been addedadded. They . They were not yet discovered when were not yet discovered when Mendeleev Mendeleev wrote the original periodic table wrote the original periodic table and he had and he had no way of predicting their no way of predicting their existence.existence.

5-5- The periodic table is arranged The periodic table is arranged according to according to atomic numberatomic number, not atomic , not atomic mass. The mass. The average atomic mass on the average atomic mass on the periodic table is periodic table is the weighted average of the the weighted average of the isotopes of an isotopes of an element and some elements element and some elements have large have large percentages of heavy isotopes.percentages of heavy isotopes.

Electron Configuration & the Periodic Electron Configuration & the Periodic TableTable

s-block elements-s-block elements- are groups #1 & #2 in are groups #1 & #2 in which a single “s” orbital is being filled in the which a single “s” orbital is being filled in the energy level equal to the period number.energy level equal to the period number.

– alkali metals-alkali metals- are the group #1 metals that are are the group #1 metals that are so reactive that they do not exist as pure elements so reactive that they do not exist as pure elements in naturein nature

– alkaline-earth metals-alkaline-earth metals- are the group #2 metals are the group #2 metals that also are very reactive and do not exist alone that also are very reactive and do not exist alone in naturein nature

– Do problem #1 on page 143.Do problem #1 on page 143.

Practice problem page 143Practice problem page 143

1-1- What is the period, group and What is the period, group and block of block of [Kr]5s[Kr]5s1 1 ??

[Kr]5s[Kr]5s11 tells us the element tells us the element rubidium is rubidium is in the: in the:

55thth period period

11stst group group

s-block s-block


p-block elements-p-block elements- are groups #13- are groups #13-#18 in which 3 “p” orbitals are being #18 in which 3 “p” orbitals are being filled in the energy level equal to the filled in the energy level equal to the period number.period number.

– halogens-halogens- are the group 17 elements are the group 17 elements

– noble gases-noble gases- are the group 18 are the group 18 elements that are non-reactive (inert)elements that are non-reactive (inert)

– Do practice problems #1 & 2 on page Do practice problems #1 & 2 on page 148.148.

Practice problems page 148Practice problems page 148

1a-1a- Write the outer electron configuration Write the outer electron configuration of the of the group 17 element in the 3group 17 element in the 3rdrd period.period.

3s3s223p3p55

1b-1b- Identify the element and identify it as a Identify the element and identify it as a metal, metalloid, or nonmetal.metal, metalloid, or nonmetal.

chlorine (Cl)chlorine (Cl)

nonmetalnonmetal


2a-2a- What is the period, block and group What is the period, block and group of the of the element [Ar]3delement [Ar]3d10104s4s224p4p33 ? ?

period 4period 4

p-blockp-block

group 15 (5A)group 15 (5A)

2b-2b- What is the name of the element and What is the name of the element and is it a is it a metal, metalloid or nonmetal?metal, metalloid or nonmetal?

arsenic (As) is a metalloidarsenic (As) is a metalloid


d-block elements (transition d-block elements (transition metals)-metals)- group #3-#12 elements in group #3-#12 elements in which 5 “d” orbitals are being filled in which 5 “d” orbitals are being filled in the energy level equal to the period # the energy level equal to the period # minus 1.minus 1.

– They are metals that have typical metallic They are metals that have typical metallic properties.properties.

– Do practice problems #1 & 2 on page 146.Do practice problems #1 & 2 on page 146.


1-1- What is the period, group, & block of What is the period, group, & block of the the element [Ar]3delement [Ar]3d884s4s22 ? ?

period 4period 4

group 10group 10

d blockd block

2-2- What is the electron configuration of What is the electron configuration of the the element in group 12 of the fifth period?element in group 12 of the fifth period?

[Kr]4d[Kr]4d10105s5s22


f-block elements-f-block elements- are the two rows at the are the two rows at the bottom of the periodic table that represent 7 “f” bottom of the periodic table that represent 7 “f” orbitals being filled in the energy level that is orbitals being filled in the energy level that is equal to the period number minus 2equal to the period number minus 2

– lanthanides-lanthanides- elements # 58-71 that are also elements # 58-71 that are also called the rare earth elementscalled the rare earth elements

– actinides-actinides- elements #90-103 that are all elements #90-103 that are all radioactiveradioactive elements 93(neptunium) through 103 elements 93(neptunium) through 103

(lawrencium) are all man-made and do not (lawrencium) are all man-made and do not occur naturallyoccur naturally

QuestionsQuestions

Do Practice Do Practice problem #1 on problem #1 on page 149.page 149.

Do Section Review Do Section Review problems #2, 4, & problems #2, 4, & 5.5.

Practice problem on page 149Practice problem on page 149

For each of the following identify the block, For each of the following identify the block, period, group, group name, element name, period, group, group name, element name, element type, and relative reactivity.element type, and relative reactivity.

1a-1a- [He]2s[He]2s222p2p55

p-block, period 2, group 17, halogen, p-block, period 2, group 17, halogen, fluorine (F), nonmetal, & highly reactive fluorine (F), nonmetal, & highly reactive

1b-1b- [Ar]3d[Ar]3d10104s4s11

d-block, period 4, group 11, transition d-block, period 4, group 11, transition metal, metal, copper (Cu), metal, & low reactivitycopper (Cu), metal, & low reactivity

Section review page 149Section review page 149

2a-2a- group 1 is the alkali metalsgroup 1 is the alkali metals

b-b- group 2 is the alkaline earth metalsgroup 2 is the alkaline earth metals

c-c- groups 3-12 are the transition metalsgroups 3-12 are the transition metals

d-d- group 17 is the halogensgroup 17 is the halogens

e-e- group 18 is the noble gasesgroup 18 is the noble gases

4-4- noble gas noble gas electron configuration of electron configuration of the the group 15 period 4 elementgroup 15 period 4 element

[Ar]3d[Ar]3d10104s4s224p4p33

5-5- period, block, & group of [Ar]3dperiod, block, & group of [Ar]3d774s4s22

period 4, d-block, group 9period 4, d-block, group 9

Electron Configuration & Periodic Electron Configuration & Periodic PropertiesProperties

atomic radius-atomic radius- one-half the distance one-half the distance between the nuclei of identical atoms that between the nuclei of identical atoms that are bonded together.are bonded together.

– As you go across a period, the positive charge As you go across a period, the positive charge of the nucleus increases across a period, the of the nucleus increases across a period, the pull exerted on the electron cloud increases pull exerted on the electron cloud increases and the atomic radius of the elements and the atomic radius of the elements decreasesdecreases across the period across the period..

– As you move down a group, each successive As you move down a group, each successive element adds an energy level so the atomic element adds an energy level so the atomic radii radii increaseincrease down a group down a group..


ion-ion- an atom or group of atoms that an atom or group of atoms that has a positive or negative chargehas a positive or negative charge

ionization-ionization- any process that results any process that results in the formation of an ionin the formation of an ion

ionization energy-ionization energy- the amount of the amount of energy required to remove one energy required to remove one electron from a neutral atom of an electron from a neutral atom of an elementelement

– ionization energies of the main group ionization energies of the main group elements elements increaseincrease across a period across a period

– ionization energies of the main group ionization energies of the main group elements usually elements usually decreasedecrease down a down a groupgroup


electron electron affinity-affinity- the energy the energy change that occurs when an electron change that occurs when an electron is acquired by a neutral atomis acquired by a neutral atom

cation-cation- an ion with a positive an ion with a positive charge due to the loss of electronscharge due to the loss of electrons

anion-anion- an ion with a negative an ion with a negative charge due to the gain of electrons charge due to the gain of electrons


valence electrons-valence electrons- the electrons the electrons available to be gained, lost, or available to be gained, lost, or shared by atoms in the formation of shared by atoms in the formation of chemical bonds to make compoundschemical bonds to make compounds

electronegativity-electronegativity- a measure of a measure of the ability of an atom in a chemical the ability of an atom in a chemical compound to attract electrons from compound to attract electrons from another atom in the compoundanother atom in the compound

– electronegativity tends to electronegativity tends to increase increase across a periodacross a period and either decrease or and either decrease or remain the same down a groupremain the same down a group

– fluorine (F) is the most electronegative fluorine (F) is the most electronegative of the elements.of the elements.

Chapter 5 ReviewChapter 5 Review

Chapter Review problems pages 166-Chapter Review problems pages 166-168168

#1, 2, 8, 9, 11, 13, 17, 18, 19, #1, 2, 8, 9, 11, 13, 17, 18, 19, 22, 23, 22, 23, 28, 32, & 40. 28, 32, & 40.

Chapter 5 Test Review ExerciseChapter 5 Test Review Exercise

1-1- Which elements are called:Which elements are called:

a-a- alkali metalsalkali metals

b-b- alkaline earth metalsalkaline earth metals

c-c- transition metalstransition metals

d-d- halogenshalogens

e- e- noble gasesnoble gases

f-f- lanthanideslanthanides

g-g- actinidesactinides

2-2- What were the major contributions of:What were the major contributions of:

a- a- Dmitri MendeleevDmitri Mendeleev

b-b- Henry MoseleyHenry Moseley

3-3- What is the period number, group What is the period number, group number, number, block, & identity of the element block, & identity of the element designateddesignated

[Kr]4d[Kr]4d10105s5s225p5p55

4-4- What are valence electrons and where What are valence electrons and where are they are they found?found?

5-5- What are the period and group trends What are the period and group trends for the for the atomic radius of the elements?atomic radius of the elements?

Helpful Hints- Periodic Table Helpful Hints- Periodic Table LabLab

Make note that the sets of elements on page one are in Make note that the sets of elements on page one are in groups (vertical columns).groups (vertical columns).

The table is for the “s” and “p” blocks ONLY, no “d” or “f” The table is for the “s” and “p” blocks ONLY, no “d” or “f” block elements are included.block elements are included.

The clues given are for periods 1 through 4 ONLY.The clues given are for periods 1 through 4 ONLY. The formulas of oxides always end with the element The formulas of oxides always end with the element

oxygen.oxygen. The elements that are liquid at room temperature are The elements that are liquid at room temperature are

written in blue on the table at the front of the room.written in blue on the table at the front of the room. The “outer energy level” includes “s” & “p” orbitals ONLY.The “outer energy level” includes “s” & “p” orbitals ONLY. The elements that are gas at room temperature are The elements that are gas at room temperature are

written in red on the table at the front of the room.written in red on the table at the front of the room. The metalloids include B, Si, Ge, As, Sb, & Te.The metalloids include B, Si, Ge, As, Sb, & Te. Periods 5 & 6 (AA-PP) will be filled out using page 3 of the Periods 5 & 6 (AA-PP) will be filled out using page 3 of the

lab. Match the element properties with those on appendix lab. Match the element properties with those on appendix A.A.

Chemistry Chapter 5 Vocabulary QuizChemistry Chapter 5 Vocabulary QuizMonday 11/7/2011Monday 11/7/2011

Dmitri Mendeleev Dmitri Mendeleev periodic lawperiodic lawperiodic table periodic table group group period period noble gasesnoble gaseslanthanides actinideslanthanides actinides

alkali metals alkali metals alkaline-earth alkaline-earth metals metals halogens halogens d-block d-block elements elements atomic radius atomic radius ionization ionization ionization energy ionization energy electronelectron affinityaffinity cationcation anion anion

valence electronsvalence electronselectronegativityelectronegativity

Chemistry Chapter 5 Test ReviewChemistry Chapter 5 Test Review

25 multiple choice questions:25 multiple choice questions: Mendeleev & his 1Mendeleev & his 1stst periodic table periodic table Definitions, locations, & properties of lanthanides, Definitions, locations, & properties of lanthanides,

actinides, noble gases, halogens, alkali metals, actinides, noble gases, halogens, alkali metals, alkaline earth metals, & transition metalsalkaline earth metals, & transition metals

Definitions of periodic law, groups, periods, atomic Definitions of periodic law, groups, periods, atomic radius, electronegativity, cation, anion, & valence radius, electronegativity, cation, anion, & valence electronselectrons

Where are valence electrons located?Where are valence electrons located? Period & group trends for atomic radiusPeriod & group trends for atomic radius What form do alkali metals take in nature?What form do alkali metals take in nature? Determine the number of valence electrons for Determine the number of valence electrons for

different groupsdifferent groups

Honors Chemistry Chapter 5 Test Honors Chemistry Chapter 5 Test ReviewReview

35 multiple choice questions worth two points each. 35 multiple choice questions worth two points each.

Know the definition and inventor (Mendeleev) of the Know the definition and inventor (Mendeleev) of the first periodic table and how he arranged the elements.first periodic table and how he arranged the elements.

Know how the modern periodic table is arranged and Know how the modern periodic table is arranged and what groups of elements have been added to it.what groups of elements have been added to it.

Know the groups and names and unique properties of Know the groups and names and unique properties of the alkali metals, alkaline earth metals, halogens, noble the alkali metals, alkaline earth metals, halogens, noble gases, transition metals, lanthanides, and actinides.gases, transition metals, lanthanides, and actinides.

Know the definition of the periodic law, periods, groups.Know the definition of the periodic law, periods, groups. Identify the period & group for a specific element.Identify the period & group for a specific element.

next slidenext slide

Know the general location of the metals, Know the general location of the metals, metalloids, & nonmetals on the periodic table.metalloids, & nonmetals on the periodic table.

Why is hydrogen often placed away from the Why is hydrogen often placed away from the body of the group 1 elements on a periodic table?body of the group 1 elements on a periodic table?

Know where the s, p, d, & f block element are Know where the s, p, d, & f block element are located and their meaning.located and their meaning.

Know the definitions of ionization energy, Know the definitions of ionization energy, electronegativity, and atomic radius and their electronegativity, and atomic radius and their trends both across a period and down a group.trends both across a period and down a group.

Know the definition of valence electrons & how to Know the definition of valence electrons & how to find their number in s & p groups.find their number in s & p groups.

Chemistry Chapter 5 the Periodic Table

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