TN Ch 9.1 Date - Chemistry...Ch 9.6 Notes (Part 1) Topic: Atoms with Orbitals EQ: How do electrons...

TN Ch 9.1 Date

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TN Ch 9.1

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WE WILL ANSWER THEM TOGETHER.

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LEFT Side – PICTURES, PRACTICE PROBLEMS, ETC

Ch 9.1-9.2 Notes

Topic: Light & Electromagnetic

Radiation

EQ: How does light interact with

atoms?

READ Ch 9.1 – 9.2 (pg. 285-288)

Write Questions & Answer Questions #1-5

(notes side) Highlight answer

Electrons in Atoms and the Periodic Table

• We examine two important models—the Bohr

model and the quantum-mechanical

model—that propose explanations for the

inertness of helium, the reactivity of hydrogen,

and the periodic law.

• These models explain how electrons exist in

atoms and how those electrons affect the

chemical and physical properties of elements.

• (Remember – elements in same group have

similar phy/chem prop’s) - Learned this in

Ch 4!!

Electromagnetic Radiation

• The interaction of light with atoms helped to

shape scientists’ models of the atom.

• Light is a form of electromagnetic radiation.

• Light has properties of both waves and

particles.

Light: Electromagnetic Radiation

When a water surface is disturbed, waves are created that

radiate outward from the site. The wave carries energy as

it moves through the water.

• Wavelength: The wavelength of light, λ (lambda), is defined as the distance between adjacent wave crests.

Draw with notes

Light: Color of Light • White light, as produced by the sun or by a lightbulb,

contains a spectrum of wavelengths and therefore a

spectrum of color.

• We see these colors—red, orange, yellow, green,

blue, indigo, and violet—in a rainbow or when white

light is passed through a prism.

• Red light, with a wavelength of 750 nm (nanometers),

has the longest wavelength of visible light.

• Violet light, with a wavelength of 400 nm, has the

shortest wavelength of visible light

(1 nm = 1 × 10–9 m).

• The presence of color in white light is responsible for

the colors we see in our everyday vision.

Components of white light

R O Y G B I V

• Light is separated into its constituent colors—red, orange, yellow, green, blue, indigo, and violet—when it is passed through a prism.

Draw with notes

• A red shirt appears red because it reflects red

light; the shirt absorbs all of the other colors of

light except the red light. Our eyes see only the

reflected light, making the shirt appear red.

• Frequency: The frequency of light, ν (nu),

is defined as the number of cycles or

crests that pass through a stationary point

in one second.

• Wavelength and frequency are inversely

related—the shorter the wavelength, the

higher the frequency.

Electromagnetic Radiation

(Photons—Particles of Light)

• Light can be viewed as a stream of particles.

• A particle of light is called a photon.

– Photon = packet (bundle) of light energy.

• The amount of energy carried in the packet depends

on the wavelength of the light—the shorter the

wavelength, higher frequency, the greater the

energy.

• Violet light (shorter wavelength) carries more energy

per photon than red light (longer wavelength).

Ch 9.3 Notes

Topic: Electromagnetic Spectrum

EQ: What are the 7 types of radiation?

READ Ch 9.3 (pg. 288-291)



• The entire electromagnetic spectrum, with short-

wavelength, high-frequency radiation on the right and

long-wavelength, low-frequency radiation on the left, is

shown below. Visible light is the small sliver in the middle.

Ch 9.3: The Electromagnetic Spectrum

Draw LEFT side (color)

• The shortest wavelength(λ) and most energetic photons are those of gamma rays.

– produced by the sun, by stars, and by certain unstable atoms on Earth.

– Excessive exposure is dangerous: high energy photons can damage biological molecules.

• X-rays, familiar to us from their medical

and dental uses.

– used to image internal bones and

organs.

– Can damage biological molecules.

– While yearly exposures to X-rays are

relatively harmless, excessive exposure

to X-rays increases cancer risk.

• Ultraviolet or UV light - sunlight that

produces a sunburn or suntan.

• Not as energetic as gamma-ray or X-ray

photons,

• Still can damage biological molecules.

• Excessive exposure to UV increases the

risk of skin cancer, cataracts and causes

premature wrinkling of the skin.

• Visible light, only radiation we can see with eyes.

• ranging from violet (shorter λ, higher E) to red (longer λ, lower E).

• Do not damage biological molecules.

• Do cause molecules in our eyes to rearrange, which sends a signal to our brains that results in vision.

• R O Y G B I V

• Infrared (IR) light - The heat you feel when you place your hand near a hot object is infrared light.

• All warm objects, including human bodies, emit infrared light.

• Can’t see with our eyes, infrared sensors can detect it and are often used in night-vision technology to “see” in the dark.

– warm objects—such as human bodies—glow light a lightbulb glows in the visible region of the spectrum.

In the infrared photograph, the warmest areas

appear as red and the coolest as dark blue.

(Note the cold noses.)

• Microwaves, used for radar and in

microwave ovens.

– Substances that contain water, such as

food, are warmed by the radiation of a

microwave oven, but substances that do

not contain water, such as a plate, are

not.

• The longest wavelengths of light are radio

waves, which are used to transmit the

signals used by AM and FM radio, cellular

telephones, television, and other forms of

communication.

Practice #1

• Arrange the three types of electromagnetic

radiation—visible light, X-rays, and

microwaves—in order of increasing:

(a) Wavelength

(b) Frequency

(c) Energy per photon

Write LEFT side

Chemistry and

Health Radiation

Treatment for

Cancer

• In radiation therapy, doctors aim

X-ray or gamma-ray beams at

cancerous tumors.

• The ionizing radiation damages

the molecules within the tumor’s

cells that carry genetic information,

and the cell dies or stops dividing.

• Healthy cells often sustain damage

during treatments, resulting in side

effects such as fatigue, skin

lesions, and hair loss.

• Doctors try to minimize the

exposure of healthy cells by

appropriate shielding and by

targeting the tumor from multiple

directions, minimizing the

exposure of healthy cells.

Ch 9.4-9.5 Notes

Topic: Atoms with Orbitals

EQ: How do electrons orbit around

the nucleus?

READ Ch 9.4-9.5 (pg. 291-295)



• Ne atoms inside a

glass tube absorb

electrical energy

and then reemit

the energy as red

light.

• Light emitted from

a Hg lamp (left) and

light emitted from a

H lamp (right).

Emission Spectra of the Elements Are Not Continuous

A white-light spectrum is continuous, with some

radiation emitted at every wavelength.

The emission spectrum of an individual element

includes only certain specific wavelengths.

Niels Bohr Developed a Simple Model to Explain

These Results

Draw with notes

The energy of each Bohr

orbit, specified by a

quantum number n = 1, 2, 3

is fixed, or quantized.

Bohr orbits are like steps of

a ladder, each at a specific

distance from the nucleus

and each at a specific

energy.

The Energy Is Quantized Draw with notes

Excitation and Emission

(Lab next week)

• When a hydrogen

atom absorbs

energy, an electron

is excited to a

higher-energy

orbit. The electron

then relaxes back

to a lower-energy

orbit, emitting a

photon of light.

Draw with notes

Hydrogen Emission Lines

The Bohr Model: Atoms with Orbits

• Bohr model - predicted the lines of the

hydrogen emission spectrum.

• However, it failed to predict the emission

spectra of other elements that contained

more than one electron.

• Bohr model was replaced with the

quantum-mechanical or wave-mechanical

model.

• In the quantum-mechanical model,

Bohr orbits are replaced with quantum-

mechanical orbitals.

• Orbitals are different from orbits - they

represent probability maps that show a

where the electron is likely to be found.

Baseball Paths and Electron Probability Maps

(Read only)

• Baseball vs an

electron.

• Imagine a baseball

thrown from the

pitcher’s mound to a

catcher at home plate.

• The baseball’s path

can easily be traced as

it travels from the

pitcher to the catcher.

Baseball Paths and Electron Probability

Maps (Read only)

• To describe the

behavior of a

“pitched” electron,

you would have to

construct a

probability map of

where it would

cross home plate.

• We cannot describe their exact paths.

– Best probability of where the electron is

likely to be found (90% of the time)

The Quantum-Mechanical Model: Atoms with

Orbitals

Ch 9.5 Quantum Mechanics • Electrons do not behave like particles

flying through space.

• Orbital (“electron cloud”)

– Region in space where there is 90%

probability of finding an electron

Courtesy Christy Johannesson www.nisd.net/communicationsarts/pages/chem

Orbital

90% probability of

finding the electron The greater dot density near

the middle represents a

higher probability of finding

the electron near the

nucleus. Draw with notes

Electron capacities

Copyright © 2006 Pearson Benjamin Cummings. All rights reserved.

Electron capacities

Principal Quantum Numbers for Orbitals

• The lowest-energy orbital 1s orbital.

• Number = 1 and the letter = s (shape of

orbital).

• The number is called the principal

quantum number (n) and specifies the

principal shell of the orbital.

• n can range from n=1….7 (why? Because

there are 7 periods)

Ground States and Excited States

• ground state - lowest energy state

• When the e- is in a higher-energy orbital,

the hydrogen atom is said to be in an

excited state.

Energy Increases with Principal

Quantum Number • The higher the principal

quantum number (n), the

higher the energy (E) of the

orbital. (direct relationship)

• The possible principal

quantum numbers are

n = 1, 2, 3, etc… to 7

• Since the 1s orbital has the

lowest possible n , it is in

the lowest-energy shell and

has the lowest possible E.

Draw with notes

Ch 9.6 Notes (Part 1)



the nucleus?

1s22s22p63s23p64s23d104p65s24d104p65s24d105p66s24f145d106p6…

READ Ch 9.6 (pg. 295-301)



Shapes of Orbitals

• The letter indicates the subshell of the

orbital and specifies its shape.

• The possible letters are s, p, d, and f, each

with a different shape.

• Orbitals can be drawn as geometric

shapes

The 2s Orbital Is Similar to the 1s Orbital, but

Larger in Size

The s Orbitals: called spheres

There are one s orbitals Draw with notes

The p Orbitals: called dumbbells

There are three p orbitals

Draw with notes

The d Orbitals: called clovers

There are five d orbitals Draw with notes

The Number of Subshells in a Given

Principal Shell = Equal to the n

Draw LEFT side

General Rules

• Pauli Exclusion Principle

– Each orbital can hold TWO electrons with

opposite spins.


Wolfgang Pauli

Orbital diagram (box)

Electron spins =

arrows in

opposite

direction

Draw with notes

General Rules

Aufbau Principle

– Electrons fill the

lowest energy

orbitals first.


2s

3s

4s

5s

6s

7s

1s

2p

3p

4p

5p

6p

3d

4d

5d

6d

4f

5f

1s

2s

2p

3s

3p

4s

4p

3d

4d 5s

5p

6s

7s

6p

6d

4f

5f

5d

En

erg

y

Don’t Draw

RIGHT WRONG

General Rules

• Hund’s Rule

– Within a sublevel, place one electron

per orbital before pairing them.

– “Empty Bus Seat Rule”


Draw with notes

Electron Filling in Periodic Table

1

2

3

4

5

6

7

s

d

p

s

f

1

2

3

4

5

6

7

s

d

p

s

f

*

W

W

*


Li

2s1

H

1s1

He

1s2

C

2p2

N

2p3

O

2p4

F

2p5

Ne

2p6

Na

3s1

B

2p1

Be

2s2

H

1s1

Al

3p1

Si

3p2

P

3p3

S

3p4

Cl

3p5

Ar

3p6

K

4s1

Ca

4s2

Sc

3d1

Ti

3d2

V

3d3

Cr

3d5

Mn

3d5

Fe

3d6

Co

3d7

Ni

3d8

Cu

3d10

Zn

3d10

Ga

4p1

Ge

4p2

As

4p3

Se

4p4

Br

4p5

Kr

4p6

Rb

5s1

Sr

5s2

Y

4d1

Zr

4d2

Nb

4d4

Mo

4d5

Tc

4d6

Ru

4d7

Rh

4d8

Pd

4d10

Ag

4d10

Cd

4p1

In

5p1

Sn

5p2

Sb

5p3

Te

5p4

I

5p5

Xe

5p6

Cs

6s1

Ba

6s2

Hf

5d2

Ta

5d3

W

5d4

Re

5d5

Os

5d6

Ir

5d7

Pt

5d9

Au

5d10

Hg

5d10

Tl

6p1

Pb

6p2

Bi

6p3

Po

6p4

At

6p5

Rn

6p6

Fr

7s1

Ra

7s2

Rf

6d2

Db

6d3

Sg

6d4

Bh

6d5

Hs

6d6

Mt

6d7

Mg

3s2

Ce

4f2

Pr

4f3

Nd

4f4

Pm

4f5

Sm

4f6

Eu

4f7

Gd

4f7

Tb

4f9

Dy

4f10

Ho

4f11

Er

4f12

Tm

4f13

Yb

4f14

Lu

4f114

Th

6d2

Pa

5f2

U

5f3

Np

5f4

Pu

5f6

Am

5f7

Cm

5f7

Bk

5f8

Cf

5f10

Es

5f11

Fm

5f14

Md

5f13

No

5f14

Lr

5f14

La

5d1

Ac

6d1

1

2

3

4

5

6

7

s

d

p

s

f

*

W

W

*

s2 s1 Elements in the s - blocks

He

s2

Label the top of the groups on your PT

1s1

1s22s1

1s22s22p63s1

1s22s22p63s23p64s1

1s22s22p63s23p64s23d104p65s1

1s22s22p63s23p64s23d104p65s24d10

5p66s1

1s22s22p63s23p64s23d104p65s24d105p66s24f145d106p67s1

H 1

Li 3

Na

11

K

19

Rb

37

Cs

55

Fr

87

Do you notice any similarity in these

configurations of the alkali metals?

The P-block p1 p2 p3 p4 p5 p6


He

2

Ne

10

Ar

18

Kr

36

Xe

54

Rn

86

1s2

1s22s22p6

1s22s22p63s23p6

1s22s22p63s23p64s23d104p6

1s22s22p63s23p64s23d104p65s24d105p6

1s22s22p63s23p64s23d104p65s24d10

5p66s24f145d106p6

Do you notice any similarity in the

configurations of the noble gases?

Transition Metals - d block

d1 d2 d3 s1

d5 d5 d6 d7 d8 s1

d10 d10

Note the change in configuration.


F - block

• Called the “inner transition elements”

f1 f5 f2 f3 f4

f6 f7 f8 f9 f10 f11 f12 f14

f13


Maximum Number of Electrons In Each Sublevel Maximum Number of Electrons

In Each Sublevel

Maximum Number

Sublevel Number of Orbitals of Electrons

s 1 2

p 3 6

d 5 10

f 7 14

LeMay Jr, Beall, Robblee, Brower, Chemistry Connections to Our Changing World , 1996, page 146

Draw LEFT side

Principal Quantum Number ( n )

– Energy level

– Size of the orbital

– PERIOD # (except

Transition/Inner Tran’s

Metals)


1s

2s

3s

Draw with notes

Electron Configurations:

How Electrons Occupy Orbitals

• An electron configuration (e.c.) shows the

location of every orbital, # of e- in each orbital for

a particular atom.

• The e.c. formula is the following:

nL#

PQ# = period # Orbital

shape =

s, p, d, f

Valence e- =

outer most

electrons

s-block 1st Period

1s1 # of valence

electrons

1

2

3

4

5

6

7

Periodic Patterns

• Example - Hydrogen


Electron Configurations: Orbital Diagrams

• The orbital diagram for a ground-state hydrogen

atom is as follows:

• The box represents the 1s orbital, and the arrow

within the box represents the electron in the 1s

orbital.

Let’s Practice

• The following slides we will do in

class!!

• Don’t write them in notes yet

• Get out PT

• List the first 20 elements (symbols)

• Leave space between each element.

1s

2s

3s

4s

2p

3p

4p

3d

4d

s

p

d

f

1

2

3

4

5

6

7

OK, so we’re going to use arrows pointing up or down to

represent the electrons. Can you guess into which box the first

electron would go given that it is attracted to the nucleus?

1 2

1 2 3 4 5 6 7 8 9 10

1 2 3 4 5 6 7 8 9 10 11 12 13 14

1 2 3 4 5 6

5s

+

1s

2s

3s

4s

2p

3p

4p

3d

4d

s

p

d

f

1s1

1

2

3

4

5

6

7

That’s right: it goes in the 1s sublevel. And its el. config is 1s2.

Notice in the table above where H is – in the area designated

as 1s. So where does the next electron go?

1 2

1 2 3 4 5 6 7 8 9 10

1 2 3 4 5 6 7 8 9 10 11 12 13 14

1 2 3 4 5 6

5s

+

1s

2s

3s

4s

2p

3p

4p

3d

4d

s

p

d

f

1s2

1

2

3

4

5

6

7

1 2

1 2 3 4 5 6 7 8 9 10

1 2 3 4 5 6 7 8 9 10 11 12 13 14

1 2 3 4 5 6

5s

If you were thinking it went in the 2s, then you forgot that each

orbital can hold up to two electrons. Note how He is right here

in the area designated as 1s2 and so its el. config. is 1s2. +

1s

2s

3s

4s

2p

3p

4p

3d

4d

s

p

d

f

1s2 2s1

1

2

3

4

5

6

7

1 2

1 2 3 4 5 6 7 8 9 10

1 2 3 4 5 6 7 8 9 10 11 12 13 14

1 2 3 4 5 6

5s

Now that the 1s is filled, the next electron goes in the

next sublevel – the 2s. Again note how Li is in 2s1.

Its full el. conf. is 1s2 2s1. What is Be’s el. conf? +

Energy Level Diagram A

rbitra

ry E

nerg

y S

cale

1s

2s 2p

3s 3p

4s 4p 3d

5s 5p 4d

6s 6p 5d 4f

NUCLEUS

Bohr Model

Electron Configuration

CLICK ON ELEMENT TO FILL IN CHARTS

N

Li = 1s22s1

Lithium

H He Li C N Al Ar F Fe La

1s

2s

3s

4s

2p

3p

4p

3d

4d

s

p

d

f

1s2 2s2

1

2

3

4

5

6

7

1 2

1 2 3 4 5 6 7 8 9 10

1 2 3 4 5 6 7 8 9 10 11 12 13 14

1 2 3 4 5 6

5s

Is this what you were thinking? Good. Now look at the

periodic table above, what comes after the 2s sublevel?

The 2p sublevel. So what will the next el. conf. be? +

1s

2s

3s

4s

2p

3p

4p

3d

4d

s

p

d

f

1s2 2s2 2p1

1

2

3

4

5

6

7

1 2

1 2 3 4 5 6 7 8 9 10

1 2 3 4 5 6 7 8 9 10 11 12 13 14

1 2 3 4 5 6

5s

Is this what you were thinking? Notice how B is

in the 2p1 spot.

So its full el. conf. is 1s2 2s2 2p1. What’s next? +

1s

2s

3s

4s

2p

3p

4p

3d

4d

s

p

d

f

1s2 2s2 2p2

1

2

3

4

5

6

7

1 2

1 2 3 4 5 6 7 8 9 10

1 2 3 4 5 6 7 8 9 10 11 12 13 14

1 2 3 4 5 6

5s

Is this what you were thinking? Notice how C is

in the 2p2 spot. So its el. conf. is 1s2 2s2 2p2

Notice also how when we fill a sublevel… +

1s

2s

3s

4s

2p

3p

4p

3d

4d

s

p

d

f

1s2 2s2 2p3

1

2

3

4

5

6

7

1 2

1 2 3 4 5 6 7 8 9 10

1 2 3 4 5 6 7 8 9 10 11 12 13 14

1 2 3 4 5 6

5s

…we put one electron in each orbital until the

sublevel is half filled…

+

1s

2s

3s

4s

2p

3p

4p

3d

4d

s

p

d

f

1s2 2s2 2p4

1

2

3

4

5

6

7

1 2

1 2 3 4 5 6 7 8 9 10

1 2 3 4 5 6 7 8 9 10 11 12 13 14

1 2 3 4 5 6

5s

… and then we go back and start pairing off

This is called “Hund’s Rule, but it also referred to

as the bus seat rule. Can you figure out why? +

1s

2s

3s

4s

2p

3p

4p

3d

4d

s

p

d

f

1s2 2s2 2p5

1

2

3

4

5

6

7

1 2

1 2 3 4 5 6 7 8 9 10

1 2 3 4 5 6 7 8 9 10 11 12 13 14

1 2 3 4 5 6

5s

Look at F. It’s just one electron away from having

filled 2p sublevel…

And it’s just one square away from the end of the 2p block. +

1s

2s

3s

4s

2p

3p

4p

3d

4d

s

p

d

f

1s2 2s2 2p6

1

2

3

4

5

6

7

1 2

1 2 3 4 5 6 7 8 9 10

1 2 3 4 5 6 7 8 9 10 11 12 13 14

1 2 3 4 5 6

5s

And then Ne has a completely filled outer level.

Na is next. Can you guess where the next

electron is going to go? +

1s

2s

3s

4s

2p

3p

4p

3d

4d

s

p

d

f

1s2 2s2 2p6 3s1

1

2

3

4

5

6

7

1 2

1 2 3 4 5 6 7 8 9 10

1 2 3 4 5 6 7 8 9 10 11 12 13 14

1 2 3 4 5 6

5s

That’s right: in the 3s sublevel. Right now,

write down in your notebook what you

think the next three el configs will be. +

1s

2s

3s

4s

2p

3p

4p

3d

4d

s

p

d

f

1s2 2s2 2p6 3s2

1

2

3

4

5

6

7

1 2

1 2 3 4 5 6 7 8 9 10

1 2 3 4 5 6 7 8 9 10 11 12 13 14

1 2 3 4 5 6

5s

Did you get this one right?

+

1s

2s

3s

4s

2p

3p

4p

3d

4d

s

p

d

f

1s2 2s2 2p6 3s2 3p1

1

2

3

4

5

6

7

1 2

1 2 3 4 5 6 7 8 9 10

1 2 3 4 5 6 7 8 9 10 11 12 13 14

1 2 3 4 5 6

5s

How about Al’s? See how Al is

in the 3p1 spot on the per table

and its el config ends with 3p1 +

Energy Level Diagram A

rbitra

ry E

nerg

y S

cale

1s

2s 2p

3s 3p

4s 4p 3d

5s 5p 4d

6s 6p 5d 4f

NUCLEUS

Bohr Model

Electron Configuration

CLICK ON ELEMENT TO FILL IN CHARTS

N

Al = 1s22s22p63s23p1

Aluminum

H He Li C N Al Ar F Fe La

1s

2s

3s

4s

2p

3p

4p

3d

4d

s

p

d

f

1s2 2s2 2p6 3s2 3p2

1

2

3

4

5

6

7

1 2

1 2 3 4 5 6 7 8 9 10

1 2 3 4 5 6 7 8 9 10 11 12 13 14

1 2 3 4 5 6

5s

Now just advance through the

next 23 slides, but as you do,

make sure you are understanding +

1s

2s

3s

4s

2p

3p

4p

3d

4d

s

p

d

f

1s2 2s2 2p6 3s2 3p3

1

2

3

4

5

6

7

1 2

1 2 3 4 5 6 7 8 9 10

1 2 3 4 5 6 7 8 9 10 11 12 13 14

1 2 3 4 5 6

5s

Exactly what is going on… how

the el configs simply follow the

sequence of the periodic table. +

1s

2s

3s

4s

2p

3p

4p

3d

4d

s

p

d

f

1s2 2s2 2p6 3s2 3p4

1

2

3

4

5

6

7

1 2

1 2 3 4 5 6 7 8 9 10

1 2 3 4 5 6 7 8 9 10 11 12 13 14

1 2 3 4 5 6

5s

Your goal by the end of this slide

show is to be able to write el

configs for any element using just

the periodic table – and your brain! +

1s

2s

3s

4s

2p

3p

4p

3d

4d

s

p

d

f

1s2 2s2 2p6 3s2 3p5

1

2

3

4

5

6

7

1 2

1 2 3 4 5 6 7 8 9 10

1 2 3 4 5 6 7 8 9 10 11 12 13 14

1 2 3 4 5 6

5s

+

1s

2s

3s

4s

2p

3p

4p

3d

4d

s

p

d

f

1s2 2s2 2p6 3s2 3p6

1

2

3

4

5

6

7

1 2

1 2 3 4 5 6 7 8 9 10

1 2 3 4 5 6 7 8 9 10 11 12 13 14

1 2 3 4 5 6

5s

+

1s

2s

3s

4s

2p

3p

4p

3d

4d

s

p

d

f

1s2 2s2 2p6 3s2 3p6 4s1

1

2

3

4

5

6

7

1 2

1 2 3 4 5 6 7 8 9 10

1 2 3 4 5 6 7 8 9 10 11 12 13 14

1 2 3 4 5 6

5s

+

1s

2s

3s

4s

2p

3p

4p

3d

4d

s

p

d

f

1s2 2s2 2p6 3s2 3p6 4s2

1

2

3

4

5

6

7

1 2

1 2 3 4 5 6 7 8 9 10

1 2 3 4 5 6 7 8 9 10 11 12 13 14

1 2 3 4 5 6

5s

+

1s

2s

3s

4s

2p

3p

4p

3d

4d

s

p

d

f

1s2 2s2 2p6 3s2 3p6 4s2 3d1

1

2

3

4

5

6

7

1 2

1 2 3 4 5 6 7 8 9 10

1 2 3 4 5 6 7 8 9 10 11 12 13 14

1 2 3 4 5 6

5s

+

1s

2s

3s

4s

2p

3p

4p

3d

4d

s

p

d

f

1s2 2s2 2p6 3s2 3p6 4s2 3d2

1

2

3

4

5

6

7

1 2

1 2 3 4 5 6 7 8 9 10

1 2 3 4 5 6 7 8 9 10 11 12 13 14

1 2 3 4 5 6

5s

+

1s

2s

3s

4s

2p

3p

4p

3d

4d

s

p

d

f

1s2 2s2 2p6 3s2 3p6 4s2 3d3

1

2

3

4

5

6

7

1 2

1 2 3 4 5 6 7 8 9 10

1 2 3 4 5 6 7 8 9 10 11 12 13 14

1 2 3 4 5 6

5s

+

1s

2s

3s

4s

2p

3p

4p

3d

4d

s

p

d

f

1s2 2s2 2p6 3s2 3p6 4s1 3d5

1

2

3

4

5

6

7

1 2

1 2 3 4 5 6 7 8 9 10

1 2 3 4 5 6 7 8 9 10 11 12 13 14

1 2 3 4 5 6

5s

+

1s

2s

3s

4s

2p

3p

4p

3d

4d

s

p

d

f

1s2 2s2 2p6 3s2 3p6 4s2 3d5

1

2

3

4

5

6

7

1 2

1 2 3 4 5 6 7 8 9 10

1 2 3 4 5 6 7 8 9 10 11 12 13 14

1 2 3 4 5 6

5s

+

1s

2s

3s

4s

2p

3p

4p

3d

4d

s

p

d

f

1s2 2s2 2p6 3s2 3p6 4s2 3d6

1

2

3

4

5

6

7

1 2

1 2 3 4 5 6 7 8 9 10

1 2 3 4 5 6 7 8 9 10 11 12 13 14

1 2 3 4 5 6

5s

+

1s

2s

3s

4s

2p

3p

4p

3d

4d

s

p

d

f

1s2 2s2 2p6 3s2 3p6 4s2 3d7

1

2

3

4

5

6

7

1 2

1 2 3 4 5 6 7 8 9 10

1 2 3 4 5 6 7 8 9 10 11 12 13 14

1 2 3 4 5 6

5s

+

1s

2s

3s

4s

2p

3p

4p

3d

4d

s

p

d

f

1s2 2s2 2p6 3s2 3p6 4s2 3d8

1

2

3

4

5

6

7

1 2

1 2 3 4 5 6 7 8 9 10

1 2 3 4 5 6 7 8 9 10 11 12 13 14

1 2 3 4 5 6

5s

+

1s

2s

3s

4s

2p

3p

4p

3d

4d

s

p

d

f

1s2 2s2 2p6 3s2 3p6 4s1 3d10

1

2

3

4

5

6

7

1 2

1 2 3 4 5 6 7 8 9 10

1 2 3 4 5 6 7 8 9 10 11 12 13 14

1 2 3 4 5 6

5s

+

1s

2s

3s

4s

2p

3p

4p

3d

4d

s

p

d

f

1s2 2s2 2p6 3s2 3p6 4s2 3d10

1

2

3

4

5

6

7

1 2

1 2 3 4 5 6 7 8 9 10

1 2 3 4 5 6 7 8 9 10 11 12 13 14

1 2 3 4 5 6

5s

+

1s

2s

3s

4s

2p

3p

4p

3d

4d

s

p

d

f

1s2 2s2 2p6 3s2 3p6 4s2 3d10 4p1

1

2

3

4

5

6

7

1 2

1 2 3 4 5 6 7 8 9 10

1 2 3 4 5 6 7 8 9 10 11 12 13 14

1 2 3 4 5 6

5s

+

1s

2s

3s

4s

2p

3p

4p

3d

4d

s

p

d

f

1s2 2s2 2p6 3s2 3p6 4s2 3d10 4p2

1

2

3

4

5

6

7

1 2

1 2 3 4 5 6 7 8 9 10

1 2 3 4 5 6 7 8 9 10 11 12 13 14

1 2 3 4 5 6

5s

+

1s

2s

3s

4s

2p

3p

4p

3d

4d

s

p

d

f

1s2 2s2 2p6 3s2 3p6 4s2 3d10 4p3

1

2

3

4

5

6

7

1 2

1 2 3 4 5 6 7 8 9 10

1 2 3 4 5 6 7 8 9 10 11 12 13 14

1 2 3 4 5 6

5s

+

1s

2s

3s

4s

2p

3p

4p

3d

4d

s

p

d

f

1s2 2s2 2p6 3s2 3p6 4s2 3d10 4p4

1

2

3

4

5

6

7

1 2

1 2 3 4 5 6 7 8 9 10

1 2 3 4 5 6 7 8 9 10 11 12 13 14

1 2 3 4 5 6

5s

+

1s

2s

3s

4s

2p

3p

4p

3d

4d

s

p

d

f

1s2 2s2 2p6 3s2 3p6 4s2 3d10 4p5

1

2

3

4

5

6

7

1 2

1 2 3 4 5 6 7 8 9 10

1 2 3 4 5 6 7 8 9 10 11 12 13 14

1 2 3 4 5 6

5s

+

1s

2s

3s

4s

2p

3p

4p

3d

4d

s

p

d

f

1s2 2s2 2p6 3s2 3p6 4s2 3d10 4p6

1

2

3

4

5

6

7

1 2

1 2 3 4 5 6 7 8 9 10

1 2 3 4 5 6 7 8 9 10 11 12 13 14

1 2 3 4 5 6

5s

+

1s

2s

3s

4s

2p

3p

4p

3d

4d 5s

s

p

d

f

1s2 2s2 2p6 3s2 3p6 4s2 3d10 4p6 5s1

1

2

3

4

5

6

7

1 2

1 2 3 4 5 6 7 8 9 10

1 2 3 4 5 6 7 8 9 10 11 12 13 14

1 2 3 4 5 6

+

Ch 9.6 Notes (Part 2)



the nucleus?


READ Ch 9.6 (pg. 295-301)

NO BQ’s

1

2

3

4

5

6

7

Periodic Patterns


Draw LEFT side

Order in which subshells are filled

with electrons

1s

2s

3s

4s

5s

6s

7s

2p

3p

4p

5p

6p

3d

4d

5d

6d

4f

5f

1s 2s 2p 3s 3p 4s 3d 4p 5s 4d … 2 2 6 2 6 2 10 6 2 10

Draw LEFT side


K

4s1

Ca

4s2

Sc

3d1

Ti

3d2

V

3d3

Mn

3d5

Fe

3d6

Co

3d7

Ni

3d8

Cr

3d4

Cu

3d9

Zn

3d10

Ga

4p1

Ge

4p2

As

4p3

Se

4p4

Br

4p5

Kr

4p6

1

2

3

4

s

d

p

s

Cr 4s13d5

Cu 4s13d10

4f

4d

4p

4s

n = 4

3d

3p

3s

n = 3

2p

2s n = 2

1s n = 1

Energ

y

4s 3d

Cr 4s13d5

4s 3d

Cu 4s13d10

Cr

3d5

Cu

3d10

Transition Metals - d block

d1 d2 d3 s1

d5 d5 d6 d7 d8 s1

d10 d10

Note the change in configuration.


Draw LEFT side

A Pattern Exists for the Entire Periodic Table

Ch 9.7 Notes

Topic: Valence Electrons &

Noble Gas e.c.

EQ: What are Val. E- & how do you

write noble gas e.c.?


READ Ch 9.7 (pg. 302-305)



1

2

3

4

5

6

7

Periodic Patterns


Review

Energy Ordering of Orbitals for Multi-

Electron Atoms

• The subshells (s,p,d,f) within a principal

shell (n) do not have the same energy

because of e - interactions.

• Different subshells within the same

principal shell have different energies.

– Increasing Energy:

3s < 3p <3d (more e-)

Core electrons: Inside Electrons closet to nucleus

Valence Electrons: electrons in the _________-_______ energy

level (or shell). (MOST IMPORTANT FOR BONDING!!)

• V.E. = “___” electrons and “___” electrons only.

(V.E. = A Groups only on PT )

Counting Valence Electrons

• MAXIMUM NUMBER OF VALENCE ELECTRONS = 8 e-

(only exception Helium = __ e-’s)

Examples: Ca = __ e-’s Nitrogen = __ e-’s Argon = __ e-’s

• d-block and f-block = _________ valence e-’s

Ch 9.7: Core and Valence Electrons

outer most

s p

2 5 8

2 or 1

2

Electron Configurations and the Periodic Table

The elements within “A” groups (not “B”

groups) of the P.T. all have the same

number of v.e. and similar outer e.c.

With notes - Make a “sketch” with boxes. Label symbols and label “A”

groups

Valence Electrons and Core Electrons

What is e.c. for Si?

Silicon has 4 v.e. (those in the n = 3 principal

shell) and 10 core electrons.

Draw with notes

Valence Electrons and Core Electrons

What is e.c. for Se?

Selenium has 6 v.e. (those in the n = 4 principal shell).

All other electrons, including those in the 3d orbitals, are

core electrons.

Draw with notes

Periodic Trends in Electron Configurations of the

Transition Series Elements

• The transition metals (“B” groups) have

e.c. differ from “A” group elements.

– For the 1st row of trans. metals (in period 4),

they all have the outer configuration of 4s23dx

(x = number of d electrons).

• So, valence e- are always 2 (or

sometimes 1 for two special groups in

the d-block…hint, hint)!!

• Two exceptions groups: Cr is 4s13d5 and

Cu is 4s13d10.

• So, valence e- will be 1!! (only for those

2 groups in d-block)

(2e–) for 4s23dx

(1e–) for 4s13d5 or 4s13d10

Periodic Trends in Electron Configurations of the

Transition Series Elements

neon's e.c. (1s22s22p6)

Noble Gas Configuration

[Ne] 3s1 third energy level

one electron in the s orbital

orbital shape

Na = [1s22s22p6] 3s1 electron configuration

A

B

C

D

Draw with notes

[Ar]

1

2

3

4

5

6

7

4s2 3d10 4p2

Noble Gas Electron Configuration

• Example - Germanium


Ge 72.61

32

• Noble Gas (Shorthand) Configuration

S 16e-

Valence Electrons Core Electrons

S 16e- [Ne] 3s2 3p4

1s2 2s2 2p6 3s2 3p4

Notation

• Longhand Configuration


S 32.066

16

Practice

[Ar] 4s2

Electron configuration Element symbol

[He] 2s2 2p5

[Kr] 5s2 4d10 5p6

V

Sg

Ag

I

[Ar] 4s23d6

Valence e-

LEFT side

Ch 9.8 Notes

Topic: Ions and E.C.

EQ: How does the e.c. change if the

atom loses/gains v.e.?


READ Ch 9.8 (pg. 305-307)

Write Questions & Answer Questions #27


• The chemical properties of elements

are largely determined by the number

of valence electrons they contain.

Ch 9.8 Electron Configuration and Ions

• Alkali metals (Group 1) are

among the most reactive

metals since their outer e.c.

(ns1)

• If they lose the 1 valence e-,

they attain a Noble Gas e.c.

• This is why whole group has

a 1+ charge.

The Alkali Metals Draw with notes

• The alkaline earth

metals (Group 2) all

have e.c. ns2 and have

2 v. e.

• In their reactions, they

tend to lose 2 e -,

forming 2+ ions and

attaining a NG

configuration.

The Alkaline Earth Metals Draw with notes

• The halogens (Group 7) all

have ns2np5 e. c. (short 1

valence e- to noble gas

config)

• Halogens tend to gain 1 e-,

forming 1− ions and

attaining a NG configuration.

The Halogens Draw with notes

• All have 8 v. e. (or 2 for

helium).

• The noble gases are

chemically stable, and are

nonreactive.

The Noble Gases Draw with notes

Elements That Form

Predictable Ions

Ch 9.8 - ELECTRONIC CONFIGURATION OF IONS

• Positive ions (cations) are formed by losing e-.

• Negative ions (anions) are formed by gaining e-.

• Electrons are removed first from the HIGHest occupied orbitals

Practice: (leave 4 lines of space for each)

1. SODIUM

2. CHLORINE

With notes

ELECTRONIC CONFIGURATION OF IONS

Electrons are removed first from the

HIGHest occupied orbitals (be careful

transition metals!!)

Practice: (leave 4 lines of space for each)

1. TITANIUM

2. Germanium

With notes

Ch 9.9 Notes

Topic: Periodic Trends

EQ: What are the 3 trends on the PT?

READ Ch 9.9 (pg. 307-312)

Write Questions & Answer Questions #28


Periodic Trends #1: Atomic Size

• #1: As you move to the right across a period in

the PT, atomic size decreases.

– atomic size determined by the distance

between the outermost electrons and the

nucleus.

– # of protons in the nucleus is increasing,

which results in a greater pull on the e- from

the nucleus, causing atomic size to decrease.

• #2: As you move down a column in the periodic

table, atomic size increases.

– highest principal quantum number, n,

increases.

– orbital increases with increasing PQ#, the e-

that occupy the outermost orbitals are farther

from the nucleus as you move down a

column.

Periodic Trends #1: Atomic Size

Periodic Properties: Atomic Size

With notes - Make a “sketch” with boxes. Draw Arrows

Periodic Trends #2: Ionization Energy

• Ionization Energy – ability to lose electrons

• Ionization energy increases as you move

to the right across a period and decreases

as you move down a column in the

periodic table.

Periodic Trends #2: Ionization Energy


Periodic Properties #3: Metallic Character

• Metals tend to lose electrons in their chemical

reactions, while nonmetals tend to gain

electrons.

• Metallic character decreases as you move to

the right across a period and increases as you

move down a column in the periodic table.

Periodic Properties: Metallic Character


TN Ch 9.1 Date - Chemistry...Ch 9.6 Notes (Part 1) Topic: Atoms with Orbitals EQ: How do electrons...

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Transcript of TN Ch 9.1 Date - Chemistry...Ch 9.6 Notes (Part 1) Topic: Atoms with Orbitals EQ: How do electrons...