Module 1 - Atoms and Moles

Proton

• charge

• relative mass

• location in atom

• +1

• 1

• nucleus

electron

• charge

• relative mass

• location in atom

• -1

• 0

• electron cloud

neutron

• charge

• relative mass

• location in atom

• 0

• 1

• nucleus

isotopes

are elements with their mass number

atomic number

\#protons

mass number

\#protons + #neutrons

average atomic mass

weighted average mass of the atoms in a naturally occurring sample of the element

O-18

• atomic number

• mass number

• protons

• electrons neutrons

• 8

• 18.00

• 8

• 8

• 10

U-235

• atomic number

• mass number

• protons

• electrons neutrons

• 92

• 235

• 92

• 92

• 143

6Li+

• atomic number

• mass number

• protons

• electrons neutrons

• 3

• 6

• 3

• 2

• 3

25Mg2+

• atomic number

• mass number

• protons

• electrons neutrons

• 12

• 25

• 12

• 10

• 13

Which of the following pairs of nuclei are isotopes of the same element?  

a. two nuclei that have the same numbers of protons, but with different masses

b. two nuclei that carry different electric charges, but have the same mass  

c. a nucleus of carbon and a nucleus of nitrogen, both nuclei with the same mass

d. two nuclei with the same numbers of neutrons, but different numbers of protons

 

a

An atom that contains 8 protons, 8 electrons, and 9 neutrons has a mass number of

17

The nucleus of an atom of K-42 contains:

19 protons and 23 neutrons

How many electrons are in a 56Fe2+ ion:

24

Compared to an atom of phosphorus-31, an atom of sulfur-32 contains:

one more proton

\
Which atom has the largest number of neutrons?

a. potassium-39 

b. phosphorus-30

c. chlorine-37

d. argon-40

d

An atom of the most common isotope of gold, Au-197, has _______ protons and ________ electrons.

79,79

Which isotope has 36 electrons in an atom?

a. Bromine-80  

b. Selenium-78

c. Chlorine-34

d. Krypton-80

d

How many neutrons are contained in the nucleus of 27Al3+?

14

60Co2+

• atomic number

• mass number

• protons

• electrons neutrons

• 27

• 60

• 27

• 33

• 25

36Cl-

• atomic number

• mass number

• protons

• electrons neutrons

• 17

• 36

• 17

• 19

• 18

K-39

• atomic number

• mass number

• protons

• electrons neutrons

• 19

• 39

• 19

• 20

• 19

Ni-58

• atomic number

• mass number

• protons

• electrons neutrons

• 28

• 58

• 28

• 30

• 28

find average atomic mass (amu) for

1. Chlorine-35, 75.77% abundance in nature

2. Chlorine-37, 24.23% abundance in nature

35\.4846amu

avogadro’s number (atoms)

6\.022 x 10^23

2\.50 mol F to g

47\.5 g F

32 g O to mol

2\.0 mol O

20 g Ca to mol

0\.50 mol Ca

5\.0 mol O to atoms

3\.0 x 10^24

20\.0 atoms Ti to mol

3\.32 x 10^-23 mol Ti

3\.011 x 10^23 atoms Mg to mol

5\.000 x 10^-1 mol Mg

3\.01 x 10^23 atoms Ne to g

1\.01 x 10^-1 g Ne

48\.0g O to atoms

1\.81 x 10^24 atoms O

10\.0 g Na to atoms

2\.62 x 10^23 atoms Na

How does Sulfur ion differ from a neutral sulfur atom

number of electrons

What is the charge of an ion that has 16 protons and 20 electrons?

\-4

how do isotopes differ

mass number (neutrons)

What is the relationship between wavelength and frequency?

Longer the wavelength, the lower frequency; shorter the wavelength, higher the frequency.

Which visible light color has the longest wavelength?

red

Which visible light color has the highest frequency?

violet

Strength of Bohr Model (1)?

The energy levels

Weaknesses of Bohr Model (2)?

Only used hydrogen and said electrons orbited the nucleus, which is still unsure of.

absorption - increase or decrease? light produced?

increase; no

emission - increase or decrease? light produced?

decrease; yes

When is light produced?

emission - from excited state to ground state

Compared to an atom of hydrogen in the ground state, an atom of hydrogen in the excited state has:

absorbed energy

The light produced by signs using neon gas results from electrons that are:

  

moving from a higher to a lower principal energy level

Principal Quantum Number

• Symbol = n

• n = 1, 2, 3, 4, 5, 6, or 7

• n = 1 is closest to the nucleus

Angular Momentum Quantum Number (shape)

s - sphere

p - dumbbell

d - cloverleaf

f - too complicated to explain shape

number of shapes per energy level

n = 1 1 shape available:   s

n = 2 2 shapes available: s, p

n = 3 3 shapes available: s, p, d

n = 4 4 shapes available: s, p, d, f

n = 5 5 shapes available: s, p, d, f….

n = 6 6 shapes available: s, p, d, f….

n = 7 7 shapes available: s, p, d, f….

**Magnetic Quantum Number (orientation)**

s - number of orientations: 1

p - number of orientations: 3

d - number of orientations:  5

f - number of orientations: 7

each orbital can hold ___

2 electrons

s - number of orbitals: 1 x 2 = 2e-

p - number of orbitals: 3 x 2 = 6e-

d - number of orbitals: 5 x 2 = 10e-

f - number of orbitals: 7 x 2 = 14e-

How to find total number of orbitals?

n^2

how many total orbitals are there in energy level 5

5^2 = 25

how many total orbitals are there in n=4

4^2 = 16 orbitals

How to find number of electrons in energy level?

2n^2

How many electrons can be contained in energy level 5?

(5)2 = 25 x 2 = 50 e-

s → n=

p → n =

d → n=

f → n=

s → n=row

p → n =row

d → n=row minus 1

f → n=row minus 2

electron configuration of Cobalt

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

electron configuration of Aluminum ion (Al3+)

1s2, 2s2, 2p6

electron configuration Cl and Cl-

Cl: 1s2, 2s2, 2p6, 3s2, 3p5

Cl-: 1s2, 2s2, 2p6, 3s2, 3p6

when atom loses electrons, it is

(+) charged

when atom gains electrons, it is

(-) charged

noble gas notation

Shorthand, using Noble Gases to indicate the end of a row.

use the noble gas that is previous to the element

noble gas notation for bromine

\[Ar\] 4s2, 3d10,4p5

noble gas notation for Cl-

\[Ne\] 3s2, 3p6

orbital notation of Mg

Sulfure:

electric configuration

noble gas notation

orbital notation -- how many lone pairs?

• 1s2, 2s2, 2p6, 3s2, 3p4

• [Ne] 3s2, 3p4

• 2 lone pairs

Alkali Metals

• ionic charge

• valence number

• characteristics

• 1+

• 1

• So reactive that they are never found in nature uncombined; must be in compound

Alkaline Earth Metals

• ionic charge

• valence number

• characteristics

• 2+

• 2

• So reactive that they are never found in nature uncombined; must be in compound

transition metals

• ionic charge

• valence number

• characteristics

• 1+ to 4+

• n/a

• Typically metals, less reactive, colorful in compounds

metalloids

the elements on the zig-zag line

have both metal and non-mental properties

halogens

• ionic charge

• valence number

• characteristics

• 1-

• 7

• n/a

noble gases

• ionic charge

• valence number

• characteristics

• 0

• 8

• nonreactive and stable; no electricity

atomic radius

\#1 element

The size of an atom

francium

ionization

\#1 element

The energy required to remove an electron

helium

electronegativity

\#1 element

The measure of an atom's ability to attract shared electrons to itself while in a compound

**Fluorine (F)**

metallic activity

\#1 element

Measures the activity of metals (reactivity)

francium

period period trends

Metal ions → positive

loses e-, smaller atomic radius

non-metals ions → negative

gain e-, bigger than atomic radius

which ion radius bigger than atomic radius

a. Mg

b. Al

c. N

d. O

d

Which of the following elements have a larger atomic radius than ionic radius?

a. Cl

b. Al

c. O

d. S

b

linear

2:0

bent

2:1

2:2

trigonal planar

3:0

Trigonal Pyramidal

3:1

Tetrahedral

4:0

shape of molecule, bond type, and intermolecular force: Ch4

tetrahedral

polar, LDF

shape of molecule, bond type, and intermolecular force: CO2

linear

polar, LDF

shape of molecule, bond type, and intermolecular force: BF3

trigonal planar

polar, LDF

shape of molecule, bond type, and intermolecular force: NCl3

trigonal pyramidal

polar, dipole

ionic bond

m/nm

transfer of electrons

polar covalent

nm/nm

H/nm (H-N, H-O, H-F)

dipole

non-polar covalent

equally sharing electrons

Diatomic

metallic force

result from the electrostatic attraction between metal cations and delocalized electrons

ionic force

Metal ion (cation) attraction to non-metal ion (anion)

3 polar forces

H-bond

dipole (polar)

LDF

Hydrogen bond

H-F, H-O, H-N