Atomic Theory and Perioidicity.notebook
Atomic Theory and the Periodic Table
August 12, 2015
(D)
(A)
(C)
(E)
(B)
"I'm old and a little scary...but I created
the periodic table so WHAT UP NOW?!?!
Sep 8­8:04 AM
Particle
Proton
Neutron
Electron
Mass
Sep 8­8:11 AM
Charge
Symbol
Atomic Number =
Atomic Weight =
Ionic Charge =
Sb
121
Protons
45
Neutrons
58 50
38
Electrons
Mass #
What is an isotope?
Sep 8­8:12 AM
Sep 8­8:12 AM
Mass Spectroscopy
Symbol What element is this?
As 75
3­
How many isotopes does
this element have?
Protons 28 53 Neutrons 31 74 Electrons 26 What is the average atomic
1­ Oxidation # Sep 8­8:12 AM
mass of this element?
What is an isotope?
Sep 3­8:42 AM
1
Atomic Theory and Perioidicity.notebook
August 12, 2015
Determine how many valence electrons
and unpaired electrons for:
unpaired
valence
electrons
electrons
(a) nitrogen
24. Element X is found in two forms: 90.0% is an isotope that has a mass of 20.0, and 10.0% is an isotope that has a mass of 22.0. What is the atomic mass of element X?
(A) 20.0
(B) 20.2
(C) 20.8
(D) 21.2
(E) 21.8
(b) magnesium
(c) chlorine
(d) boron
Sep 8­8:34 AM
Sep 8­8:13 AM
Write the abbreviated electron config for:
Write the abbreviated electron config for:
(a) sodium
(a) Zn2+
(b) sulfur
(b) O2­
(c) iron
(c) What is one element and one ion that O2­
(d) Ag+
is isoelectronic with?
(f) Cl­
Sep 8­8:12 AM
Sep 8­8:12 AM
Sep 8­8:12 AM
Sep 8­8:38 AM
2
Atomic Theory and Perioidicity.notebook
August 12, 2015
Diamagnetic
Paramagnetic
Fe
Cu
Zn
Sep 8­8:32 AM
Colored as
a solution
Cr
Sep 8­8:32 AM
Flame Test Colors
Na+
Li+
K +
Cu2+
Sep 8­8:58 AM
c = λ υ
speed of light = wavelength x frequency
speed of light = 3 x 108 m/s
Sep 12­7:59 AM
Mass Spectroscopy
Photoelectron Spectroscopy
E = h υ
Energy = Planck's constant x frequency
Planck's constant = 6.63 x 10­34 J sec
Sep 12­8:01 AM
Sep 9­7:47 AM
3
Atomic Theory and Perioidicity.notebook
All Periodic Trends can be explained
using three basic principles:
1. Electrons are attracted to the protons in the nucleus. (Zeff = effective nuclear charge)
(a) The closer the electron is to the nucleus, the more strongly it is attracted.
August 12, 2015
All Periodic Trends can be explained
using three basic principles:
2. Electrons are repelled by other electrons.
(a) Valence electrons are shielded by completed shells of electrons.
(b) The more protons in the nucleus, the more strongly the electron is attracted
Sep 13­7:54 AM
All Periodic Trends can be explained
using three basic principles:
3. Completed shells are very stable. Atoms will lose or gain valence electrons to created completed shells if possible.
Sep 13­7:54 AM
Attacking Atomic Theory Statements
#1 Determine what the elements or
compounds have in common.
#2 Determine what the elements or
compounds differ in.
#3 Go to your principles to explain
the difference clearly and concisely.
Sep 13­7:54 AM
Sep 13­8:03 AM
Explain each in terms of principles of atomic
structure
(a) Fluorine has a smaller atomic radius than lithium
Explain each in terms of principles of atomic
structure
(a) Cl­, Ar, and K+ are isoelectronic. Which has the smallest radius and why? Which has the biggest and why?
(b) Rubidium has a larger atomic radius than sodium
Sep 13­8:05 AM
(b) State the trend for atomic radius in going across a period from left to right and why.
Sep 13­8:05 AM
4
Atomic Theory and Perioidicity.notebook
August 12, 2015
Explain each in terms of principles of atomic
structure
(a) Potassium has a lower first ionization energy as compared to lithium.
(b) Sodium has a lower first ionization energy as compared to sulfur.
Sep 13­8:05 AM
Explain each in terms of principles of atomic
structure
(a) O or O2­ . Which is larger and why?
(b) Potassium has a low first ionization energy but a relatively large second ionization energy.
Sep 13­8:05 AM
Explain each in terms of principles of atomic
structure
(a) The difference between the first and second ionization energies of sodium is much larger than the difference between the first and second ionization energies of magnesium. (b) What element could this be. Explain.
1st IE = 540 kJ, 2nd IE = 1000 kJ, 3rd IE = 1700 kJ, 4th IE = 5400 kJ, 5th IE = 5950 kJ
Sep 13­8:05 AM
Sep 16­9:36 AM
Explain each in terms of principles of atomic
structure
(a) Why is the second ionization energy always larger than the first?
(b) Write the chemical reaction showing the first ionization energy of sodium. Sep 13­8:05 AM
Explain each in terms of principles of atomic
structure
(a) Boron has a smaller first ionization energy than beryllium.
(b) Write a chemical reaction for the electron affinity of fluorine.
(c) The electron affinity for chlorine is negative whereas for argon it is positive.
Sep 13­8:05 AM
5
Atomic Theory and Perioidicity.notebook
Explain each in terms of principles of atomic
structure
(a) Cesium is much more reactive in the presence of water as compared to lithium.
(b) The difference between the atomic radii of lithium and sodium is relatively smaller than the difference between the atomic radii of rubidium and cesium.
Sep 13­8:05 AM
August 12, 2015
Explain each in terms of principles of atomic
structure
(a) A sample of solid nickel chloride is attracted into a magnetic field whereas a sample of solid zinc chloride is not.
(b) Phosphorous forms fluorides of PF3 and PF5 whereas nitrogen only forms NF3.
Sep 13­8:05 AM
Answer the following questions about the element selenium, Se (atomic number 34).
(a) Samples of natural selenium contain six stable isotopes. In terms of atomic structure, explain what these isotopes have in common, and how they differ.
(b) Write the complete electron configuration (e.g., 1s2 2s2 … etc.) for a selenium atom in the ground state. Indicate the number of unpaired electrons in the ground­state atom, and explain your reasoning.
(c) In terms of atomic structure, explain why the first ionization energy of selenium is
(i) less than that of bromine (atomic number 35), and
(ii) greater than that of tellurium (atomic number 52).
Sep 17­8:52 AM
Sep 20­11:18 AM
Sep 14­7:58 AM
6
Atomic Theory and Perioidicity.notebook
August 12, 2015
Use only a periodic table, individually write
the following explanations using your theory
of atomic principles
1) Predict which element, Na or K, has a
larger first ionization energy and explain
your choice.
2) Sulfur has a smaller radius than
Phosphorous. Explain this trend.
Sep 19­11:20 AM
Sep 17­8:52 AM
7