Periodic Table Study Guide
Periodic Table
Organized by elements’ atomic numbers so that those with similar
properties line up in the same columns.
Period – horizontal row – tells the energy level electrons live in.
Group – vertical column – matches number of valence electrons.
Metal – left side of table – malleable, ductile, shiny, conduct electricity and
heat, lose electrons to become + charge when reacting and bonding.
Non-metals – right side of table – brittle, do not conduct electricity/heat –
gain electrons to become – charge when reacting and bonding.
Groups or Blocks of Elements to know:
Alkali Metals
Alkaline Earth Metals
Lanthanide Series
Actinide Series
Carbon Group
Nitrogen Group
Halogens
Noble Gases
Trends:
1. Atomic Radius (size of atoms)
2. Density
3.
4.
5.
6.
7.
8.
9.
Transition Metals
Boron Group
Oxygen Group
Smaller
Ionic Radius
Bigger
If the atom gains electrons (nonmetals), the radius gets bigger.
If the atom loses electrons (metals) the radius gets smaller.
Ionization Energy – energy required to pull an electron from an atom.
Electronegativity – the desire an atom has for an electron
Metals are generous! They like to give away electrons so they
have low EN and IE.
Non-metals are greedy! They want more electrons and have high
EN and IE.
Bigger
Smaller
Valence – same as Roman Numeral Group Number (# of bonding
electrons!)
Oxidation Number - +1, +2, +3, +4, -3, -2, -1, 0
Know all s, p, d, and f blocks
Overall Activity or “Reactivity” - desire to react
Metals
Nonmetals
F
more
more
Active
active
Fr
Practice:
1.How many valence electrons do the following elements have?
a. Rn-8 b. Ra-2 c. Xe-8 d. K-1 e. Hg-2 f. As-5
2.Write the electron dot structures for the following elements. Write the
symbol with the indicated number of dots.
a. Cs-1 b. I-7 c. Sn-4 d. Po-6 e. Ca-2 f. Zn-2
3.Name an element for each of the following:
a. a halogen-F,Cl,Br, I, At
b. a member of Group 15- N, P, As, Sb, Bi
g. a lanthanide metal- La, Ce, Pr, Nd, Pm, Sm, Eu, Gd, Tb, Dy, Ho, Er,
c. an element that has 3 valence electrons- B, Al, Ga, In, Tl
h. 3 transition metals- Sc, Ti, V etc.
d. a noble gas-He, Ne, Ar, Kr, Xe, Rn
i. 2 metalloids- B, Si, Ge, As, Sb, Te, Po
e. an alkali metal- Anything in group 1
j. a chalcogen
f. an alkaline earth metal- Anything in group 2 k. a transition
metal- Anything in the d-block
4.Name an element for each of the following:
a. the element in Group 2 and Period 5-Sr
b. The element in Group 18 and Period 4- Kr
c. an element with a -3 oxidation number- Anything in group 15
d. an element with a +2 oxidation number- Anything in group 2
e. an element with a +1 oxidation number- Anything in group 1
f. the element whose e- config. ends with 5p1 – In
g. the element whose e- config. ends with 7s2 -Ra
h. the elements whose e- config. ends with 4d4 -Mo
i. the element whose e- config. ends with 3d1 -Sc
j. the element whose e- config. ends with 5d8 -Pt
k. an element that has the valence of 4s2 4p4 -Se
l. an element that has a valence of 2s2 2p1 -B
5.Within each of the following groups, state which is the larger:
a. Li and Be
b. F and Ne
c. Au and Ag
d. Br and I and Cl
6.Within each of the following groups, state which has the largest ionization
energy:
a. Li and Be
b. F and Ne
c. C and O
d. B and Al
e. K and Na
f. N and Na
7.Within each of the following groups, state which has the greatest
electronegativity:
a. Li and Be
b. F and Fr
c. F and Ne
d. C and O
e. Xe and I
f. Cs and K
8.Identify the following:
a. [Kr] 5s2 4d3- Nb
b. [Ne] 3s2 3p5-Cl
9.Write Noble Gas configurations for:
Mn: [Ar] 4s2 3d5
Te:[Kr] 5s2 4d10 5p4
Ra: [Rn] 7s2
[Xe] 6s1-Cs
10.Rank the following from smallet to the largest (within each set)):
a. Mg, Al, Ba
b. Br, Ar, I, Ne
c. Si, P, S, O
Al, Mg, Ba
Ne, Ar, Br, I
O, S, P, Si
ELECTRON STRUCTURE REVIEW
A. WAVES
Waves move energy from one place to another. A list of the different type of
waves is the Electromagnetic Spectrum. Here is the list from low energy to
high.
Radio Micro Infrared Visible
Ultra Violet
X-ray Gamma
Visible light can be broken into the 7 colors of the rainbow. ROYGBIV. Red
is lowest energy and Violet is highest.
C. ELECTRON CONFIGURATION - address of each electron in the
atom
Each wave has the characteristics:
Wavelength - complete crest and complete trough ( )
Frequency - # waves that pass per second. measured in Hertz ( )
Electrons live in atom houses called orbitals. Orbitals have a distinct size
shape and orientation. These can be represented in three ways: Electron
Configuration (1s2 2s2 etc), Orbital Notation (lines with arrows) and Lewis
Dot Structures (dots for valence e )
To locate electrons in an atom look at the Quantum Numbers.
- . Principle Quantum Number (n) - energy level denotes the size of the
orbital or closeness to nucleus. There are 7 in an atom.
1 is the closest to nucleus, smallest and lowest energy
7 is the farthest biggest, and highest energy
** (Honors) These two properties can be interrelated with the equation c =
Where c is the speed of light: 3.0 x108 m/sec
** (Honors) Frequency and energy can be related by the formula: E = hv
where h is Planck’s constant 6.63 x10-34
B. BOHR Model;
Excited Electrons become excited when exposed to a form of energy. They
are very unhappy when excited and desperately want to go back to their
original orbital. Upon their return they emit or release energy in the form on
light. The light seen corresponds to specific jumps between energy levels.
The Bohr model and diagram shows the light given off in Hydrogen only.
- Orbital Quantum Number ( l) - sublevel refers to the shape of the
orbital - s,p,d,f
s - sphere
p - peanut
d - daisy
f - most complex
- . Magnetic Quantum Number (m) - tells how many orientations or how
many orbital of each shape exist on each energy level.
s - 1 on every level
p - 3 starting on 2nd energy level
d5 starting on 3rd energy level f - 7 starting on 4th
This means that on the 2nd energy level there are three “p” shaped orbitals.
Also on the 5th energy level there are another three “p” shaped orbitals.
3. In a hydrogen atom rank the following jumps of an excited electron
form highest energy photon released to lowest energy photon released.
A. 3rd energy level to 1st energy level
B. 6th energy level to the 3rd energy
- . Spin Quantum Number (s) - there can be two electrons in each orbital.
They spin in different directions.
s can hold 2 electrons
p can hold 6 electrons
d can hold 10 electrons
f can hold 14 electrons
C. 2nd energy level to the 1st energy level
D. Principles:
According to the Aufbau principle , electrons always fill in orbitals of
lowest energy first! Follow diagonal rule to determine lower energy
orbitals. If the electrons do fill the lowest energy orbitals they are in the
ground state.
- Hund stated that orbitals of the same size and same shape will be filled in
individually first before pairing up. For example, when you do orbital
notation diagrams and are filling electrons in the three 2 p orbitals , give each
one 1 electron first before pairing them up. “Bachelor Pad before
roommates”
E. LEWIS DOT STRUCTURES:
Represent the valence electrons. Valence electrons are the electrons in the
largest energy level. They are the electrons that are involved in reaction.
You will never have more than 8 valance electrons or 8 dots.
level
D. 4th energy level to the
2nd energy level A, C, D, B
2. How many energy levels exist in an atom? 7
3. How many sublevel exist in an atom? 4
4. For the “f” sublevel, how many orbitals exist? 7
5. For the “d” sublevel, how many orbitals exist? 5
6. How many electrons can live in the “s” sublevel? 1
7. How many electrons can live in the “p” sublevel? 3
8. Determine how many electrons total can live on the 3rd energy
level.18
9. Determine how many electrons total can live on the 4th energy
level.32
10. Determine the higher energy orbital in each of the following pairs.
A. 3d or 4s
B. 4d or 4f
C. 6d or 7s
D. 5p or 4f
11. Write the orbital notation for Ain’t nobody got time for that.
F. NOBLE GAS NOTATION:
An abbreviated way to write electron configuration. The noble gases are the
last column of the periodic table. Total the number of electrons represented
and determine the element.
Ex [Ne]3s23p4 represents the element sulfur.
A. Fe
B. Br
13. What is the electron configuration for see number 11
A. Sr.
2. Identify which waves move contain more energy.
A. Blue light or red?
B. orange or violet
C. x-ray or yellow
D. infrared or indigo
B. Sc
C. Cl
D. P
14. How many valence electrons do the following have?
A. Cu -2
Study your “cheat sheet”
D. N
12. What is the highest occupied energy in Br? 4p
Practice Problems:
1. Without your notes, construct the electron configuration trends.
C. Al
B. P-5
C. Ar-8
D. Br-7
17. Draw the Lewis dot structure for the elements in # 16.
18. Determine the element represented below
A. 1s22s22p63s23p64s23d1 Sc
D. [Xe]6s1 Cs
B. 1s22s22p1 B C. [Kr]5s24d5 Tc
E. [Xe] 6s24f145d6 Os
Honors ONLY
19. Violet light has a wavelength of 4.10 x 10-12 m. What is the
frequency? 7.32 x 1019 Hz
20. Calculate the energy of a photon of radiation with a wavelength
of 6.4 x 10-7 m. 3,11 x 10-19 J
3. What is the wavelength (in meters) of the electromagnetic
carrier wave transmitted by The Sports Fan radio station at a
frequency of 640 kHz?(Hint: convert kHz into Hz by multiplying by
103.) 470 m
21. What is the energy of light whose wavelength is 4.06 x 10-11 m?
2.69 x 10-44 J
22. What is the wavelength of light with a frequency of 7.66 x 1014
Hz?
3.92 x 10-7 m