Name, Date, Hr/Per_____________________________________________________________________________
MATTER & THE PERIODIC TABLE – UNIT 2 – INSTRUCTIONAL PACKET #1
UNIT 2 Vocabulary: Create notecards or a key-term foldable for Chapter 15 Vocabulary. Due __________________
Lecture 2-1: Properties of Matter
Matter:
- Definition
Properties of Matter:
- Physical Properties
-
Physical Changes
-
Chemical Properties
-
Chemical Changes
o
Signs of a chemical change
Composition of Matter:
Phases of Matter:
Type
of
Volume
Matter
Solid
Shape
Particle Movement
Energy /
Temp.
Other Notes:
Liquid
Gas
Plasma
1
Phase Changes: (warming up)
-
Melting
-
Vaporization
-
Sublimation
Phase Change Diagram:
(Draw and label the diagram below)
Phase Changes: (cooling down)
-
Condensation
-
Freezing
Homework:
Physical vs. Chemical Change w/s
In a physical change, the original substance still exists, it has only changed in form. Energy changes usually do not
accompany physical changes, except in phase changes and when substances dissolve,
In a chemical change, a new substance is produced. Energy changes always accompany chemical changes. Chemical
changes are always accompanied by physical
Classify the following as examples of a physical change [P], a chemical change [C] or both kinds of change [P / C].
1. _________ Sodium hydroxide dissolves in water
6. _________ Iron rusts
2. _________ Hydrochloric acid reacts with sodium
7. _________ Ice melts
hydroxide to produce a salt, water and heat.
8. _________ Acid on limestone produces
3. _________ A pellet of sodium is sliced in two
carbon dioxide gas
4. _________ Water is heated and changed to steam
9. _________ Milk sours
5. _________ Potassium chlorate decomposes to
10. _________ Wood rots
potassium chloride and oxygen gas
States of Matter – Crossword w/s
[crossword follows on next page]
DOWN
1. The three forms of matter (liquid, solid, and gas).
(3 words – not specific; general overall term)
14. In ____, atoms move the fastest.
3. The change in a state of matter from a solid to a liquid.
15. Water changes from a liquid state to a solid-state
at ____ degrees Celsius.
5. The gas state of water. (2 words)
16. The particles in ____ move back and forth in place.
8. Matter in a gas state will ____ out to fill its container
19. The particles in liquids ____ past each other.
9. The change in a state of matter from a gas to a liquid.
20. A solid always take up the same amount of this.
11. If you add heat to matter, the atoms that make up
the matter will begin to move ____.
21. A state of matter that has no fixed shape and no
fixed volume.
2
ACROSS
1. If you subtract heat from matter, the atoms that
make up the matter will begin to move ____.
12. The change in a state of matter from a liquid
to a solid.
2. The temperature at which a given substance will
change from a liquid into a gas. (2 words)
13. The change in a state of matter from a liquid
to a gas.
4. The particles in a solid state move around
___ point.
17. The pull on the surface of liquids that allow
liquids to form drops when they fall. (2 words)
6. The number of states of matter.
18. The basic building blocks of matter.
7. You can change the state of matter by either
adding or subtracting ____.
22. The temperature at which a given substance will
change from a solid into a liquid. (2 words)
10. A state of matter that has no fixed shape but
that has a definite volume.
23. A state of matter that has a definite shape and
a definite volume.
11. Particles in a gas are ____ apart than the
particles in a liquid.
24. Gases ____ to fill whatever space is available
to them.
3
Lecture 2-2: Composition of Matter
Composition:
- Pure Substance
-
Mixture
Pure Substance:
- Elements
-
Compounds
Practice:
Mixture:
- Homogeneous
o
Solvent
Types of Solutions:
- Alloy
-
Amalgam
-
Aqueous Solution
Heterogeneous
o
examples
Solution (aka: Homogeneous Mixture):
- Solute
-
-
Example
-
Soluble
-
Insoluble
-
Concentrated
-
Dilute
-
Temperature
Making a Solution:
- “Surround and Separate”
Speeding up the Solution Process:
- Agitation
-
o
Surface Area
Exception for Gas
Solubility:
- Definition
Saturation of Solute:
- Unsaturated
-
Saturated
o
Supersaturated
-
Solubility Curve (graph)
-
Example
Saturation Point
Heterogeneous Mixture:
- Definition
4
-
Types of Heterogeneous Mixtures:
- Suspensions
-
Colloids
o
Tyndall Effect
Homework:
Substances vs. Mixtures w/s
A substance is matter for which a chemical formula can be written. Elements and compounds are substances.
Mixtures can be in any proportion, and the parts are not chemically bonded.
Classify the following as to whether it is a substance or a mixture by writing “S” or “M” in the space provided.
1. _____ sodium
8. _____ cake batter
15. _____ eggs
2. _____ water
9. _____ air
16. _____ blood
3. _____ soil
10. _____ soup
17. _____ table salt
4. _____ coffee
11. _____ iron
18. _____ nail polish
5. _____ oxygen
12. _____ salt water
19. _____ milk
6. _____ alcohol
13. _____ ice cream
20. _____ cola
7. _____ carbon dioxide
14. _____ nitrogen
Homogeneous vs. Heterogeneous Matter w/s
Classify the following substances and mixtures as either homogeneous [HO] or heterogeneous [HE]
1. ______ flat soda pop
6. ______ aluminum foil
11. ______ alcohol
2. ______ cherry vanilla ice cream
7. ______ black coffee
12. ______ iron
3. ______ salad dressing
8. ______ sugar water
13. ______ beach sand
4. ______ sugar
9. ______ city air
14. ______ pure air
5. ______ soil
10. ______ paint
15. ______ spaghetti sauce
Solutions, Colloids, and Suspensions w/s
Label the following mixtures as a solution, colloid, or suspension. Give an example of each.
1. has large particles which settle out upon standing
a. kind of mixture ________________________________
b. example: _____________________________________
2. has medium sized particles which settle out upon standing; scatters light
a. kind of mixture ________________________________
b. example: _____________________________________
3. has very small particles which do not settle out upon standing
a. kind of mixture ________________________________
b. example: _____________________________________
5
Separation of Mixtures w/s
Taking advantage of various physical and chemical properties, how would you separate the following mixtures into
their components?
1. Sand and water ____________________________________________________________________________
_________________________________________________________________________________________
2. Sugar and water ___________________________________________________________________________
_________________________________________________________________________________________
3. Oil and water _____________________________________________________________________________
_________________________________________________________________________________________
4. Sand and gravel ________________________________________________________ ___________________
_________________________________________________________________________________________
5. A mixture of heptane (boiling point 98°C) and heptanol (boiling point 176°C) __________________________
_________________________________________________________________________________________
6. A mixture of iodine solid and sodium chloride (Hint: Iodine is not soluble in water) _____________________
_________________________________________________________________________________________
7. A mixture of lead and aluminum pellets ________________________________________________________
_________________________________________________________________________________________
8. A mixture of salt and iron filings ______________________________________________________________
_________________________________________________________________________________________
A
Solubility Curves w/s
Answer the following questions based on Solubility graph A
1. Why do the temperatures on the graph only go from 0º
C to 100º C ?
2. Which substance is most soluble at 60º C ?
3. Which two substances have the same solubility at 80º C ?
4.Which substance’s solubility changes the most from 0º C
to 100º C ?
5.Which substance’s solubility changes the least from 0º C
to 100º C ?
6. What is the solubility of potassium nitrate at 90º C ?
6
7. At what temperature does potassium iodide have a
solubility of 150 g/ 100 cm3 water ?
Continue answering the following questions based on Solubility graph A from the previous page.
8. You have a solution of sodium nitrate containing 140 g at 65º C. Is the solution saturated, unsaturated, or
supersaturated ?
9. You have a solution of potassium chlorate containing 4 g at 65º C. How many additional grams of solute must be
added to it, to make the solution saturated ?
10. A solution of potassium iodide at 70º C contains 200 g of dissolved solute in 100 cm3 water. The solution is
allowed to cool. At what new temperature would crystals begin to start forming ?
11. What is the general trend that you see on the graph? Use the IV and DV in your answer.
Answer the following questions based on Solubility graph B
1. At which temperature do KBr and KNO3 have the
same solubility?
2. At which temperature do NaCl and KNO3 have the
same solubility?
3. At which temperature do NaClO3 and KNO3 have the
same solubility?
4. At 60oC, how much KNO3 can 100 g of water hold?
5. At 80oC, how much NaCl can 100 g of water hold?
6. At 0oC, how much KBr can 100 g of water hold?
7. A solution of NaCl contains 50g at 70 º C. Is the
solution saturated, unsaturated, or supersaturated ?
8. A solution of KBr contains 100g at 95 º C. Is the
solution saturated, unsaturated, or supersaturated ?
9. Which compound's solubility changes very little with
temperature?
10. Which compound's solubility changes the most with
temperature?
11. Which compound has the greatest solubility at 60oC?
12. Which compound has the least solubility at 20o C?
7
Element, Compound, Solution, or Heterogeneous Mixture? w/s
Identify each as an element [E], a compound [C], a solution [S], or a heterogeneous mixture [HM].
1. _____ Sand
11. _____ Salad Dressing
20. _____ Calcium Nitrate
2. _____ Salt
12. _____ Salt Water
21. _____ Kool-Aid ®
3. _____ Pure Water
13. _____ Raisin Bran
22. _____ Sugar water
4. _____ Soil
14. _____ Silver
23. _____ Chocolate milk
5. _____ Soda
15. _____ Lithium Carbonate
24. _____ Salt water
6. _____ Pure Air
16. _____ Apple Pie
25. _____ Coffee with milk
7. _____ Carbon Dioxide
17. _____ Iced Tea (with
powder, well mixed)
26. _____ Cup of tea with
tea leaves floating in it
18. _____ Potassium
27. _____ Salt
19. _____ Soda
28. _____ Chocolate chip
cookies
8. _____ Gold
9. _____ Bronze
10. _____ Oxygen
Reading a Phase Diagram w/s
Examine the phase diagram below, then answer the questions which follow.
1. If you were to have a bottle
containing compound X in your
closet, what phase would it most
likely be in?
@ sea level,
pressure =
1 atm
2. What is the triple point of
compound X (At what temperature
and pressure will all three phases
coexist)?
3. If you have a bottle of compound X at a pressure of
3 atm and temperature of 1000 C, then raise the
temperature to 4000 C, what phase transition(s)
would occur?
4. If you have a bottle of compound X at a pressure of
4 atm and temperature of 1000 C, then raise the
temperature to 8000 C, what phase transition(s)
would occur?
5. Why can’t compound X be brought to a boil at
a temperature of 2000 C?
7. At 5000 C and at 2 atm, in what state is the
substance? ________
8. At 4500 C and at 4 atm, in what state is the
6. Is it possible for humans to drink compound X?
Why or why not?
8
substance? ________
9. At 7500 C and 6 atm, in what state is the
substance? ________
Lecture 2-3: Atoms
Atom:
- Definition
-
Composed of
Subatomic Particles:
- Protons
-
Electrons
-
Quarks?
-
Neutrons
Elements:
- Definition
- Atomic Number
- Chemical Symbol
- Atomic Mass
Nucleon
Practice [see graphic above – label the image and write # of subatomic particles]:
Writing Elements:
- Steps
Counting Particles:
- Protons =
-
Neutrons =
-
Electrons =
If electrons differ:
- Ion
If neutrons differ:
- Isotope
-
Example
-
Example
If protons differ:
Allotrope:
- Definition
Electron Dot Models:
Practice drawing
electron dot models:
Homework:
9
Elements to Memorize
List the chemical symbol for each element and memorize them 10 per night. You will be quizzed on them in these
sets of ten – SPELLING COUNTS. After you have been quizzed a few times, you will have a large quiz with 25-30 of
these 45 elements. This large quiz will contain one or more bonus elements
______1.
Hydrogen
______16.
Titanium
______31.
Silicon
______2.
Iodine
______17.
Calcium
______32.
Gold
______3.
Lithium
______18.
Manganese
______33.
Tin
______4.
Helium
______19.
Strontium
______34.
Zinc
______5.
Sodium
______20.
Iron
______35.
Lead
______6.
Neon
______21.
Barium
______36.
Mercury
______7.
Potassium
______22.
Cobalt
______37.
Nitrogen
______8.
Argon
______23.
Radium
______38.
Uranium
______9.
Cesium
______24.
Nickel
______39.
Phosphorous
______10.
Krypton
______25.
Boron
______40.
Plutonium
______11.
Francium
______26.
Platinum
______41.
Oxygen
______12.
Xenon
______27.
Aluminum
______42.
Sulfur
______13.
Beryllium
______28.
Copper
______43.
Fluorine
______14.
Radon
______29.
Carbon
______44.
Chlorine
______15.
Magnesium
______30.
Silver
______45.
Bromine
Elements and their Symbols w/s
Write the symbols for the following elements.
1. ______ oxygen
6. ______ carbon
11. ______ magnesium
16. ______ silver
2. ______ hydrogen
7. ______ helium
12. ______ manganese
17. ______ lead
3. ______ chlorine
8. ______ nitrogen
13. ______ neon
18. ______ iron
4. ______ sodium
9. ______ copper
14. ______ bromine
19. ______ calcium
5. ______ fluorine
10. ______ sulfur
15. ______ phosphorus
20. ______ potassium
Write the name of the element that corresponds to each of the following symbols
21. ____________ Cu
26. ____________ Pb
31. ____________ Ca
36. ____________ Sn
22. ____________ K
27. ____________ Fe
32. ____________ Ag
37. ____________ H
23. ____________ C
28. ____________ Na
33. ____________ P
38. ____________ F
24. ____________ Au
29. ____________ S
34. ____________ O
39. ____________ Ni
25. ____________ Zn
30. ____________ Al
35. ____________ I
40. ____________ Hg
Number of Atoms in a Formula w/s
Determine the number of atoms in the following chemical elements.
1. ______ NaCl
6. ______ Ba(OH)2
11. ______ Cu(NO3)2
16. ______ Fe2O3
2. ______ H2SO4
7. ______ NH4Br
12. ______ KMnO4
17. ______ NaC2H3O2
3. ______ KNO3
8. ______ Ca(PO4)2
13. ______ H2O2
18. ______ Mg(C2H3O2)2
4. ______ CaCl2
9. ______ Al2(SO4)3
14. ______ H3PO4
19. ______ Hg2Cl2
5. ______ C2H6
10. ______ Mg(NO3)2
15. ______(NH4)3PO4
20. ______ K2SO3
Parts of an Atom w/s
An atom is made up of protons and neutrons which are in the
nucleus, and electrons which are in the electron cloud surrounding
the atom.
The atomic number equals the number of protons. The electrons in
a neutral atom equal the number of protons. The mass number
equals the sum of the protons and neutrons.
The charge indicates the number of electrons that have been lost or
gained. A positive charge indicates the number of electrons (which
are negatively charged) lost. A negative charge indicates the
number of electrons gained.
Complete the following chart.
Element / Ion
24
12
39
19
23
11
19
9
27
13
1
1
24
Mg
K
Na+1
F-1
Al+3
H
Mg+2
Ag
S-2
2
1
35
H
Cl-
Atomic
Number
Mass
Number
Charge
# of Protons
# of
Neutrons
# of
Electrons
Be+2
11
Parts of the Atom w/s
Using the Periodic Table of the Elements, determine the number of protons, neutrons, and electrons in each of the
following atoms. Draw a model of the atom showing the electrons in the proper energy levels.
Model:
_____ protons
1
1
H
_____ neutrons
_____ electrons
Model:
_____ protons
12
6
C
_____ neutrons
_____ electrons
Model:
_____ protons
23
11
Na
_____ neutrons
_____ electrons
Model:
_____ protons
21
15
P
_____ neutrons
_____ electrons
Model:
_____ protons
16
8
O
_____ neutrons
_____ electrons
12
Valence Clues w/s
Atomic Structure – Create the appropriate Bohr model.
Use the PT to fill in the info for each element given.
Element: Boron
Number of Valence Electrons: _______
Group Number: _______
Oxidation Number: _______
Period Number: _______
Circle One:
metal, non-metal, metalloid, noble gas, halogen
Element: Silicon
Number of Valence Electrons: _______
Group Number: _______
Oxidation Number: _______
Period Number: _______
Circle One:
metal, non-metal, metalloid, noble gas, halogen
Element: Nitrogen
Number of Valence Electrons: _______
Group Number: _______
Oxidation Number: _______
Period Number: _______
Circle One:
metal, non-metal, metalloid, noble gas, halogen
Element: Carbon
Number of Valence Electrons: _______
Group Number: _______
Oxidation Number: _______
Period Number: _______
Circle One:
metal, non-metal, metalloid, noble gas, halogen
Element: Hydrogen
Number of Valence Electrons: _______
Group Number: _______
Oxidation Number: _______
Period Number: _______
Circle One:
metal, non-metal, metalloid, noble gas, halogen
13
Element: Neon
Number of Valence Electrons: _______
Group Number: _______
Oxidation Number: _______
Period Number: _______
Circle One:
metal, non-metal, metalloid, noble gas, halogen
Element: Fluorine
Number of Valence Electrons: _______
Group Number: _______
Oxidation Number: _______
Period Number: _______
Circle One:
metal, non-metal, metalloid, noble gas, halogen
Element: Oxygen
Number of Valence Electrons: _______
Group Number: _______
Oxidation Number: _______
Period Number: _______
Circle One:
metal, non-metal, metalloid, noble gas, halogen
Element: Calcium
Number of Valence Electrons: _______
Group Number: _______
Oxidation Number: _______
Period Number: _______
Circle One:
metal, non-metal, metalloid, noble gas, halogen
Element: Helium
Number of Valence Electrons: _______
Group Number: _______
Oxidation Number: _______
Period Number: _______
Circle One:
metal, non-metal, metalloid, noble gas, halogen
14
Bohr Model Practice w/s
For each element, write the total number of electrons on the line. Then color the correct number of electrons for
each orbit. Remember, fill the orbit closest to the nucleus first, but never exceed the number each orbit can hold.
This number is _______ for the first shell and _______ for the shells that come afterward.
Check the Periodic Table to find out how many electrons each element actually has.
To indicate the number of protons & neutrons in the nucleus, draw a line extending from the center pointing to your
labels.
15
Now, draw your own Bohr model diagrams for the elements listed below.
Lithium (Li) _________
Sulfur (S) _________
Neon (Ne) _________
Bohr Models w/s
Check the periodic table to find out how many of each type of subatomic particle each element below has.
Small circles in the images will represent possible electron locations. For each element [as modeled in lecture]:
a. write the atomic number on the line provided
c. draw electron clouds with:
b. draw and label the nucleus of the atom
i. blue inner electrons & red valence electrons
Sodium (Na) _________
16
Phosphorous (P) ________
Aluminum (Al) ________
Carbon (C) _______
Silicon (Si) ________
Oxygen (O) ________
Chlorine (Cl) ________
Argon (Ar) ____
Lecture 2-4: Electron Configuration
Background Info:
- Groups
-
Orbitals:
- Lewis Dot
Quantum Numbers:
- First
-
Periods
-
-
Bohr Model
Second
-
Third
Example(s)
Homework:
Electron Configurations - Tutorial
An electron configuration is a method of indicating the arrangement of electrons about a nucleus. A typical electron
configuration consists of numbers, letters, and superscripts with the following format:
1. A number indicates the energy level [“the quantum number”]
2. A letter indicates the type of orbital; s, p, d, f. [we will not use f]
a. “s” orbitals can hold up to 2 electrons
b. “p” orbitals can hold up to 6 electrons
c. “d” orbitals can hold up to 10 electrons
d. Orbitals fill in this order: 1s, 2s, 2p, 3s, 3p, 4s, 3d, 4p, 5s, 4d, 5p…and so on.
i. “d” orbitals are filled after the “s” orbital of the next energy level
1. you can clearly see this on the periodic table!!
ii. You will not be asked for anything further than this on an exam.
3. A superscript indicates the number of electrons in the orbital. Example: ls2 means that there are two electrons
in the “s” orbital of the first energy level. The element is helium.
The periodic table can help us figure out what these configurations are. To the left are the “s” orbitals. The “p”
orbitals are shown on the right, and the “d” orbitals are in the center.
The periodic table has been labeled with the correct period numbers on the far left and on the far right for you. You
already know that the group number helps indicate the number of valence electrons and the charge/oxidation
number; the period number tells you which energy level/shell those electrons belong to. The area of the periodic
table which corresponds to elements in the “d” level [the transition metals] belong to one energy level less than the
period that it is in. This has been noted for you on the chart to the right.
Example: Chlorine – Chlorine is in group 17. Chlorine has 17 electrons [which is totally a coincidence, not related to
group number…]. Chlorine is in period 3. Following the rules of filling electron levels… Chlorine has:
a. 2 electrons in the 1s level [full] = 1s2
d. 2 electrons in the 3s level [full] = 3s2
b. 2 electrons in the 2s level [full] = 2s2
e. 5 electrons in the 3p level [not full] = 3p5
6
c. 6 electrons in the 2p level [full] = 2p
Check it out – it matches the electron configuration!! Trace this across the periodic table left to right. When you get
to the end of a period, go to the next period starting at the right…etc. You cross:
a. 2 elements in the “s” block of the period 1
c. 6 elements in the “p” block of the period 2
b. 2 elements in the “s” block of the period 2
d. 2 elements in the “s” block of period 3
17
e. …and Chlorine is the 5th element in the “p”
block of period 3
Now, you try – write the full electron configuration of the following elements.
Helium______________________________________________________________
Neon______________________________________________________________
Sodium______________________________________________________________
Zinc______________________________________________________________
Sulfur______________________________________________________________
Palladium_____________________________________________________________
Electron Configurations w/s
PART A: Longhand Electron Configuration –
Use the patterns within the periodic table to write longhand electron configurations for the following atoms.
1. Symbol: __Mg__ # of electrons: ______
Long-Hand Electron Configuration:
2. Symbol: __P__ # of electrons: ______
Long-Hand Electron Configuration:
3. Symbol: __V__ # of electrons: ______
Long-Hand Electron Configuration:
4. Symbol: __Ge__ # of electrons: ______
Long-Hand Electron Configuration:
5. Symbol: __Kr__ # of electrons: ______
Long-Hand Electron Configuration:
6. Symbol: __O__ # of electrons: ______
Long-Hand Electron Configuration:
PART B: Shorthand Electron Configurations –
Use the patterns within the periodic table to write longhand electron configurations for the following atoms.
18
7. Symbol: __Ca__ # of electrons: ______
Short-Hand Electron Configuration:
8. Symbol: __Pb__ # of electrons: ______
Short -Hand Electron Configuration:
9. Symbol: __F__ # of electrons: ______ Short -Hand Electron Configuration:
10. Symbol: __O__ # of electrons: ______ Short -Hand Electron Configuration: __________
11. Symbol: __S__ # of electrons: ______
Short -Hand Electron Configuration: __________
12. Symbol: __Al__ # of electrons: ______
Short -Hand Electron Configuration: __________
13. Symbol: __Cs__ # of electrons: ______
Short -Hand Electron Configuration: __________
14. Symbol: __Sb__ # of electrons: ______
Short -Hand Electron Configuration: __________
Valence Electrons & the Periodic Table w/s
Group = vertical columns; begins with H/Li, Be, skips transition metals, continues with B-He/Ne;
Period = horizontal rows [not needed for this w/s]
Using the information above and a periodic table, complete the tables below with the requested information.
Number of…
Chemical Symbol
Chemical Name
Atomic #
e-s _____
Li
nos _____
p+s _____
nos _____
p+s _____
nos _____
p+s _____
nos _____
group # _____ valence e-s _____ oxidation # _____
e-s _____
Ne
p+s _____
group # _____ valence e-s _____ oxidation # _____
e-s _____
F
nos _____
group # _____ valence e-s _____ oxidation # _____
e-s _____
O
p+s _____
group # _____ valence e-s _____ oxidation # _____
e-s _____
N
nos _____
group # _____ valence e-s _____ oxidation # _____
e-s _____
C
p+s _____
group # _____ valence e-s _____ oxidation # _____
e-s _____
B
nos _____
group # _____ valence e-s _____ oxidation # _____
e-s _____
Be
p+s _____
p+s _____
nos _____
group # _____ valence e-s _____ oxidation # _____
What do you notice about:
1. …the number of valence e-s as you go across the periodic table?
2. …the number of valence e-s compared to the group number?
19
Predict how many valence electrons each would have: Ba ______, Br ______, Xe ______, At ______
Electron Configuration Practice w/s
In the space below, write the unabbreviated [long-hand] electron configurations of the following elements:
1. sodium
_________________________________________________________________________________
2. iron __________________________________________________________________________________
3. bromine ______________________________________________________________________________
4. barium
_____________________________________________________________________________
In the space below, write the abbreviated [short-hand] electron configurations of the following elements:
5. cobalt
_______
6. silver
_______
7. tellurium
_______
8. radium
_______
Determine what elements are denoted by the following electron configurations:
9. 1s2 2s2 2p6 3s2 3p4 ____________________
11. 1s2 2s2 2p6 3s2 3p6 4s2 __________________________
10. 1s2 2s2 2p6 3s2 3p6 4s2 3d10 4p6 5s1 _______________ 12. 1s2 2s2 2p6 3s2 3p6 4s2 3d10 4p1 ___________________
Determine which of the following electron configurations are valid, and which are invalid.
13. 1s2 2s2 2p6 3s2 3p6 4s2 4d10 4p5 _______________
15. 1s2 2s2 2p9 3s2 3p6 4s2 ____________________
14. 1s2 2s2 2p6 3s3 3d5 ____________________
16. 1s2 2s2 2p6 3s2 3p4 ____________________
Explain what is wrong with the following electron configurations:
17. 1s2 2s2 2p6 3s2 3p6 4s2 4d10 4p6 ___________________________________________________________________
18. 1s2 2s2 2p6 3s3 3d5 _____________________________________________________________________________
Use the following clues to identify the element. Show any figuring in the space below.
19. This element has a 3p sublevel that contains 3 electrons.
20. This element has a 4s sublevel with 2 electrons for its outermost electrons.
21. This element has 1 electron in its 3d sublevel.
22. This element has 5 electrons in its 5p sublevel
23. This element has a completely filled 3p sublevel for its outermost electrons.
24. This element has 2 electrons in its 6p sublevel.
Lecture 2-5: Periodic Table
Periodic Table:
- Describes…
Properties:
- Chemical Properties
20
-
Consists of
-
Valence Electrons
Charge:
- Octet Rule
-
Cation
-
Anion
Mendeleev’s Contributions:
- First Periodic Table
-
Undiscovered Elements
Periodic Table:
- Columns called -
-
Rows called -
-
Groups
Oxidation #:
- Definition
-
Practice
Group 1:
- Name
-
Characteristics
Group 2:
- Name
-
Characteristics
Groups 3-12:
- Name
-
Characteristics
-
Lanthanides & Actinides
Metals
Non-Metals
Location
Appearance
“Shape-Ability”
Conductivity
Physical State
Charge
Metalloids:
- Properties
-
Location
Group 17:
- Name
-
Characteristics
Group 18:
-
Semi-conductors
21
- Name
Electronegativity:
- High
-
-
Characteristics
Low
Reactivity:
- Definition
-
-
Increases
-
Decreases
Metals
-
Non-Metals
Atomic Radius:
- Properties
Homework:
Color the Trends in the Periodic Table w/s
Color according to trends listed; record colors by coloring in terms provided on table.
Metals Non-Metals Metalloids
Zig-Zag Divider
[red]
[blue]
[purple]
[make line darker]
@ Standard Pressure & Temperature:
Solid Liquid
Gas
[red] [blue] [white]
22
Non-Metals Alkali Metals Alkaline Earth Metals
Metalloids
Halogens
[blue]
[red]
[green]
[purple]
[yellow]
Transition Metals
Noble Gases
Lanthanides
Actinides
[brown]
[white]
[light orange]
[orange]
Draw arrows representing the trend(s) in Electronegativity.
Draw arrows representing the trend(s) in Atomic Radius [size].
23
An Elemental Tale: The Gold Dust Kid w/s
The Kid mounted his trusty steed, old [B] ___________. His shooting [Fe] ____________ strapped to his side, he
headed out for the bright [Ne] ____________ lights of Toronto, aiming to rob the mid-day stage. There was sure to be
a load of precious [U] ______________ aboard, and probably [K] ____________, too. Inhaling a deep breath of
[O] ____________ he coughed on the [S] ____________ from the nearby mills. Since the [Hg] ______________ was
climbing, he quenched his thirst with some H2O, tasting the [Cl] ____________ all big cities like Brockville had. As he
headed north his bones ached from [Ca] _____________deposits built up over the years of riding the [Zn] _________
trail. Overhead a [He] __________-filled balloon floated in the breeze; the sun beat down like burning
[P] _______________. Soon he spotted the stage, guarded only by a sheriff with a [Sn] ____________ badge. "Halt,"
he yelled. "or I'll fill you full of [Pb] ____________." The sheriff drew his gun, but alas, was too slow. The Kid's gun,
blazing like flaming [Mg] ______________ did the [Cu] ____________ in. Anyone who drew on the Kid should know
his life wasn't worth a plugged [Ni] ______________. A [Pt] ____________ blonde riding beside the
[Al] ______________-framed coach rode for her life when the Kid pulled out some [N] ____________ compounds,
preparing to blow the safe to atoms. Suddenly, a shout rang out, "Hi Ho [Ag] ___________ and a masked man on a
white horse raced across the [Si] ____________ sands like [Na] ______________ skittering on H2O. A
[H] ______________ bomb would not have stopped the lawman; the Kid had met his doom. The rest of his life was to
be spent behind [Co] ___________ steel bars, a warning to all who flirt with danger. Your first detention may be the
initial step in a [C] ____________ copy life of the saga of the [Au] ____________ dust Kid.
~Author unknown
Protons, Neutrons & Electrons Practice w/s
Adapted from a worksheet from ChemFiesta.com
Directions: Using a periodic table and your knowledge, fill in the missing chart information below.
o
+
(same as #p )
Atomic Symbol Atomic Number
(Mass - #n )
(same as At #)
(same as #e )
(Mass - #p )
(same as #p )
(#p +# n )
Protons
Neutrons
Electrons
Atomic
Mass
B
+
+
6
11
23
31
39
39
29
89
35
43
98
Pb
207
103
89
Mo
70
227
54
81
24
+
204
o
100
157
No
259
Make Your Own Periodic Table w/s
For chemistry help, visit www.chemfiesta.com © 2009 All Rights Reserved
You’ve heard how the periodic table was invented and had a chance to make one in class. Now that you’re a pro at
classifying elements, you get a chance to make your very own periodic table using real elements. If you do this
correctly, your classification scheme should be the same as the actual periodic table.
Unfortunately, you’re not going to be given the names of the elements or a complete list of their properties. Using
partial information (such as scientists had in the old days), see if you can arrange these real elements into their proper
periods and families. One hint: These elements should be arranged into a grid that’s three boxes tall by four boxes
wide, with no blank spaces. [ie, the one below]
In no particular order:
Element 1: Solid, metal, does not corrode in air, density = 1.85 g/mL.
Element 2: Yellow gas, highly dangerous to handle, toxic in low doses.
Element 3: White, shiny, metallic solid, reacts slightly in air, density = 1.55 g/mL.
Element 4: Colorless gas, stable in air, forms very few chemical compounds.
Element 5: White, shiny metallic solid, unreactive, good electrical conductor, ductile,
density = 10.5 g/mL.
Element 6: Orange-red metallic solid, ductile, density = 8.9 g/mL.
Element 7: White metallic solid, reacts easily in air, density = 3.5 g/mL.
Element 8: Colorless gas, unreactive with any element.
Element 9: Red nonmetallic liquid, irritates skin and lungs.
Element 10: Colorless gas, denser than air, forms no chemical compounds.
Element 11: Radioactive metalloid, very little known about its properties.
Element 12: Yellow metallic solid, extremely malleable, unreactive with most
chemicals, density = 19.3 g/mL.
Good luck!
25
Trends in the Periodic Table – Graphing w/s
Graph paper is 32 x 32
1. Draw a line in the middle of a piece of graph paper, separating the page into top and bottom [DONE FOR YOU].
On the top, plot a graph of ionization energy (y-axis) vs. atomic number (x-axis). On the bottom plot a separate
graph of atomic radius vs. atomic number. For each graph, connect successive dots with straight lines. Also,
ensure that identical atomic numbers are plotted on the same vertical position on the sheet (i.e. atomic number
1 in the top graph should be on the same line as atomic number 1 in the bottom graph – your X axis is the
same).
2. Examine your graph of ionization energy (IE) vs. atomic number.
a. Which elements are found at the main peaks on your graph (there should be 3)? What do these
elements have in common?
b. Which elements are found at the main valleys on your graph (there should be 3)? What do these
elements have in common?
3. Examine your graph of atomic radius verses atomic number.
a. Which elements are found at the peaks on your graph? What do these elements have in common?
b. Which elements are found at the valleys on your graph? What do these elements have in common?
26
4. How are atomic radii and ionization energy related (i.e. as atomic radius increases, what happens to the
ionization energy)?
5. Generally, as you go from left to right across a period on the periodic table, what happens to…
a. atomic radius?
b. ionization energy?
6. Generally, as you go down a group in the periodic table, what happens to atomic radius and IE?
7. When Na forms an ion it loses its outer electron to become Na+. Draw Bohr diagrams for Na and Na+.
a. What element does Na+ resemble (with respect to its electron arrangement)?
b.
In general, which group’s electron configuration do the alkali metals resemble when they form ions
(i.e. lose an outer electron)?
8. Why does radius increase as you go down a group (hint: think of Bohr diagrams)?
9. Why would an increase in radius make it easier to lose an outer electron (i.e. give a lower ionization energy)?
10. What happens to the number of protons in the nucleus as you go across a period? Use this to explain the
trends in atomic radius and ionization energy across a period.
11. There is one group that is usually ignored because it does not follow the trends in the periodic table. Which
group is usually ignored?
12. Define electron affinity. In which corner of the periodic table is it highest? Explain why this is so.
13. Define Electronegativity. Where on the periodic table is it highest? Explain why this is the case.
Periodic Table Assignment w/s
[crossword follows on next page]
ACROSS
1. Synthetic elements with atomic numbers greater than 93
5. This law states that the properties of elements repeat as a function of their atomic number
7. Silicon is in this period
8. Elements were originally placed in order of atomic __, now they are in order of atomic __.
9. The group that consists of very nonreactive gases
10. Number of elements known in 1800
13. Element 101 was named in his honor
17. The periodic table is normally drawn with 18 columns. A more accurate representation has ___ columns
19. Most nonmetals are in this state
20. Nonmetal that is a liquid at SATP
21. The general name given to a column in the periodic table
22. According to figure 6, when aluminum combines with oxygen, three oxygen atoms combine with this many
aluminum atoms
DOWN
2. Elements that most closely follow the
12. Iodine belongs to this group
periodic law
14. The first alkali metal
3. The first scientist to organize elements
15. This element was assigned a relative atomic
based on repeating patterns
mass of one because it is the lightest element
4. The modern name for eka-silicon
16. The state of matter represented by (aq)
6. Most elements are ___, since they fall to the
18. Silicon is in this group
left of the "staircase line"
20. The staircase that separates metals and
11. The general name given to a row (left-to-right)
nonmetals begins below this element
in the periodic table
27
T
R A
N
S
U
R A
N I
C
D
E
O
P
B
R
E
E
R
S
E
E
I
N
T
N
A
R
T
E
W
E
N T Y O
N E
I
V
E
I
V
A
On the periodic table on the following page…
1. Place a large G in boxes that house elements that are gases at SATP, and a large L in boxes that contain
elements that are liquids. The rest of the elements are solids; do not write anything in these boxes.
2. Darken the “staircase line” that divides metals from non-metals
28
3. Metalloids (i.e. semi-conductors) are elements that have properties midway between metals and non-metals.
The metalloids are: B, Si, Ge, As, Sb, Te, Po, At. Identify the metalloids by drawing diagonal lines in these boxes.
4. Notice that each group (column) in the periodic table is identified at the top with a number and/or letter.
There are two conventions used in the textbook. Label the groups that end in A (e.g. IA, IIA, IIIA, etc).
5. Frame and color the following groups (note: H is not an IA metal): Alkali metals, alkaline earth metals, halogens,
noble gasses, transition metals, the inner transition elements (made up of lanthanides and actinides).
6. Create a legend for your periodic table.
Legend:
Fun Reviewing the Periodic Table w/s
1
Size of an atom.
MOATIC
RUDIAS
2
Atomic # = # of these.
RNTOPSO
3
Rows in the periodic table.
DORIPE
4
A chemical symbol
represents an ___.
LETNEEM
5
Exist in the nucleus of an
atom.
NENSOTRU
6
An element is made of
one of these.
TOAM
7
A diatomic nonmetal
which forms a green gas.
CLRNHOIE
8
Similar to oxidation
number.
HEGACR
9
Most are cations.
TEMLA
10
Metals in group 1.
LIAKAL
44
19
8
14
7
21
25
37
35
42
22
32
28
36
46
49
11
Most elements exist as ___
at room temperature.
DOSLIS
12
Any element in group 18.
NELBO ASG
13
Elements which donate electrons if ionically bonded.
TIOPESIV
CASNTIO
41
54
2
27
26
33
43
29
14
Protons + neutrons = this. CIMTAO SAMS
15
The outer shell of
electrons.
16
17
20
CAVNEEL LEHSL
12
Every valence shell
[except the first] strives TOCET LURE
to have 8 electrons.
Each element has
IATOCM BURENM
its own of this.
6
34
18
Columns on the
periodic table.
PROUG RO
LAMFIY
19
Metals in group 2.
KELLANAI TEARH
20
Elements which accept
electrons if ionically
bonded.
NEGVIATE NOINA
21
A proton + a
neutron = this.
22
Similar to charge.
23
39
48
5
24
NOATIOXID
Groups 3-12.
17
NAISONTITR
53 29
25
Surround the nucleus
of an atom.
CENTEOLRS
26
The most electronegative element.
ULFIENOR
27
Contains properties of both a
metal and a non-metal.
MOETADLIL
Creator of our modernday periodic table.
Increases as you
move across
CLEIENAVT
[L-R] on the
GOEYRITT
periodic table.
Exist as liquids
MOREBNI
at room
DAN
temperature.
CYRUREM
31
51
NEELUCNO
LNTENMOA
30
15
40
Most are anions.
29
10
52
24
28
23
50
11
16
30
1
VEMLENEDE
3
18
45
38
47
4
Use the numbers given in your unscrambled answers to solve the puzzle below.
J
1
2
3
4
5
6
7
8
9
10
11
12
13
?
24
30
25
26
,
27
28
29
15
16
,
30
.
14
31
4
32
33
J
17
18
19
20
21
22
W
34
35
!!
36
,
23
37
38
39
40
41
.

42
43
12
44
45
46
47
48
49
50
51
52
53
54
Periodic Table Practice Test
adapted from talsc.com - The Active Learning Science Classroom
1. In your own words, sum up the periodic law.
2. In the Periodic Table, rows are known as ____________________.
3. In the Periodic Table, columns are known as ____________________.
4. Group 1 is referred to as ____________________.
5. Group 2 is referred to as ____________________.
6. Groups 3 through 12 are known as ____________________.
7. Group 17 is known as ____________________.
8. Group 18 is known as ____________________.
9. There are two major families in the periodic table. What are they?
10. How did Mosley arrange his periodic table?
11. How did Mendeleev arrange his periodic table?
12. Explain the difference in ionization energy for sodium and magnesium.
13. True or false. Non-metals are an excellent conductor of electricity.
14. Argon is in group 18. Does group 18 have a high reactivity rate or a low reactivity rate? Why?
15. As you move down Group 1, does reactivity increase or decrease? Why?
16. As you move down group 17, does reactivity increase or decrease? Why?
17. Lithium is a shiny metal. When cut, it dulls quickly. It also reacts violently with water. Name another element
that would possibly show the same characteristics.
18. This group of elements are harder, stronger than group 1. They also have a higher melting point. Which
group are they?
19. This group of elements means “salt-former.” They are very reactive. They have an s2p5 electron
configuration. Which group are they?
20. Circle the element with the higher ionization energy.
a. Sodium vs. Magnesium
b. Oxygen vs. Fluorine
c. Iodine vs. Bromine
d. Lithium vs. Sodium
21. Which has the larger…? Nitrogen vs. Oxygen
a. Ionization Energy
b. Atomic Radius
22. Which has the larger…? Magnesium vs. Calcium
a. Ionization Energy
b. Atomic Radius
c. Electronegativity
c. Electronegativity
31
State the Trend.
Trend Down
Trend Across
23. Ionization Energy
24. Atomic Radius
25. Electronegativity
26. In 2-3 sentences, state why the downwards trend of atomic radius occurs that way.
27. In 2-3 sentences, state why the across trend of ionization energy occurs that way.
28. In 2-3 sentences, state why the across trend of melting point occurs that way.
Identify the following elements.
32
29. ________________ Period 4, Group 12
32. ________________ Calcium is in this row.
30. ________________ Filled with the 2p5 electron.
33. ________________ Nitrogen is in this column.
31. ________________ 9th e- in the 4d sub-level.
34. ________________ Chlorine is in this group.