MRHS
Chemistry
Name: ________________________________________________ Date: _____________ Pd: __________ Day: ________
Answer the following questions to create an outline for Chapter 4. Use your textbook, pages 72-103 as you work through these problems. DUE _________________________________
Section 4.1: The Elements
1.
Presently, how many different elements are known to exist? ______________. a.
Of these, how many occur in nature? ____________ (WARNING: YOUR TEXTBOOK GIVES AN INACCURATE
COUNT, PLEASE USE OTHER RESOURCES/PERIODIC TABLE TO DETERMINE ANSWER). b.
How many are synthetic or manmade? _________ c.
How many elements account for most of the compounds on earth? ____________
2.
List the first six MOST abundant elements by MASS in the Earth’s crust, in order from highest to lowest. a.
_________________________ b.
_________________________ c.
_________________________ d.
_________________________ e.
_________________________ f.
_________________________
3.
In what form is the most abundant element found? _____________________________________________. a.
What percent of our atmosphere does this element make up? ______________
4.
List the first six MOST abundant elements by MASS in the human body, in order from highest to lowest. a.
_________________________ b.
_________________________ c.
_________________________ d.
_________________________ e.
_________________________ f.
_________________________
5.
What are trace elements (in living matter)? ___________________________________________________________
_______________________________________________________________________________________________ a.
List TWO trace elements found in the human body. Give the USE for each i.
__________________: ________________________________________________________ ii.
__________________: ________________________________________________________
4.2: Symbols for Elements
6.
Describe the format used for writing symbols of elements: ______________________________________________
_______________________________________________________________________________________________
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Chapter 4: Chemical Foundations: Elements, Atoms and Ions
Guided Notes Outline

7.
Give three reasons why certain elements have symbols that don’t match their English names? a.
________________________________________________________________________________________ b.
________________________________________________________________________________________ c.
________________________________________________________________________________________
8.
List the symbol for the following elements. Give the non-English NAME and ORIGIN, and the meaning of the name.
English Name Symbol Original Name
Lead
Gold
Tungsten
Language / Place Meaning (if relevant)
Tin
Potassium
***You need to know the first 36 element names and symbols, PLUS additional common ones like gold, silver, uranium, lead, Iodine, Radon, Radium, Barium, Mercury etc. *** Quiz coming up very shortly
4.3: Dalton’s Atomic Theory (Review)
9.
What two factors did scientists begin to understand in the eighteenth century a.
Most natural materials are ____________________ of _____________________________________ b.
Pure substances are either ___________________ or combinations of elements called _________________. c.
A ____________ compound always __________________________________________________________. i.
Known as the law of ________________________________________________.
1.
Give an example: ____________________________________________________________. ii.
Person credited with above law: __________________ d.
List the five postulates of Dalton’s Atomic Theory i.
__________________________________________________________________________________ ii.
__________________________________________________________________________________ iii.
__________________________________________________________________________________ iv.
__________________________________________________________________________________ v.
__________________________________________________________________________________
4.4: Formulas of Compounds
10.
RECALL: A compound is made of ______ or more elements _________________ bonded, with properties (circle 1)
SAME AS / DIFFERENT FROM component elements.
11.
Represented by ________________________________ a.
Each element is represented by its element __________________ b.
The number of each type of element is indicated by a _____________ written as a ________________.
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Chapter 4: Chemical Foundations: Elements, Atoms and Ions
Guided Notes Outline

c.
____________________
2.
Fill in the following table indicating the properties of the three subatomic particles. (HINT: Not given in your textbook. Search online for “subatomic particle properties” and you should be able to find the information relatively easily)
Particle Symbol Symbol Charge Location Actual mass (kg) Mass # (amu) Relative Mass
(amu) i.
If ONLY 1 atom of a particular element is needed, only the ___________ is written, and
_____________ is NOT required. c.
Example: Indicate the type and count of each element in the following compounds. The first one is done for you. i.
Mg
3
N
2
: 3 atoms of Magnesium, 2 atoms of Nitrogen ii.
H
2
SO
4
______________________________________________________________ iii.
Mg(OH)
2 ______________________________________________________________________________________________ iv.
Ca
3
(PO
4
)
2 _____________________________________________________________________________________________ d.
Practice: Write the formula for the following: i.
Molecule containing four phosphorous atoms and ten oxygen atoms: __________ ii.
Molecule containing one uranium atom and six flourine atoms: _________ iii.
Molecule containing 1 aluminum atom and three chlorine atoms: ________________
4.5: The Structure of the Atom/4.6: Modern Concept of Atomic Structure
1.
The atom is composed of ____________ ________________ particles a.
____________________ b.
____________________
3.
What is meant by the term Nuclear Atom:
___________________________________________________________________________________________
___________________________________________________________________________________________
4.
“All atoms are composed of these same components, why do different atoms have different chemical properties”. Answer the following questions based on the above statement a.
Which subatomic particle determines chemical behavior: _____________________. This is based on both the __________________ and ___________________ of the above particle. i.
Explain why: ____________________________________________________________________
______________________________________________________________________________ b.
Which subatomic particle count NEVER changes for a given element? ________________. c.
INFER: Which of the above two subatomic particles can you use to identify the element? ____________.
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Chapter 4: Chemical Foundations: Elements, Atoms and Ions
Guided Notes Outline

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Chapter 4: Chemical Foundations: Elements, Atoms and Ions
Guided Notes Outline

4.7: Isotopes
5.
Atoms of the _____________ element (identified by the number of _______________) with a difference in the number of _________________.
6.
Who is the person credited with identifying the THIRD subatomic particle: ____________________
7.
Which of Dalton’s postulates did this discovery change? ______________________________________________ a.
Why? ________________________________________________________________________________
8.
The ATOMIC number indicates the ______________________________________________________________.
It is represented by the following letter: ________
9.
The MASS number indicates the ________________________________________________________________.
It is represented by the following letter: ________
10.
The following letter is used to represent the generic symbol of an element: ________ a.
Examples. i.
Use figure 4.10 to indicate the composition of the two isotopes of sodium.
1.
Isotope 1: 2.
Isotope 2: a.
X = ________ b.
A# = ________ a.
X = ________ b.
A# = ________ c.
Z# = ________ c.
Z# = ________
11.
When comparing two isotopes of a given element, the ______________ number will ALWAYS be the same, the
______________ number will be different.
12.
If the atom is neutral (total charge of ZERO), then the number of _____________ is EQUAL to the number of
______________.
13.
Elements are often represented as shown below. What does each symbol in the notation given below indicate?
A# X
Z#
A#: ____________________
Z#: ____________________
X: _____________________
14.
Based on the above notation, identify the following elements, number of protons and number of neutrons. The first one is done for you. a.
13
6
C indicates the following i.
C : symbol for element Carbon ii.
13 (superscript): A# = Mass # = sum of protons and neutrons iii.
6 (subscript): Z# = atomic # = # protons iv.
Number of Neutrons =
______
ANSWER: 7 neutrons
=
Mass Number – Atomic Number
13 – 6
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Chapter 4: Chemical Foundations: Elements, Atoms and Ions
Guided Notes Outline

b.
40
20
Ca i.
Element: _______________ ii.
Mass Number: __________ c.
19
9
F i.
Element: _______________ ii.
Mass Number: __________ iii.
Atomic Number: _________ iv.
Number of Neutrons: ________ iii.
Atomic Number: _________ iv.
Number of Neutrons: ________
15.
Practice: Fill in the table based on the information given. Assume neutral atom
Symbol Element Name Atomic Number
(# of protons)
Number of
Neutrons
Number of
Electrons
64
29
Cu
Phosphorous 17
11
5
B
47
12 12
Mass Number
108
4.8: Introduction to the Periodic Table
16.
First periodic table to follow similar pattern as today (rows and columns), developed by Russian scientist
___________________.
17.
What does the term “periodic table” refer to (or is based on)?
___________________________________________________________________________________________
___________________________________________________________________________________________ a.
List two other natural phenomenon you can think or that are “periodic”
______________________________________ and ___________________________________________
18.
Vertical columns on the periodic table are called _______________. a.
Sometimes these are also referred to as _______________ because they have _________________ chemical properties. b.
There are __________ columns. i.
19.
Horizontal rows are called _____________. a.
There are __________ rows b.
Properties of element _______________ as you go across a row, and then ____________ when you return to same group. c.
These correspond to the following quantum number _________________________________________, symbolized by letter ______. (Ch. 11)
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Chapter 4: Chemical Foundations: Elements, Atoms and Ions
Guided Notes Outline

20.
Regions of the periodic table: Indicate the location of the following: Alkali metals, Alkali Earth metals, Noble
Gases, Halogens, Lanthanides, Actinides, Transition metals, Metalloid ladder, metalloids, non-metals, metals. a.
Group 1A: _________________________________ b.
Group 2A: _________________________________ c.
Group 7A: _________________________________(sometimes represented as group _______) d.
Group 8A: _________________________________(sometimes represented as group _______) e.
Group B: _________________________________ (sometimes represented as groups ______ to ______) f.
Most elements are ________________ i.
Typical properties
1.
_______________________________________________________________________
2.
_______________________________________________________________________
3.
_______________________________________________________________________
4.
_______________________________________________________________________
5.
Example: ________________________________________________________________
6.
Most are ____________ at room temperature. Exception ______________. g.
Separated from non-metals by ________________. i.
Represented on the ___________________________. Exception ______________ (_________). ii.
Sometimes called _____________________ iii.
Show mixture of ______________ and ________________ properties.
1.
Example: silicon and boron are relatively _________________, however a mixture of these two creates a ____________________ h.
Non-metals: Located to the _______________ of the metalloid ladder i.
Typical properties
1.
___________ properties of metals
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Chapter 4: Chemical Foundations: Elements, Atoms and Ions
Guided Notes Outline

2.
Many are ___________. Some are ___________. One is __________ (_____________).
3.
Solids tend to be ________________, meaning they crumble or are powdery.
4.
Poor ______________________ meaning they DO NOT conduct heat well. Tend to make good __________________ meaning they conserve heat well.
4.9: Natural State of Elements
21.
Most matter around us exists as _________________. Generally these mixtures are made of _______________.
22.
Elements are generally (circle one) FOUND / NOT FOUND in elemental form. This is because in the elemental form, most elements are (circle one) STABLE / VERY REACTIVE a.
Some exceptions are elements ____________, ____________ and ________________. Often called
_______________________________ because they are relatively unreactive. b.
Another ENTIRE group that is an exception to the above rule is group 18, or the ____________ gases. i.
In this context, the term “noble” means _________________________________________.
23.
What are diatomic molecules? _________________________________________________________________ a.
There are ______ elements that exist as diatomic molecules. They are (indicate name and symbol)
1.
________________________________________________________________________
4.10: Ions
24.
What are ions? _______________ atoms a.
Due to ____________ or ____________ of electrons
25.
Sodium tends to (circle one) GAIN / LOSE electrons to form (circle one) NEGATIVE / POSITIVE ion called a (circle one) ANION / CATION. This is represented as __________ a.
In general, metals tend to ____________ electrons to form _________________ ions, called
_____________ i.
Example: Ca +2
1.
WHY? Ex: Neutral Calcium has _______________________. Loses __________ so negative charge is __________
.
Total charge is _______________________
26.
Chlorine tends to (circle one) GAIN / LOSE electrons to form (circle one) NEGATIVE / POSITIVE ion called a (circle one) ANION / CATION. This is represented as __________ a.
In general, non-metals tend to _____________ electrons to form ________________ ions, called
____________. i.
Example: O -2
1.
WHY? Ex: Neutral Oxygen has _______________________. Loses __________ so negative charge is __________
.
Total charge is _______________________
27.
True or False: Isolated atoms can exist in ionic form. a.
If false, under what conditions do these ions form?
28.
Indicate the most common charge of Ions based on an element’s position on the periodic table. a.
Group 1A: ____________
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Chapter 4: Chemical Foundations: Elements, Atoms and Ions
Guided Notes Outline

b.
Group 2A: ____________ c.
Group 3A: ____________ (exception: _____________) d.
Group 6A: ____________ e.
Group 7A: ____________ f.
Group 8A: ____________
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Chapter 4: Chemical Foundations: Elements, Atoms and Ions
Guided Notes Outline