Download The Particle Theory of Matter

Chapter 2 - Elements and Compounds Notes
The Particle Theory of Matter
1. All matter is made up of _____________________.
2. All particles of one substance are the __________. Different substances
are made up of _____________________.
3. The particles are always _______________. The more energy the
particles have, the _______________________.
4. There are attractive forces between the particles. These forces are stronger
when the particles are closer together.
 There are attractive forces between particles. In a solid, the attraction
between particles is ____________________________. The particles are
____________________, but they are not able to _________________
each other. They just _______________.
 In a liquid the attractive forces are _____________. The particles are able
to __________________________________. The forces are strong
enough to keep the particles from _________________.
 In a gas, the attraction between particles is __________________
______________________________________ that they are held.
 As well as classifying matter as solids, liquids, and gasses, we can classify
matter as either a ________________________________.
 A ______________ is made from only one type of particle. These specific
particle types give the substance its _________________ such as odor,
color, hardness.
 A ______________ contains two or more pure substances. (See Fig. 1 pg.
45)
 A ____________________ has two substances where the particles are
____________________________. To the eye, the mixture appears to be
pure substance.
 When the particles stay intermixed and don’t settle into layers we call the
homogeneous mixture a __________________.
 A ____________________ has large clumps of particles that ____
_________________________________ with the other substance.
 Examples of heterogeneous mixtures are ____________________
_____________________________________________________
Elements and Compounds
• Elements are _____________________ that _________________
_____________________________________________________.
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Chapter 2 - Elements and Compounds Notes
• Compounds are pure substances that ________________________ in a
fixed proportion. They are formed when elements _________
__________________________________________.
Atoms and Molecules
• The particles that make up the particle theory are now known as
_________________.
• Each element is made up of only one kind of atom.
• When 2 or more atoms join together, they form a _____________.
• Molecules can contain ______________________ or __________
________________________________.
• Different molecules can also be made up of the same elements but in
different proportions.
What makes up an atom?
• Three types of particles make up an atom; these are called
__________________________.
• _____________________________________________________
• _____________________________________________________
• _____________________________________________________
Properties of Metals
• Metals are ____________________________________________.
• Metals are ____________________
• Metals are ___________________________________________
• Metals are ___________________________________________
• A chemical property of metal is its reaction with water which results in
_____________________.
Properties of Non-Metals
• Non-metals are ________________________________________.
• Non-metals are ________________________________________.
• Solid non-metals are _________________________________.
• They are ___________________________________.
• Many non-metals are ____________________.
Properties of Metalloids
• Metalloids (metal-like) have properties of ___________________
__________________________________________________.
• They are solids that can be ___________________________.
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Chapter 2 - Elements and Compounds Notes
• They conduct heat and electricity better than non-metals but not as well as
metals.
• They are __________________________________________
Chemical Symbols
• All elements have their own unique symbol.
• It can consist of a ______________________________________
_____________________________________________________
• Elements have their name for a variety of reasons. Some are named after
mythology, countries, scientists or in Latin or Greek.
•So how do we know how many protons, neutrons and electrons are in an
atom?_____________________________________________________
•What’s in a square?
•Different periodic tables can include various bits of information, but
usually:_______________________________________________________
Key to the Periodic Table
•Elements are organized on the table according to their _________________,
usually found near the top of the square.
•The atomic number refers to how many __________________________ an
atom of that element has.
•For instance, hydrogen has ___proton, so it’s atomic number is ______.
•The atomic number is unique to that element. No two elements have the
same atomic number.
Atomic Mass
•Atomic Mass refers to the “weight” of the atom.
•Protons and Neutrons have a mass of ___________. Electrons weigh
_________________ thus are given a mass of ______ for our purposes now.
•So Atomic mass is derived at by adding the number of ______________
with the number of _________________________.
•So to find the # of neutrons we use the following:
•
__________________________________________________
Valence Electrons
•The number of valence electrons an atom has may also appear in a square.
•Valence electrons are the electrons in the ___________________________
of an atom.
•These are the electrons that are transferred or shared when atoms bond
together.
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Chapter 2 - Elements and Compounds Notes
•What does it mean to be reactive?
•We will be describing elements according to their reactivity.
•Elements that are reactive bond easily with other elements to make
compounds.
•Some elements are only found in nature bonded with other elements.
•What makes an element reactive?__________________________________
•All atoms (except hydrogen) want to have ______electrons in their very
outermost energy level (This is called the octet rule.)
•Atoms bond until this level is complete. Atoms with less than 4 valence
electrons lose them during bonding. Atoms with 6, 7, or 8 valence electrons
gain electrons during bonding.
•Elements that have either gained or lost electrons are called ____________.
•Positively charged ions: ______________________
•Any atom that loses electrons to form compounds are called
______________. Cations have a __________________ charge.
•Naming cations: Use the element name followed by __________________
Some Cations have more than one charged form.
•Negatively charged ions: __________________
•Atoms that ___________ electrons to form compounds are called
_____________. Anions have a __________________ charge.
•Naming Anions: Drop the last few letters of the element name and add
_____________________
How can we determine the charge of an ion?
•For some of the elements it is very easy. Elements in groups 1, 2, 13, 14,
15, 16, & 17 will lose or gain electrons so they have the same # as the nearest
Noble Gas (group 18).
•The transition metals (groups 3- 12) cannot have their charges predicted in
this way due to many of them having isotopes. Their charges must be
predicted in other ways.
Noble Gases
•Noble Gases are colorless gases that are extremely un-reactive.
•One important property of the noble gases is their inactivity. They are
inactive because their outermost energy level is full.
•Because they do not readily combine with other elements to form
compounds, the noble gases are called inert.
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Chapter 2 - Elements and Compounds Notes
•The family of noble gases includes helium, neon, argon, krypton, xenon,
and radon.
•All the noble gases are found in small amounts in the earth's atmosphere.
Chemical Formulas
• When atoms of different elements combine, they form _________.
• A chemical formula is the combination of symbols that represents a
particular compound. (Table 2 pg. 59).
• If there is more than one atom of the element in a compound, the symbol is
followed by ___________________________________
• Eg. __________________________________________________
Names and Formulas for Compounds
• Chemical formulas are used to represent compounds, but how are the
compounds made? How do we know that sodium and chlorine combine to
make NaCl and not Na2Cl or NaCl2, etc.?
Rules For Combining Elements
• Rule 1: ______________________________________________.
• Rule 2: Write the name of the metal _____________ and the non metal
________________.
• Rule 3: Change the ending of the _________________________.
• Rule 4: Each atom has its own __________________________.
• Rule 5: Atoms combine so that ____________________________
___________________________________________.
Combining Capacity
• Combining capacity is the ability of an element to combine with other
elements.
• It is a _____________________ given to each metal and non metal to
explain the compounds that they form.
• For example. Both sodium and chlorine are assigned a combining capacity
of 1. This means that each of these elements can make 1 connection. Thus
the formula for this compound is NaCl.
• The combining capacities for some metals and non metals are in Tables 2
& 3 on pg. 64.
• When naming the compound, _____________________________
_____________________________________________________
• ___________________________________
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Chapter 2 - Elements and Compounds Notes
• There are some elements that have more that one combining capacity.
• When writing the names (not the symbols) for these compounds, the
combining capacity must be written in ___________________ between the
metal and non metal.
• Example: ____________________________
• _____________________________________
When combining 2 ions, you need to create ________________________.
2+
 Eg. Ca + Cl
CaCl2 (2 positives, 2 negatives = 0 charge)
If you do not know the combining capacity of the element, you can use your
knowledge of ions. The charge of the ion is its combining capacity.

Crossing Over Method
Ca2+ + O2-
Mg2+ + Cl-
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