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The Periodic Table-Chapter 6
Organizing the elements
A few elements, such as ______ and ________, have been known for thousands of
years.
Yet, only about ___ had been identified by the year 1700.
As more were discovered, chemists realized they needed a way to _____________
the _____________.
Mendeleev’s Periodic Table
Chemists used the ____________ of elements to sort them into __________.
By the mid-1800s, about ______ elements were known to exist
Dmitri Mendeleev – a Russian __________ and ____________ arranged elements
in order of ______________ __________ ________.
Thus, the first __________ _________ was created.
Moseley’s Periodic Table
In 1913, Henry Moseley – A British physicist, arranged ___________ according to
increasing _________ ___________
This is the arrangement used today
The __________, __________ _________ & _________ are basic items included.
The Periodic Law states:
 When elements are arranged in order of ________________atomic number,
there is a periodic ____________of their physical and chemical
___________________.
 Horizontal rows = ____________
o There are ___ _________
 Vertical column = _________ (or __________)
o Similar ___________ & _____________ properties
o Identified by __________ & ________ (IA, IIA)
Areas of the Periodic table
Three classes of elements are: ___________, _____________, and
____________
Metals: electrical conductors, have ________, are __________ and malleable
Nonmetals: generally ________ and dull, poor conductors of heat and electricity.
Metalloids: border the line-2 sides
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Properties are intermediate between _____________ and _______________
 Notice the heavy, _________-______ line?
Remember: Many periodic tables are set up differently.
Make sure to pay attention!
Electron Configuration in Groups
Elements can be sorted into 4 different groupings based on their ___________
________________:
1. Representative Elements
2. ____________ __________
3. __________ ________
4. Inner transition metals
1) Representative Elements are in Groups 1A through 7A
• They display wide range of ___________.
• Their outer s and p electron configurations are __________ _________
or already full.
2) Transition metals are in the “B” columns of the periodic table
• A __________ between the _______ area and the ____________ area.
• Electron configuration has the outer s sublevel ______, and is now filling
the “d” sublevel.
3) Noble gases are the elements in Group ___ ___ (also called Group 18)
• Previously called “________ _________” because they rarely take part in
a reaction; very stable = _______ _______.
• Electron configuration that has the outer s and p sublevels ____________
___________. The d sub levels may or may not be full.
4) Inner Transition Metals are located below the ______ body of the table, in
_____ rows
• Formerly called “______-_______” elements, but this is not always true
because some are very abundant.
• Electron configuration has the outer ____ sublevel full. The p and d
___________ may or may not be _______. The ____ ____________ is
filling.
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Elements in the 1A-7A groups are called the representative elements
Group 1A are the __________ __________ (but NOT H)
Group 2A are the __________ _________ ____________
Group 8A are the _________ __________
Group 7A are the _________
Trends in Atomic Radius
First problem: Where do you start measuring from?
The __________ ____________ doesn’t have a definite edge.
They get around this by measuring more than 1 atom at a time.
Atomic Size
Measure the Atomic Radius - this is ________ the distance between the _______
nuclei of a diatomic molecule.
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Atomic Size- Group Trends
 As we increase the atomic number or go down a group. . .
each atom has another energy level, so the atoms get __________.
Atomic Size-Period Trends
 Going from left to right across a ___________, the size gets __________.
 ____________ are in the same energy level.
 But, there is more nuclear charge.
 Outermost __________ are pulled closer to the atom’s nucleus.
Ions
 An ion is an atom or group of atoms that has a ________ or _________ charge.
 Remember that atoms are neutral because the # of protons = # of electrons.
 Some compounds are composed of particles called ions.
 Positive and negative ions are formed when __________ are __________ (lost
or gained) between atoms.
Metals tend to LOSE electrons, from their outer energy level
 Sodium loses one: there are now more protons (11) than electrons (10), and
thus a __________ charged particle is formed = “___________”
 The charge is written as a number followed by a plus sign: _________
 Na1+ is re-named a “__________ ________”
Nonmetals tend to GAIN one or more electrons
• Chlorine will gain one _________
• Protons (17) no longer equals the electrons (18), so a charge of 1• _______________ ions are called “___________”
• Cl1- is re-named a “chloride ion”
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Ionization Energy Trends
________________ energy is the amount of energy required to completely remove
an electron (from a gaseous atom).
Removing one ______________ makes a 1+ ion.
The energy required to _________ only the first __________ is called the first
ionization energy.
The second ionization energy is the energy required to remove the __________
__________.
Always greater than first IE.
And so on…
Ionization Energy - Group Trends
As you go down a group, the first ionization energy decreases because...
The _____________ is further away from the attraction of the
____________.
Ionization Energy - Period Trends
 All the atoms in the same period have the ________ __________
_________.
 Increasing nuclear charge
 So IE generally _____________from left to right.
 Exceptions at full and 1/2 full ____________.
Driving Forces
Full Energy Levels require lots of energy to ____________ their electrons.
Noble Gases have _______ __________ __________.
Atoms behave in ways to try and achieve a __________ ______ configuration.
Trends in Ionic Size: Cations
 ____________ form by _________ electrons.
 Cations are __________ than the atom they came from – not only do they lose
electrons, they lose an ____________ ___________ ____________.
 Metals form _________.
Trends in Ionic size: Anions
 Anions form by _________ electrons.
 Anions are ___________ than the atom they came from – have the same
________ level, but a greater area the nuclear charge needs to cover
 ___________ form _________.
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Electronegativity Trends
 _______________________ is the tendency for an atom to __________
electrons to itself when it is chemically combined with another______________.
 They ________ the electron, but how equally do they share it?
 An element with a big electronegativity means it pulls the
______________towards itself _____________!
Electronegativity Trends-Groups
 The further _________ a group, the ____________ the electron is away from
the _______________, plus the more electrons an atom has.
 This causes the electronegativity to ____________ as you go down the group.
Electronegativity Trends-Periods
 Metals are on the _______ of the table.
 They let their ____________ go easily
 This causes electronegativity to be on the low side.
 On the ________ are the _______________.
 They want more ____________, so they try to take them away from others
 This causes electronegativity to ____________ as you go across the table.
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