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Name: _________________________________
3. Each row in the periodic table is called a ________________
Periodic Table Trends
4. Elements in the same period share the same
Organization of the Periodic Table
1. First created by Dmitri Mendeleev
A. Organized atoms by ________________________
__________________________.
Noble Gases
B. This was ok, but trends in the periodic table did not
match up
C. Mendeleev was able to predict how elements interacted
with each other and wanted his table to display those
trends.
Henry Moseley
1. Took the ____________________charge, which is the number
of protons in the nucleus, and ordered the periodic table using
the number of protons in the atom.
2. The trends found by Mendeleev were in place.
Periodic Law
1. States that physical and chemical properties of elements are
properties of their ___________________________________.
2. Each column on the periodic table is called a ______________
A. Groups have the same number of
_____________________________ in their
outer-most sublevel
1. Group _______
2. Have filled ____ and ____ orbitals
3. Are very _________________. Do not form bonds with other
molecules
4. All atoms desire to be noble gases and will ____________ or
__________electrons from other atoms to do so.
A. This is how a _________________________________
is made
5. To act like noble gases, atoms will take the easiest route, and
either give up electrons or gain them
Alkaline Earth Metals
Alkali Metals
1. Group _____
1. Found in ________________________
2. Made of _________________________ (meaning easy to
bend)
3. Outer electron shell has an _______ configuration
4. React quickly with ______________ or ________
A. Can create a basic _________________ with water
5. Have an extra electron to give up in order to form a _______
ion.
2. Outershell has a ________configuration
3. Metals are ]____________ and __________ reactive
4. Become ions with a _____ charge
Transition Metals
3. Some glow when electrons hit them.
4. _______ series
Actinides
1. Groups __________________
2. __________________ metals and even ___________ reactive
than groups 1 and 2
Lanthanides
1. ____ series
2. All are ________________
A. ___________________ important for nuclear reactions
B. Many are man-made
Main Block Elements
1. Groups 3A-8A
2. Made of
______________________________________________________
1. Contain atomic numbers 57-71
2. Shiny and reactive _______________
_____________________
A. Metal examples: aluminum, gallium, indium, tin
thallium, lead, bismuth, polonium
B. Metalloids: boron, silicon, germanium, arsenic,
antimony, and tellurium.
C. Nonmetal examples: hydrogen, oxygen, nitrogen,
carbon, phosphorus, sulfur, selenium, fluoride, chlorine,
bromide, iodine, and noble gases
configuration
A. Become a ________ ion if this happens
Chalcogens
3. The periodic _________________________: The area on the
periodic table that divides the metals from the nonmetals
1. Group _____
A. Atoms around the stair step are ___________________
i.
Metalloids have characteristics of nonmetals
and metals
ii.
Metalloids are also termed
2. Try to gain two electrons to have a noble gas electron
configuration.
A. Become a _____ ion if this happens
Periodic Trends
________________________________
1. The four different trends to know include:
Halogens
A. ________________________________________
B. ________________________________________
C. ________________________________________
D.
E. ________________________________________
Electronegativity
1. Defined by an atoms tendency to attract electrons in a chemical
bond.
1. Group _____
2. In a chemical bond, atoms have to
2. Form salts with __________________ metals
_____________________________________
3. The most ____________________ nonmetals
4. ______________________ electrons to have a noble gas
3. The atom with a higher electronegativity will keep the
electrons closer to it.
4. Atoms with the highest electronegativity are found in the
_____________________________ an atom contains.
____________________-side of the periodic table; excluding
1. This means, assuming the atom looks like a sphere, the
noble gases.
______________________ of the atom would increase as
you go down the
5. The atom with the highest electronegativity is
periodic table.
______________________
3. The top, right-area of the periodic table has the smallest atomic
1. The lowest is ___________________
radius ____________________
Atomic Radius
4. Which would you assume to have the largest atomic radius: Al,
Al+, or Al5. Which would you assume to have the smallest atomic radius:
C2+, C+, C, C-, C21. Atoms with the largest atomic radius are found at
_______________________________-side of the periodic table
2. The further you go down the periodic table, the more
PROBLEM: Using only the periodic table, rank each set of main group
elements in order of decreasing atomic size:
(a) Ca, Mg, Sr
(b) K, Ga, Ca
(c) Br, Rb, Kr
(d) Sr, Ca, Rb
Electron Affinity
1. The ability of an atom to ___________________ and hold onto
an atom.
Ionization Energy
1. Defined as the energy needed to remove an electron from an
atom
2. The __________________________-area of the periodic table
contains the atoms with the highest ionization energy.
2. Electron affinity is highest in the
________________________________________ of the periodic
table.
3. _________________ has the highest ionization energy
3. _______________ has the highest electron affinity.
PROBLEM: Using the periodic table only, rank the elements in each of the
following sets in order of decreasing IE1:
(a) Kr, He, Ar
(b) Sb, Te, Sn
(c) K, Ca, Rb
(d) I, Xe, Cs
4. _____________________________: inner electrons are
shielded by outer electrons, so outer electrons are removed before
inner electrons.
A. That is why _____________________ is so reactive. It
quickly reacts with something around it.
B. Electrons in the outer energy levels feel _______ of the
nuclear charge (they feel ________ of the positive
charge).
C. This is commonly referred to as
________________________________. Most trends
can be described by the shielding effect and effective
nuclear charge.