Name: ______

Periodic Table Trends

Organization of the Periodic Table

  1. First created by Dmitri Mendeleev
  2. Organized atoms by ______
  1. This was ok, but trends in the periodic table did not match up
  1. 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.
  1. The trends found by Mendeleev were in place.

Periodic Law

  1. States that physical and chemical properties of elements are

properties of their ______.

  1. Each column on the periodic table is called a ______
  1. Groups have the same number of

______in their

outer-most sublevel

  1. Each row in the periodic table is called a ______
  1. Elements in the same period share the same

______.

Noble Gases

  1. Group ______
  1. Have filled ____ and ____ orbitals
  1. Are very ______. Do not form bonds with other

molecules

  1. All atoms desire to be noble gases and will ______or

______electrons from other atoms to do so.

  1. This is how a ______

is made

  1. To act like noble gases, atoms will take the easiest route, and either give up electrons or gain them

Alkali Metals

  1. Found in ______
  1. Made of ______(meaning easy to bend)
  1. Outer electron shell has an ______configuration
  1. React quickly with ______or ______
  1. Can create a basic ______with water
  1. Have an extra electron to give up in order to form a ______ion.

Alkaline Earth Metals

  1. Group _____
  1. Outershell has a ______configuration
  1. Metals are ]______and ______reactive
  1. Become ions with a _____ charge

Transition Metals

  1. Groups ______
  1. ______metals and even ______reactive

than groups 1 and 2

Lanthanides

  1. Contain atomic numbers 57-71
  1. Shiny and reactive ______
  1. Some glow when electrons hit them.
  1. ______series

Actinides

  1. ____ series
  2. All are ______
  1. ______important for nuclear reactions
  2. Many are man-made

Main Block Elements

  1. Groups 3A-8A
  1. Made of

______

______

  1. Metal examples: aluminum, gallium, indium, tin thallium, lead, bismuth, polonium
  2. Metalloids: boron, silicon, germanium, arsenic, antimony, and tellurium.
  3. Nonmetal examples: hydrogen, oxygen, nitrogen, carbon, phosphorus, sulfur, selenium, fluoride, chlorine, bromide, iodine, and noble gases
  1. The periodic ______: The area on the

periodic table that divides the metals from the nonmetals

  1. Atoms around the stair step are ______
  1. Metalloids have characteristics of nonmetals and metals
  1. Metalloids are also termed

______

Halogens

  1. Group _____
  1. Form salts with ______metals
  1. The most ______nonmetals
  1. ______electrons to have a noble gas

configuration

  1. Become a ______ion if this happens

Chalcogens

  1. Group _____
  1. Try to gain two electrons to have a noble gas electron configuration.
  1. Become a _____ ion if this happens

Periodic Trends

  1. The four different trends to know include:
  1. ______
  1. ______
  1. ______
  2. ______

Electronegativity

  1. Defined by an atoms tendency to attract electrons in a chemical bond.
  1. In a chemical bond, atoms have to

______

  1. The atom with a higher electronegativity will keep the electrons closer to it.
  1. Atoms with the highest electronegativity are found in the

______-side of the periodic table; excluding

noble gases.

  1. The atom with the highest electronegativity is

______

  1. The lowest is ______

Atomic Radius

  1. Atoms with the largest atomic radius are found at

______-side of the periodic table

  1. The further you go down the periodic table, the more

______an atom contains.

  1. This means, assuming the atom looks like a sphere, the

______of the atom would increase as you go down the

periodic table.

  1. The top, right-area of the periodic table has the smallest atomic

radius ______

  1. Which would you assume to have the largest atomic radius: Al, Al+, or Al-
  1. Which would you assume to have the smallest atomic radius: C2+, C+, C, C-, C2-

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.
  1. ______has the highest ionization energy

Electron Affinity

  1. The ability of an atom to ______and hold onto an atom.
  1. Electron affinity is highest in the

______of the periodic table.

3. ______has the highest electron affinity.

4. ______: inner electrons are shielded by outer electrons, so outer electrons are removed before inner electrons.

  1. That is why ______is so reactive. It quickly reacts with something around it.
  2. Electrons in the outer energy levels feel ______of the nuclear charge (they feel ______of the positive charge).
  3. This is commonly referred to as ______. Most trends can be described by the shielding effect and effective nuclear charge.