Properties of Elements Study Guide (Ch. 19 and Ch. 25 Section 1)
Metals
Nonmetals
Metalloids
Ductility
Malleability
Luster
Alkali Metals
Alkaline Earth Metals
Terms You Need to Know
Halogens
Noble Gases
Transition metals
Inner transitional
metals
Coinage metals
Iron triad
Ion (cation, anion)
Bonding (ionic,
metallic, covalent)
Salt
Allotrope
Alloy
Diatomic molecule
Semiconductor
Superconductor
Be able to identify the location of the following on a periodic table:
Metals
Alkaline Earth Metals
Inner transitional
Nonmetals
Halogens
metals
Metalloids
Noble Gases
Coinage metals
Alkali Metals
Transition metals
Iron triad
What are the similarities and differences between the three types of bonding?
Similarities – all involve electrons changing locations.
Differences – In ionic bonding, electrons are given from one atom to another,
causing the atoms to be bonded. This usually happens between metals and
nonmetals or metals and semimetals. In covalent, the electrons are shared. This
often happens in bonds between nonmetals. Metallic bonding involves only metal
atoms and electron clouds overlap, allowing them to move easily from one atom
to another (conductivity).
What types of elements combine to form salts?
Halogens (group 17) gets electrons from metals in ionic bonds.
What is the purpose of forming alloys?
Combining metals with different properties creates an alloy with some properties
of each of the component metals. The alloys can have better strength, durability,
resistance to corrosion, malleability, ductility, etc.
What are the most reactive metals? Why are they so reactive?
The alkali metals (group 1 minus H). they are so reactive because they have only
one valence electron in their outer shell. They would be more stable if they had a
full outer shell and giving one away gives them a full outer shell.
What are the most stable elements? Why are they so stable?
The noble gases (group 18). They have a full outer shell, making them stable and
nonreactive. The noble gases will react very rarely under specific conditions. This
is more the exception than the rule however.
How are different carbon allotropes similar? How are they different?
Allotropes are similar because they are all made up of only carbon atoms bonded
to other carbon atoms. They are different because they have different structures
and shapes. The way the carbon atoms are bonded gives each allotrope different
properties.
What properties do metals have?
Usually (but not always) metals are: malleable, ductile, very lustrous, strong, solid
at room temperature, and good conductors of heat and electricity.
Where are metals/semimetals/nonmetals found on the periodic table?
Metals – All elements to the left of the stair-step line (but not touching it) on the
periodic table. The two exceptions are Aluminum because it is touching the stair
step line but is a metal and Hydrogen because it is to the left but not a metal.
Nonmetals - All elements to the right of the stair-step line (but not touching it) on
the periodic table. The exception is Hydrogen because it is to the left but is a
nonmetal.
Semimetals – All elements touching the stair-step line with the exception of
aluminum.
How are ions formed? What are the two kinds of ions?
Ions are formed when an atom gains or loses one or more electrons. This results in
a net charge on the atom. Cations are positively charged ions resulting from a lost
electron – more protons than electrons left in the atom. Anions are negatively
charged ions resulting from gained electrons – more electrons than protons left in
the atom.