Periodic Table
Metallic Bonds
and Molecular Geometry
and Molecular Geometry
Ionic Bonds
Covalent Bonds
Polarity
100
The amount of valence electrons used to make a single bond
What is 2 electrons?
100
In metallic bonds you combine what types of elements
Metal and a Metal
(two or more metals)
100
Type of elements that forms an ionic bond
metal/nonmetal
100
When an electron is attracted to the nuclei of two or more non metals atoms at the same time
What is a covalent bond?
100
Electronegativity is
The attraction that electrons experience to bond
200
The group that has two valence electrons?
What is group 2?
200
Metallic bonds are considered to float in a sea of electrons and are usually delocialized. Delocialized means
Free electrons (constantly in motion)
200
In ionic bonds electrons are
Transferred
200
the overall charge of a particle that is covalently bonded
What is neutral?
200
The DEN of a molecule represents
The difference in electronegativity
300
The group that has a full outer shell
What are the noble gases?
300
Is KCl a good example of a metallic bond?
No, this bond is ionic
300
Group 1 elements can form an ion of ______ to become an ion
+1
300
The particle formed when atoms share electrons
What is a molecule?
300
The DEN for NO2
0.4
400
the number of electrons in bromine's outer shell
What is 7?
400
What makes the molecular geometry of trigonal planar and pyramidal different ?
Pyramid central atom has lone pairs
Trigonal Planar does not
400
The element K (potassium) can form an ion of ______ to bind with Cl.
+1
400
When a atom shares two electrons with another atom
What is a double bond?
400
What makes a molecule non polar
DEN is less then 5
500
The number of valence electrons in the found in H (Hydrogen)
1
500
Molecular or Structural or Lewis Dot of NH3
Answers may vary
500
Element that can form an ionic compound when reacted with S.
Any elements from group 2
or 2 elements from group 1
500
Construct the molecular formula for As2.
Should have a tripe bond and two lone pairs
500
These diagrams indicate
The pull of electrons. The partial negative demonstrates the strong pull