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Inorganic Chapter 9
Terms in this set (14)
Explain the melting point trend for group 2 elements
Alkaline Metals: like the alkali metals (Group 1) MP decrease going down the group
Explain the melting point trend for group 17 elements
Halogens: like the Noble gases (Group 18) MP increases going down the group
Explain the trend for groups 13-16
The trends are based on the types of bonding:
Covalent: (increase down) higher melting points
Metallic: low melting points; depending on strength of bonds
Network Covalent: VERY high melting points
We observe systematic patterns in chemical formulas of the compounds formed by the elements. Partial trends in physical and chemical properties.
Second & Third Period
Increases then significantly decreases. Based on Bonding type
Fluorides with the 2nd and 3rd period
Diagonal bonding type pattern, i.e. Li and Mg both form ionic solids with fluorine. I, NC, C
Oxygen and hydride compounds follow this pattern as well.
*Various phases of C bonding
share the same total number of valence electrons and the same total sum electrons
have acidic and basic qualities
Group (n) and Group (n+10) similarities
Similarities in chemical formula and structures of the highest oxidation state of some members of the (n) group elements of the numbers corresponding (n+10) group elements.
Similarities between Al and Sc
Primary oxidation state: 3+ (acidic)
Mid to basic: Al(OH)3 (solid) and Sc(OH)3 (solid)
Very Basic: Al(OH)4- and Sc(OH)4-
1. +4 oxidation
2. +5 oxidation
Upper diagonal pattern in bonding
The Knight's move relationship
There is similarity between the Group (n) & Period (m) and Group (n+2) & Period (m+1) in the oxidation states. It is found in the lower right portion of the periodic table.
When trying to identify between two cations (Mg and Zn), What could you use to experimentally identify which on it is?
Add OH-. The group 2 elements for hydroxides with the compound. Many metals are amphoteric (Cu, Zn, Sn, Pb, Al, and Be), therefore with excess base, the compound will redissolve in solution, while the group 2 would stay a precipitate.
When trying to predict the highest element of another element (fluoride of iodide)....
Look at the size of the compound and determine how many bonds it can have.
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