When naming ionic compounds, when must you use parenthesis?
When there is more than one oxidation number--a transition metal which can form more than one type of ion. For example, iron (II) or iron (III)
100
When must you use parenthesis in writing a formula for an ionic bond?
When you need more than one of a polyatomic ion to balance the charge to electrically neutral
100
What does it mean if an electron is delocalized?
The electron is not associated with a single atom--rather could extend around several adjacent atoms. These electrons are free to move around.
100
When are ionic bonds able to conduct electricity?
When melted (in liquid state) or dissolved in a liquid. This way ions are free to move.
100
How many periods are there on the periodic table?
7
200
What is the difference between monatomic and polyatomic ions?
Monatomic ions are those which are made of only one type of atom--Polyatomic ions are those made of more than one type of atom, but only have one charge (ex) NH4 is made of nitrogen AND hydrogen, but have a charge of +1)
200
Write the formula for cadmium chlorite.
Cd(ClO2)2
200
How do the metal atoms become positively charged?
The atoms allow their electrons to roam freely between adjacent atoms--when this happens, a positive charge is induced.
200
Give 2 properties of ionic compounds.
Moderately high melting points and high boiling points, typically brittle and solid, good conductors when melted or allowed to dissolve in water, crystal
200
Which group of metals is the most reactive? Why?
The alkali metals--They are group one metals. Therefore, they only need to lose one electron to have a full outer energy level. This makes them extremely reactive.
300
Name the following compound: Ca(OH)2
calcium hydroxide
300
Write the formula for potassium dichromate
K2Cr2O7
300
Give 2 properties that occur due to the metal atom's electrons being able to roam freely.
good conductors of heat and electricity, malleable, reflect light (luster)
300
What is lattice structure?
3-d geometric shape showing the arrangement of atoms, molecules, or ions in a structure
300
What happens to atomic radius as you move across a period? Why?
Atomic radius is decreased. You are not moving up in energy levels, so electrons are not any further away from the nucleus--but the nucleus is getting more positively charged with each element moving right.
400
Name the following compound: Li3N
lithium nitride
400
Write the formula for sodium hydroxide
NaOH
400
Give 2 of the 3 groups of metals on the periodic table; not including lanthanides or actinides
Which would have a greater lattice energy: LiF or LiBr?
LiF--The bond is the strongest when the ions are small. Because F has less electrons than Br, the electrons are more attracted to the nucleus--so it takes more energy to get them away.
400
What happens to ionic radius as you move down a group?
The radius gets larger with the addition of protons and electrons.
500
Name the following compound: CuF2
copper (II) fluoride
500
Write the formula for manganese (II) phosphate
Mn3(PO4)2
500
Give 2 examples of why its important for metals to be malleable.
Jewelry, coins, weapons
500
Which would have a greater lattice energy: MgO or NaCl?
MgO--As the charge increases for the ions in an ionic bond, so does the lattice energy.
500
Without writing out the full electron configuration, what would you expect strontium's configuration to end in? Why?