Metals Flashcards
What is Aufbau’s principle?
orbitals of lower energy get filled first
What is Pauli’s exclusion principle
the maximum number of electrons per orbital is 2 and no two electrons in an atom or ion can have the same four quantum numbers
What is Hund’s rule
When filling degenerate orbitals put one electron in each of the degenerate orbitals before pairing electrons
e- come out the shell with the largest ____ ____ first
n value
could also say with the highest principle quantum number
Name 6 general properties of metals
- Conductive of heat and energy
- malleable
- Ductile
- shiny
- hard (Na and Hg exceptions)
- high melting and boiling points
What is ionization energy?
the energy required to remove an electron from the gaseous atom or ion
Why is ionization energy low in metals?
electrons are already mobile within the metal and so can be removed from the structure easily
Metals are made up of…?
closely packed metal cations in “a sea of electrons”
In metals e- are ___ throughout the _____
delocalized
lattice
Can you isolate ions?
no
Are ions compounds?
no
Cations are ____ than the atoms from which they
are formed
smaller
Define isoelectronic
species have the same number of electrons in identical configurations
For isoelectronic cations, the more positive the ionic charge, the ____ the ionic radius.
smaller
Anions are ___ than the atoms from which they are formed.
larger
For isoelectronic anions, the more negative the charge, the ____ the ionic radius.
larger
Ionic bonding results from the reaction of an atom with ____ ionization energy with an atom of ____ electron affinity
low
high
in covalent bonds atoms ____
overlap
In metallic bonds, ____ ____ are lost and gained
valance electrons
e- jump from one atom to another
What is the structure of an MX compound?
metal cations packed with anions into an ionic lattice
In MX what do the M and X stand for?
M is for metal
X is for halogen
Lattice energy is the energy required to ….?
separate the ions
Name 4 properties of MX compounds
- hard and brittle
- high melting point
- dissolve in polar (ionizing) solvents
- do not conduct electricity as solids but do conduct electricity in molten or solution form
why does the size of M and M+ increase down the group?
More shells as you go down
Why does IE decrease moving down a metal group?
Because the size of the orbitals increase moving down a column making the valance e- easier to remove
Metals become more ____ moving down a column
metallic
Why do metals become more metallic moving down a column?
Because the valance e- are easier to remove because the atoms are larger
What is ionic potential?
the ratio of metal cation charge (Z) to ionic radius (r) (ie Z/r)
Ionic potential measures the ability to ____
polarize
The smaller the metal cation and the ___ its charge density, the ___ it will polarize the electron cloud of the anion
higher
more
IP (ionic potential) or Polarizing ability ____ down a group
decreases
Why is NaCl water soluble when AgCl is not?
Na+ has noble gas configuration but Ag+ has 5s and 4d orbitals which are closer in energy and this results in more polarizing effect so the AgCl salt is hard to dissolve
Are most MX compounds water soluble?
yes
Do anions polarize cations or do cations polarize anions?
Cations polarize anions
The anion that has more ___ and a ___ volume is more likely to get polarized
electrons
larger
Cations with the noble-gas electronic configurations are ___ polarizing than those with non-noble gas electronic configurations
less
The cation with the larger charge density is __ likely to polarize an anion
more
What are the group 1 metals called?
alkali metals
The ionization energy of the alkali metals ____ down the group
decreases
Are alkali metals (group 1) dense?
no they are low density metals
Why is the metallic bonding of group 1/alkali metals weak?
because only one valance e- contributes to metallic bonding
Why are group1/alkali earth metals not very dense?
Because they have very weak metallic bonding which is cause by there only be one valance e- per atom to contribute to metallic bonding
The reactivity of metal _____ down a group
increases
The reaction between an group1/alkali metal and water results in….?
an alkaline solution of a metal hydroxide
What alkali earth metal can be used for carbon dioxide scrubbing?
Na in NaOH
Which are more reactive alkali/group 1 metals or alkaline earth/group 2 metals?
Alkali/group 1 metals
Group 1 metals have ____(lower/higher) melting points than group 2 metals
higher
Why do group 2 metals have higher melting points than group 1 metals?
Because group 2 metals have more valance e- to contribute to metallic bonding
Do ionic compounds containing group 1 or group 2 metals have lower solubility in water?
ionic compounds containing group 2 metals have a lower solubility in water
Why do ionic compounds containing group 2 metals have lower solubility in water than group 1 metals?
group 2 metals have a stronger cation-anion interactions (ie stronger metallic bonding)
Are lattices of ions with similar or dissimilar charge densities more stable?
similar
Why are group 2/alkaline earth metals less reactive than group 1/alkali metals?
Because for group 2/alkaline earth metals to reach noble gas configuration the must lose 2 e- not just one. (Have to overcome 2 IE)
Group 2 metals have higher melting points than group 1 metals with one exception. Which metal is the one exception?
Magnesium
What is the layer that forms on group 2 metals that stop the reaction with water from continuing called?
a metaloxide layer
The ____ (lower/higher) the charge density the more polarizing the cation
higher
Which group 1 metals can react with unlimited oxygen supply to form oxides?
all group 1 metals
Which group 1 metals can react with unlimited oxygen supply to form peroxides?
all group 1 metals except lithium (Li)
Which group 1 metals can react with unlimited oxygen supply to form superoxides?
all group 1 metals except lithium (Li) and Sodium (Na)
ie from Potassium (K) down forms superoxides
