ionic bonding (checklist) Flashcards
an ion is
an electrically charged atom or group of atoms formed by the loss or gain of electrons
why do ions need to lose or gain electrons
to obtain a full outer shell of electrons
Negative ions are called
anions
anions form when
atoms gain electrons, meaning they have more electrons than protons
positive ions are called
cations
cations form when
atoms lose electrons, meaning they have more protons than electrons
all metals lose or gain electrons to become positively charged ions ?
lose
all non metals ____ electrons to become negatively chraged ions
gain
Elements in Group 1 form ions with a ___charge
1+
Elements in Group 2 form ions with a ___charge
2+
Elements in Group 6 form ions with a ___ charge
2-
silver is
Ag +
copper is
Cu2+
iron is
Fe 2+
Lead is
Fe2+
Zinc
Zn2+
Hydrogen
H+
Ammonium
NH4+
Hydroxide
OH-
Nitrate
NO3-
Carbonate
CO₃²+
Sulfate
SO₄²-
what is an ionic bond in terms of electrostatic attractions
electrostatic attraction between oppositely charged ions
ionic compounds form
giant ionic lattices
giant ionic lattices are made up of
many oppositely charged ions held together by strong electrostatic attractions
why do giant ionic lattices have a high melting and boiling point
because it takes a lot of energy to break the electrostatic attraction, or the bonds holding them together
why do solid ionic compounds not conduct electricity
because there are no free electrons or ions that can move so cannot conduct electricity
when can ionic compounds conduct electricity
when molten or in an aqueous solution
why can giant ionic lattices conduct electricity when molten
because the ions are free to move and so can carry charge
The lattices formed by ionic compounds
consist of a regular arrangement of alternating positive and negative ions
Ionic compounds are poor conductors in the solid state because (2)
The ions are in fixed positions in the lattice
They are therefore unable to move and carry a charge
Ionic compounds are good conductors of electricity in the molten state or in solution because
When the ionic compound is melted or dissolved in water, the ions are able to move and carry a charge
simple molecular structures have low melting and boiling points because
the weak intermolecular forces are easily overcome and take only a small amount of energy to break.
As the relative molecular mass of a simple molecular structure increases so does the melting point/boiling point because
The weak intermolecular forces are stronger in larger molecules because they have more electrons.
a giant covalent structure is a ( state) and has ___ melting and boiling point
solid
high
most covalently bonded substances form
simple molecular structures
when you melt or boil giant covalent structures, what need to be broken
the strong covalent bonds
properties of diamond (3)
- very hard (made of strong covalent bonds so hard)
- cannot conduct electricity because there are no free electrons
- high melting and boiling point
properties of graphite
- high melting and boiling point as it has layers of carbon atoms covalently bonded together
- weak intermolecular forces between the layers so the layers can move past each other making it soft and slippery
- has a sea of delocalised electrons so can conduct electricity
is diamond a giant covLENT STRUCTURE
yes
is C60Fullerene a giant covalent structure
yes
properties of c60fullerene
- low melting and boiling point because there are weak intermolecular forces between each molecule.
- This also makes it soft.
- It has delocalised electrons that are free to move around the structure so can conduct electricity
do giant covalent structures usually conduct electricity
no
