Bonding (16-20) (paper 1) Flashcards
What is a negative ion
an anion
What are simple ions
Atoms with a charge
what is a positive ion
a cation
Which groups lose electrons
1, 2, 3
which groups gain electrons
5, 6, 7
what is the formula for ammonium
NH4 +
what is the formula for hydroxide
OH -
what is the formula for nitrate
NO3 -
what is the formula for sulfide
S 2-
what is the formula for sulfate
SO4 2-
what is the formula for carbonate
CO3 2-
what is the formula for nitride
N 3-
what is the formula for hyrogen carbonate
HCO3 -
describe the transfer of electrons
- a metal and non-mental react together to gain full outer shells
- metal forms a positive ion and non-metal forms a negative ion
- the ions are strongly attracted by electrostatic attractions
What is the structure like on an ionic compound
they are closely packed in a 3D lattice arrangement
define ionic bonding
Electrostatic attraction betwenn positive and negative ions
What is the melting point like in an ionic bond
high because the strong bond needs a lot of energy to break
Can ionic bonds conduct
only when molten or dissolved in a solution so the ions can move to carry a charge
Define metallic bonding
electrostatic attraction between rows of metal cations and a sea of delocalised electrons
what is the melting point like in metallic bonding
High meling point because the bonds require lots of energy to break
Can metallic bonds conduct
Yes as a solid and liquid becuase the delocalised electrons can flow to carry a charge
Where are the bonds in covalent bonds
Covalent bonds between atoms and weak intermolecular forces between molecules
What is the melting point like in a covalent bond
Low melting point because the weak intermolecular forces require little energy to break
Do covalent bonds conduct
no becuase there are no free moving charged particles
Define covalent structures
electrostatic attraction between the pair of bonding electrons and bonded nuclei
What is the melting point like of giant covalent stuctures
very high melting poing becuase the strong covalent bonds require lots of energy to break
Do giant covalent structures conduct
no but graphite does because of its delocalised electrons
Why are metallic stuctures malleable
because the layer of positive ions slide
What are the three giant covalent structures
- diamond
- graphite
- sand
define the term malleable
the metal can be shaped
what is C60 fullerene
a simple molecular structure
desribe C60 fullerne molecules
hollow spheres make up of 60 carbon atoms
How is diamond made up
network of carbon atoms that form four covalent bonds
describe the formation of C60 fullerene
molecules are hollaw spheres made up of 60 carbon atom
how are the carbon atoms in C60 fullerene held togethere
intermolecular forces = can slide = soft
does C60 fullerene have a delocalised electron
yes
what is strange about the delocalised electron in C60 fullerene
it cannot move between the molecules so it is a poor conducter of electricity and heat
