Topic 2 - Bonding & Structure Flashcards
Bonding and Structure
How are ions formed?
when electrons are transferred from one atom to another
What are simple ions?
Ions which have either lost or gained 1,2,3 electrons so they have a full outer shell
what do all elements in the same group have?
same number of outer electrons
What is an ionic bond?
it is the strong electrostatic attraction between two oppositely charged ions
What is electrostatic attraction?
it holds positive and negative ions together- it’s very strong
How do you get an ionic compound?
When oppositely charged ions form an ionic bond.
The total charge is 0
Two things that affects the strength of an ionic bond?
- Ionic charges-
greater the charge=stronger ionic bond=higher melting/boiling point - Small closely packed ions - stronger ionic bonding
what is an isoelectronic ion
ions of a different atom with the same number of electrons
(explains why atomic radius decreases across a period)
What is the structure of an ionic compound ?
giant ionic lattice
What are the physical properties of ionic bonding and explain them (4)
high melting point - ions held together by strong attraction
soluble in water but not non-polar - as particle are charged
don’t conduct electricity when solid - particles in fixed position ( when molten or dissolved particles free to move and carry charge )
brittle - trying to pull layers over each other create strong repulsion between same charge ions
Describe an experiment that gives evidence for the presence of charged particles
electrolyse green solution of copper (II) chromate (VI) on piece of wet filter paper
paper turns blue at cathode (negative electrode) - positive copper ions = blue
paper turns yellow at anode (positive electrode) - negative chromate ions = yellow
what is a covalent bond
the strong electrostatic attraction between a shared pair of electrons and two positive nuclei
what is ionic bonding
the bonds between a two oppositely charged ions
What does there need to be a balance of in a covalent bond
the attraction from the positive nuclei to the shared pair of electrons and the repulsion between the nuclei
what is bond length
the distance between the two nuclei in a covalent bond
what affects bond length
electron density - the higher it is, the higher the bond enthalpy and shorter the bond length
what is a dative covalent bond
one atom donates both electrons to a bond
how is a dative covalent shown (if not by the same dot/cross)
an arrow pointing away from ‘donor’ atom
what is the order of the strength electron pair repulsion
lone pair - lone pair
lone pair - bond pair
bond pair - bond pair
what is the shape of a molecule with 2 electron pairs around central atom (include name and bond angles)
linear molecules
180°
what is the shape of a molecule with 3 electron pairs around central atom (include name and bond angles)
- 3 bonding, 0 lone
trigonal planar
120° - 2 bonding, 1 lone
bent
119°
what is the shape of a molecule with 4 electron pairs around central atom (include name and bond angles)
- 4 bonding, 0 lone
tetrahedral
109.5° - 3 bonding, 1 lone
trigonal pyramidal
107° - 2 bonding, 2 lone
bent
104.5°
what is the shape of a molecule with 5 electron pairs around central atom (include name and bond angles)
- 5 bonding, 0 lone
trigonal bipyramidal
90° 120° - 4 bonding, 1 lone
seesaw
87° 102° - 3 bonding, 2 lone
distorted T
87.5°
what is the shape of a molecule with 6 electron pairs around central atom (include name and bond angles)
- 6 bonding, 0 lone
octahedral
90° - 5 bonding, 1 lone
square pyramidal
90° 81.9° - 4 bonding, 2 lone
90°
Why do metal have a giant structure?
1.Metals have delocalised electrons which makes them positive metal ion
2. Positive metal ions are electrostatically attracted to the delocalised electrons
3.layers of positive metal ions separated by layers of electrons
describe the structure and properties of graphite
each carbon bonded to 3 other carbons - layers of hexagonal rings
no covalent bond between layers and weak intermolecular forces
soft
slippery
can conduct electricity as one electron from each carbon atom is delocalised
describe the structure and properties of graphene (5)
one layer of graphite
conduct electricity
incredibly strong
transparent
light weight
what are the uses of graphite
electrode
lubricant
what are the uses of diamond
cutting tools
Are melting points of metals generally high or low and why?
-High because of strong metallic bonding
-More electrons strengthen the metallic bonding, which would make the melting point increase