2.2.2 Bonding And Structure Flashcards
What is ionic bonding
Electrostatic attraction between positive and negative ions
Ionic bonding occurs when?
Metal and non metal
Electrons are transferred from the metal to the non metal
Oppositely charged electrons attract through?
Electrostatic forces to become a giant ionic lattice
Example of giant ionic lattice
Sodium chloride
Ions with a grater charge will have a?
Charge-strength of the ionic bond
It will have a greater attraction and therefore stronger ionic bonding
Larger ions with a greater ionic radius will have?
A weaker attraction to the oppositely charged ion because the forces have to act over a greater distace
Type of bonding GIL and between what particles
Giant ionic lattice
Ionic and between oppositely charged ions
Positive and negative
Solubility
GIL
Soluble to polar substances
Conducts when solid? And why?
GIL
No because they are no mobile delocalised electrons
The ions are in fixed structure
Conducts when molten/dissolved and why?
GIL
Yes because the ions are now mobile
High or low melting/boiling points and why?
GIL
Yes high melting/boiling points because they are strong ionic bods which require energy to break
Examples?
GIL
NaCL
MgO
Giant covalent lattice
Types of bond and between what particles
GCL
Covalent bonding
Between atoms
Solubility?
GCL
Insoluble
Conducts when solid? And why? GCL
No because they are no mobile delocalised charged electrons
High melting/boiling points? and why? GCL
Yes high because there are strong covalent bonds and requires energy to break
Examples? GCL
Diamond and silicon dioxide
Giant metallic lattice
Types of bonds? And between what particle?
Metallic bonding and between positive and negative and delocalised electons
Solubility? GML
Insoluble
Conducts when solid?
And why? GML
Yes because there are mobile delocalised electrons
And it conducts when molten and dissolved
High or low melting/boiling points and why?GML
High melting and boiling points because strong metallic bonds so strong attractions so lost of energy is needed to break
Examples? GML
Nickel
Magnesium
Copper
Simple covalent bonds
Types of bonds and between what particles
Intermolecular forces and between molecules
Solubility? SCB
Polar substances dissolve polar substances
Non polar substances dissolve non polar substances
Conducts when solid? And why? SCB
No because there are not mobile charged particles
Conducts when molten/dissolved SCB
No because there are no mobile charged particles
High or low melting/boiling points and why? SCB
Low melting and boiling points because of weak intermolecular forces which require little energy to break
Examples? SCB
CO2
Group 7 of the periodic table
H20
What is a covalent bond
Strong electrostatic attraction between a shared pair of electrons
How do they form
Two nonmetals
Electrons are shared to gain a full outer shell
Enthaply changes?
The heat energy changes stored in a chemical system - H
(Triangle h)
electonegativity?
the degree of attraction by a bonded atom for a pair of electrons in a covalent bond
metallic bonding?
electrostatic attraction between a fixed lattice of a positive metal ions and a “sea of declocalised electrons”
properties of a metal?
good conductors of heat and electricity
high melting and boiling points
strong and durable
malleable
why can a metal conductor electricity?
mobile declosied electrons
why do metals have a high melting/boiling points?
they have strong metallic bonds so a strong attraction and require lots of energy to break
why are metals malleable
the layers of metal ions can slide over each other
general trend across periods for metals
melting points increase
more delocalised electrons
ions have a greater charge
ionic radius decrease so attraction between ions and electrons is stronger
polar?
dipoles don’t cancel out
non symmetrical
non polar?
no dipoles/dipoles cancel out
similar electronegativity
symmetrical
big four with large polarity
fluorine
oxygen
nitrogen
chorine
type of bond is permanent dipole dipole
polar bonds
explain permanent dipole dipole bonds
when two oppositely charged dipoles attract
