Bonding Flashcards
Which intermolecular force is generally the strongest
Hydrogen bonds
define metallic bonding and its structure and bonding type
strong electrostatic attraction of positive metal ions surrounded by a sea of delocalised e-.
giant metallic lattice
STRONG metallic bonds
define covalent bonds and its structure and its bonding type
shared pair of e- between 2 atoms ,
macromolecular and simple molecular
strong covalent bonding
What is ionic bonding? (refer to structure and bonding)
Strong electrostatic attraction between positively charged metal ions and negatively charged non-metal ions.
Have a giant ionic lattice
Strong ionic bonding
what is a coordinate bond
shared pair of electron which come from the same atom, atom donates a pair of electrons to another shown by an arrow
define electronegativity
power of an atom to attract a pair of electrons in a COVALENT bond.
what is polarity
the difference in electronegativity, presented by delta - and delta +
what molecules are the Intermolecular force Permanent dipole dipole between
Polar molecules , asymmetrical
What is a dative covalent bond
A pair of electrons shared between two atoms where one atom has donated two electrons
In terms of structure and bonding explain why Calcium has a higher melting point than methane
Calcium has a metallic lattice and metallic bonding
Methane has simple molecular structure and intermolecular forces between molecules.
Metallic bonding in Ca is stronger than the IMF between CH4.
More energy is required to overcome the metallic bonds in Ca.
Why do ionic compounds have a high melting point? (3)
Strong electrostatic bonds
Between oppositely charged ions
Require a large amount of energy to break
What is the general trend n the melting and boiling points in Period 3
The general trend is that the melting and boiling points increase and then decrease as you move across Period 3 from left to right.
How does induced dipole-dipole arise?
Random movement of electrons in one molecule leads to an
Uneven distribution of electrons, creating a
Temporary dipole in one molecule. This
Induces a dipole in a neighboring molecule
Dipoles attract
How would you compare 2 metallic bonding atoms
Compare the charges of each atom from the group
Explain why the melting point of magnesium is higher than melting point of sodium (2)
-Mg2+ has a higher charge than Na+/
more delocalised electrons than Na
-Stronger attraction to delocalised sea of electrons / stronger metallic
bonding
