OBHB - Module 2.2 Flashcards
Define ‘atomic orbital’.
A region around the nucleus that can hold up to 2 electrons with opposite spins.
Define ‘average bond enthalpy’.
A measurement of the strength of a covalent bond.
Define ‘covalent bond’.
A strong electrostatic attraction between a shared pair of electrons and the nuclei of the bonded atoms.
Name the four types of sub-shell.
S, p, d, f
How many orbitals are there in an s sub-shell?
1
How many orbitals are there in a p sub-shell?
3
How many orbitals are there in a d sub-shell?
5
How many orbitals are there in an f sub-shell?
7
Name two exceptions to the order in which shells are filled.
Cu29 and Cr24
What is the end of Cr24’s electron configuration?
3d5 4s1
What is the end of Cu29’s electron configuration?
3d10 4s1
Give an example of a non-linear molecule.
H20
Give an example of a trigonal planar molecule.
BF3
Give an example of a pyramidal molecule.
NH3
Give an example of a tetrahedral molecule.
CH4
Give an example of an octahedral molecule.
SF6
Give an example of a linear molecule.
C02
What is the bond angle for non-linear molecules?
104.5
What is the bond angle for trigonal planar molecules?
120
What is the bond angle for pyramidal molecules?
107
What is the bond angle for tetrahedral molecules?
109.5
What is the bond angle for octahedral molecules?
90
What is the bond angle for linear molecules?
180
How many bonded pairs are there in non-linear molecules?
2
How many bonded pairs are there in trigonal planar molecules?
3
How many bonded pairs are there in pyramidal molecules?
3
How many bonded pairs are there in tetrahedral molecules?
4
How many bonded pairs are there in octahedral molecules?
6
How many bonded pairs are there in linear molecules?
2
How many lone pairs are there in non-linear molecules?
2
How many lone pairs are there in trigonal planar molecules?
0
How many lone pairs are there in pyramidal molecules?
1
How many lone pairs are there in tetrahedral molecules?
0
How many lone pairs are there in octahedral molecules?
0
How many lone pairs are there in linear molecules?
0
Define a ‘dative covalent bond’.
A bond in which both of the shared pair of electrons are supplied by only one of the bonding atoms.
Define an ‘expanded octet’.
When the outer shell has more than eight electrons.
Define ‘permanent dipole-dipole interactions’.
Forces which occur between neighbouring molecules with a permanent dipole.
Define ‘induced dipole-dipole interactions’.
Forces which occur when electrons moving randomly create a dipole and induce one in a neighbouring molecule.
Which three elements can form hydrogen bonds?
Oxygen, nitrogen, and fluorine.
What is the bond angle around the H atom in a hydrogen bond?
180
Around which atom is the 180 degree bond angle in a hydrogen bond?
Hydrogen
Are sodium, potassium, and ammonium salts soluble in water?
Yes
Are nitrates soluble in water?
Yes
Are chlorides soluble in water?
Mostly, yes
Are sulfates soluble in water?
Mostly, yes
Are silver and lead chlorides soluble in water?
No
Are lead, barium, and calcium sulfates soluble in water?
No
Are carbonates soluble in water?
Mostly, no
Are hydroxides soluble in water?
Mostly, no
Which carbonates are soluble?
Sodium , potassium, and ammonium
Which hydroxides are soluble?
Sodium , potassium, and ammonium
Which chlorides are insoluble?
Silver and lead
Which sulfates are insoluble?
Lead, barium, and calcium
What is electronegativity?
The ability of an atom to attract the bonding atoms in a covalent bond.
