Chapter 5 Electrons and Bonding
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How are shell numbers and energy related? What is n?
As the shell number increases, the energy of the shell increases. The shell number is n, the principal quantum number
What are atomic orbitals?
Regions of space around the nucleus which can hold up to two electron of opposite spin
What are electrons?
Clouds of negative charge
What are shells made of? What are sub shells?
Shells are made of sub shells Sub shells are made of the same type of orbital grouped together, 3d sub shell contains 5 d orbitals
What is the shape of S orbitals? How many does each shell have?
Spherical shaped Each shell has 1 s orbital
What is the shape of the p orbital? How many p orbitals does each shell have?
Dumbbell shaped. One in the x, y, and z axis. After the second shell (inclusive of the second), each shell has 3 p orbitals
How many d and f orbitals does each shell have?
At the 3rd shell and above, each shell has 5 d orbitals each, with the d sub shell holding up to 10 electrons At the 4th shell and above, each shell has 7 orbitals each, with the f sub shell able to hold up to 14 electrons
How do orbitals fill?
The lowest energy orbital fills first. If a sub shell is present, meaning all orbitals are at the same energy level, each one is singly occupied first, before pairing begins
What is the sequence of orbitals filling?
1s, 2s, 2p, 3s, 3p, 4s, 3d, 4s, 4p
How is the electron configuration written? How does orbital filling relate?
In terms of sub shells, with the number of electron filled in superscript. Even though the 4s sub shell fills first, the 3d sub shell should be written before the 4s
How do sub shells empty? What is an important note about this rule?
Highest energy fills first The 4s sub shell empties first, as the 3d sub shell has a lower energy than the 4s when filled. This explains why most transition metals have at least a +2 ion
What is the electron configuration of Bromine? What is the shorthand configuration? Atomic number 35
1s2, 2s2, 2p6, 3s2, 3p6, 3d10, 4s2, 4p5 [Ar] 3d10, 4s2, 4p5
How do you write the shorthand configuration of electrons?
Find the noble gas for the element in question before it. Must be before. Write the noble gas in square brackets, continue the electron configuration from after the noble gas
What are the two exceptions to electron configuration and what is their configuration?
Chromium 1s2, 2s2, 2p6, 3s2, 3p6, 3d5, 4s1 Copper 1s2, 2s2, 2p6, 3s2, 3p6, 3d10, 4s1
Why is lithium called an s block element?
It’s highest energy electron/ sub shell is (in) the s orbital
Define ionic bonding
The strong electrostatic force of attraction between anions and cations
What is a giant ionic lattice?
Repeating, regular arrangement of oppositely charged ions, with the attraction in all directions
Why do ionic compounds have very high melting points? What factors affect the strength of an ionic compound?
Ionic compounds are in a giant ionic lattice. Lots of energy is needed to overcome the many ionic bonds, the strong electrostatic force of attraction between oppositely charged ions, giving a high boiling boing The great the charge of the ions, the greater the attraction between the ions, and the greater the melting point/ energy to overcome Also atom size
What happens when an ionic compound dissolves?
The ionic lattice breaks down. The water surrounds the ions The stronger the charges, the greater the ionic bonds, more energy needed to overcome, them, so lower solubility.
How is electrical conductivity differ with ionic compounds?
In solids, the oppositely charged ions are in fixed positions, unable to more and carry charge In aqueous / molten, the ions are free to move, so can move and carry charge, acting as mobile charge carriers, conducting electricity
What factor does solubility depend upon?
Whether the interactions between the solvent and ionic compound is greater than the strength of the ionic lattice
Define a covalent bond
The strong electrostatic force of attraction between a shared pair of electrons and the nuclei of the bonded atoms
Compare the location of attraction with ionic compounds and covalent bonds?
In ionic, the attraction is in all directions in 3 dimensions In covalent, the attraction is localised, based solely between the shared pair of electrons and the nuclei of the bonded atoms
How many covalent bonds can form?
Usually, the bonded atoms will aim to have the same electron configuration as the nearest noble gas There are exceptions, including expanding the octet, BF3 After period 3, inclusive, d sub shell becomes available so can form as many covalent bonds as the number of electrons in the outer shell