1.3. Ionization energy

Question 1

ionization energy

Answer 1

the E required to remove one e- from an isolated atom (in a gaseous state), measured in kJ

Question 2

Why does an element have to be in gaseous state to measure the Ei?

Answer 2

Because otherwise the E would be used to break the bonds between atoms, and we wouldn’t know which portion of it went to taking an e- away.

Question 3

Ei changes with:

Answer 3

1) the number of shells (how close is the e- rotating around te nucleus) - PERIOD
2) the attraction force of the nucleus (also decreasing the atom radius) - GROUP (no. of protons)

Question 4

Ei is ____ with the number of occupied shells in an atom, and ____ with the number of protons.

Answer 4

inverse proportional, proportional

Question 5

13th and 16th group - why does Ei drop?

Answer 5

13th - 1 e- in 4th shell, wants to be removed
16th - 4 e- in a p subshell - 1 wants to be removed so that the subshell is half-filled - when only 1 e- is in the orbital, the repulsion force is lesser (more stable atom)

Question 6

Jumps in Ei occur between removing the ___ e- of one shell and the ___ of the next one.

Answer 6

last, first

Question 7

Energy of electrons ___ with the shells, subshells and orbitals.

Answer 7

increases (because of centripetal force, radius increases)

Question 8

Electon configuration…

Answer 8

…describes the arrangement of electrons in atoms.

Question 9

valence electrons

Answer 9

• the outermost electrons in an atom, (with the potential to be) involved in the bonding process
• defined by the group of an element (1st group - 1e-, 13th group - 3 e-, 17th group - 7 e-)
• represented by Lewis dots by the element symbol

Question 10

In electronic configuration, number of the shell is defined by the ___, the subshell by the ___, and the number of electrons in the subshell by the ___.

Answer 10

period (of the element), area of PTE (in which the element is situated), the group (of the element)

Question 11

building up principle

Answer 11

/noble gas configuration - configuration of the closest n.g. with a lesser atomic no. and building subshells on that till we get to the element of interest

Question 12

types of orbitals

Answer 12

x, y, z

Question 13

according to the diagonal rule, the subshells are listed like this:

Answer 13

1s, 2s, 2p, 3s, 3p, 4s, 3d, 4p, 5s, 4d, 5p, 6s, 4f, 5d, 6p, 7s, 5f, 6d, 7p, 6f, 7d, 7f

Question 14

Which two transition metals are exceptions when it comes to electron configuration?

Answer 14

Cr (instead of 4s^2 3d^4, it has 4s^1 3d^5 - half filled - most stable)
Cu (instead of 4s^2 3d^9, it has 4s^1 3d^10 - half/completely filled)

Question 15

Only ___ first lose electrons from the s shell and then d.

Answer 15

transition metals (e.g. 4s lower Ei than 3d - further shell)

Question 16

The most stable state of silver is ___ because…

Answer 16

Ag+, it has e- configuration 5s^1 4d^10 and it wants to get rid of the one e- in the 5th shell.

Question 17

Greater emission of E results in ____, and the lower emission of E results in ___ light.

Answer 17

ultraviolet, infrared

Question 18

On an Ei/ionization number graph (atom losing e- one by one) the greatest jump of Ei is from ___ to ___ shell, then ___ to ___, and then ___.

Answer 18

its last, second to last, second to first, as usual by their energies (3-2, 4-3…)

Question 19

The y axis on the Ei/ionization number graph is never Ei but __ because…

Answer 19

logEi, the value of Ei is too small (difficult to graph).

Question 20

E =

Answer 20

hf = h(c/y) (y expressed in nm) (c=3*10^8 m/s)

Question 21

planck’s constant

Answer 21

h=6.63*10^-34 J