electrons and ionisation energy

what is the definition of an electron shell?

an electron shell is a group of atomic orbitals with the same principle quantum number representing the main energy level of an atom

what is the definition of a sub shell?

a sub shell is a group of orbitals within a shell that are the same type and energy

what is the definition of orbitals

an orbital is a region of space around the nucleus that can hold up to two electrons with opposite spins

what is an electrons cloud

an electron cloud is a region around the nucleus where electrons are likely to be found based on the probability distribution of their orbitals

what is the quantum number

the principle quantum number indicates the shell or main energy level in which an electron is found and its relative distance from the nucleus

What is an electron spin?

the clockwise or counterclockwise motion of an electron

what do the numbers 1,3,5 and 7 indicate

the number of orbitals in each type of sub shell

how many orbitals does a s sub shell hold

1

how many electrons does an s orbital hold?

max of 2

how many s orbitals does anything above n=1 hold?

1

what changes as the Principe quntium number increases in s orbitals?

the greater the shell number the greater the radius of the s orbital

what shape is an s orbital

spherical

What shape is the p orbital?

dumbell

What is the Aufbau principle?

electrons occupy the orbitals of lowest energy first

how many electron orbitals does a p sub shell contain

3

what is different about the potion of each different p sub shell in an orbital

they are all at right angles to each other, either on the x y or z axis

how many p orbitals are from n=2

3 orbitals

how many d orbitals are there from n=3?

5 orbitals

how many f orbitals are there from n=5

7 orbitals

what is the way to calculate the maximum number of electrons that can fit in a shell

2n^2

what is different between the different types of sub shells

within the same shell sub shells have different energies

which sub shell has the least amount of energy and what does that mean

the s sub shell has the least amount of energy which means it is filled first - aufbaus principle

what is an acceptation to the energy sub shell rule

the 4s sub shell is filled before the 3d sub shell as it has slightly lower energy

what does the electron in box model represent

it represents the orbitals as boxes

what does each each box in the electron box model represent

the orbital

what do the half arrows in the electron box model represent

an individual electron

what is the same amount orbitals int he same energy level

orbitals have the same energy

why does one electron occupy one orbital before electron pairing starts

prevents any repulsion between paired electron before there is no further orbital available at the same energy level

what is the definition of ionisation energy

measures how easily an atom loses electrons to form a positive ion

what is the first ionisation energy definition?

the energy requires to remove one electron from each atom in one mol of gaseous atoms of an element to form of mol of gaseous 1+ ion.

what are the three factors that effect the attraction between the nucleus and the outmost electron

atomic radius, nuclear charge, electron shielding

what does atomic radius refer to?

The greater the distance between the nucleus and the outer electron, the less the nuclear attraction. The force of attraction falls off sharply with increasing distance

what does nuclear charge refer to?

The more protons there are in the nucleus of an atom, the greater the attraction between the nucleus and the outer electron

electron shielding

electrons are negatively charged and so inner electrons repels outer shell electrons. This repulsion is called the shielding effect and it reduces the traction between the nucleus and the outer electrons

how many ionisation energies does an element have

As many as there are electrons

what happens after the first electron is lost

after the first electron is lost the remaining electrons are pulled closer to the nuclei's and there is higher nuclear attraction which causes the ionisation energy for the remaining electrons to increase

what is second ionisation energy

the energy needed to remove one electron from each ion in one mole of gaseous 1+ ions of an element to form gaseuous 2+ ions

what happens to first ionisation energies across the first three periods

it increases

what happens to ionisation energies down a group

they descreace