atomic structure

Question 1

when writing ionic equations what state does an ionic compound have to be to be split apart?

Answer 1

aq

Question 2

in electron impact ionisation, the m/z ratio of each peak is….
in electron spray ionisation, the m/z ratio of each peak is… AND why?
what do the number of peaks determine in a mass spectrum graph?
what does the height of the peaks determine?

Answer 2

• equal to the relative mass of THE isotope
• one unit greater than the relative mass of the isotope because we’re adding an H+ ion to each particle which increases the mass number
• the number of isotopes
• the relative abundance

Question 3

why do isotopes have similar chemical properties?
what is a mass spectrometer used for?
why does it need to be under a vacuum?
what type of elements and substances is electron impact used for?
what can electron impact do to large organic molecules?

Answer 3

• because they have the same electronic structure
• to determine all the isotopes present in a sample of an element and therefore identify an element
• otherwise air particles will ionise and register ON the detector
• ones with a low formula mass
• cause them to fragment

Question 4

what’s the deal with Cr and Cu? (coraline movie)
what does this in turn give (3 points perhaps)
what’s the rule with ionised transition elements - electrons is removed from _____ then _______
a half filled 3d ORBITAL is ________ in energy than a paired electron in the 4s orbital

Answer 4

• one electron jumps from the 4s to the 3d
• it gives a stable, half filled d subshell
• electrons is being removed from the 4s first then the 3d
• lower in energy

Question 5

what is the definition of ionisation?
when writing ionisation equations what side do we put the electron (the +e- part)
what sort of state symbols do we HAVE to remember to add to ionisation equation?
what are we doing in the 1st ionisation energy?
how does the definition for ionisation change when it comes to the 2nd ionisation energy: amount of energy required to move 1 mole of electrons from 1 mole of _____ in gaseous state
what is the trend for ionisation energy generally down the group?
why?
what also comes into play when it is DOWN the group (always goes hand in hand with atomic radius
what is the trend for ionisation energy generally across the group?
why?
what is shielding?
the more inner electrons there are…. the ______ shielding
how does shielding affect ionisation energy (long winded answer)
what are the 3 factors of ionisation energy?

Answer 5

• amount of energy required to REMOVE 1 mole of electrons from 1 mole of atoms in gaseous state
• right hand side
• gaseous
• we’re removing the 1st electron from the outer shell
• IONS
• decreases
• the atoms get bigger and so there’s a bigger atomic radius and so the amount of energy required to remove the outer electron decreases
• greater shielding
• increases
• the number of protons increases meaning there’s a greater/bigger attractive force between the outer electron and the positive charge in the middle
• the effect the inner electrons have on the ability to remove the outer electron
• greater
• less amount of energy required to remove outer electron thus lowers/decreases ionisation energy
• number of protons (effective nuclear charge italian man)
• atomic radius/distance from NUCLEUS
• shielding

Question 6

what does a large increase in IE data actually MEAN or show?
why is there a gradual increase with these succesive ionisation energies (3 points)

Answer 6

• it shows that there’s been a removal of an electron closer to the nucleus
• we’re creating a more positive ion
• there are more protons than electrons due to electron loss
• strong attraction between remaining electrons

Question 7

MUST KNOW QUESTIONS:
why is there a small drop from Mg to Al?
why is there a small drop from P to S?

Answer 7

• Al is starting to fill out a 3p subshell. Mg has its outer electrons in the 3s sub shell. The electrons in the 3p subshell are easier to remove as the 3p electrons are higher in energy. They’re ALSO SHIELDED BY THE 3S ELECTRONS.
• sulfur has 4 electrons in the 3p subshell with 2 electrons in the first 3p orbital. there is repulsion occuring in the first 3p orbital with the two negatively charged electrons repulsing each other meaning that the second electron will be easier to remove (spin pair repulsion)

Question 8

what is relative atomic mass (Ar)?

Answer 8

the average mass of an atom of an element measured on scale ON WHICH the mass of an atom of 12C is exactly 12

Question 9

random notes:
- shielding is similar when it comes to looking at how ionisation energy increases across the period