chemistry quiz oct 10th on periodic trends

what determines the properties of elements in periodic trends

valence electrons

what is the first concept that explains periodic trends

opposite charges attract: the positively charged nucleus attracts electrons to itself. This fundamental attraction influences atomic size, ionization energy, and electronegativity.

what is the second concept that explains periodic trends

like charges repel: electrons repel each other and organize themselves to minimize said repulsion. includes afbaus rule, hunds rule, and pauli exclusion principle

what is the third concept that explains periodic trends

more energy levels results in more sheilding

what is shielding

the blocking of nuclear charge (charge of nucleus) from reaching and attracting the valence electron and shell due to more energy levels

what is atomic radii

distance from nucleus to outermost electron

what happens to the atomic radii as you go across a period

the atomic radii decreases

why does atomic radii decrease as you go across a period

increased nuclear charge pulls valence electrons closer to the nucleus, reducing atomic radii

what happens to the atomic radii as you go down a group

it increases

why does the atomic radii increase as you move down a group

because as you move down a group the outermost orbitals size increases, shielding valence electrons from nucleuses pull, and overpowering the increased pull of the positive nucleus on valence electrons, so atomic radii increases

does more protons make atom smaller or bigger

smaller because it pulls the electrons in better

what does isoelectric mean

if the atoms we are comparing have the same number of electrons and configuration

which has a greater effect: shielding or nuclear charge

more shielding has a greater effect than more nuclear charge

what are cations

positive ions formed by losing electrons

are cations bigger or smaller than their atoms

smaller because they have the same nuclear charge but less electrons to pull in and less energy levels

what are anions

negative ions, formed by gaining electrons with ide endings (nonmetals)

are anions bigger or smaller than their atoms

the atom is smaller than the anion because they have the same nuclear charge but less electrons to pull in 

what are the 3 most stable orientations in order

1) p^6 filled

2) filled sublevel 
3) a half filled sublevel

what is ionization energy

the energy required to remove an electron from an atom in its gaseous state 

what does ionization energy dictate

how strongly atoms nucleus hold onto valence electrons

what does a high ionization energy result in

atom has a strong hold on the electrons, making it hard to remove them and requiring more energy

what does a low ionization energy result in

atom has a weak hold on electrons, making it easy to remove them and requiring less energy

what happens to ionization energy as you go across a period

it increases, but the shielding stays consistent whilst atoms get smaller

why does ionization energy increase as you go across a period

because increased nuclear charge of each successive element makes increased hold on valence electrons (since stronger NC=harder to remove valence electrons as electrons pulled closer to positive nucleus)

what happens to ionization energy as you move down a group

it decreases

why does ionization energy decrease as you move down a group 

because the increasing atomic size pushes valence electrons away from the nucleus, so it takes less energy to remove the electron since strength of attraction is less

what is successive ionization energy

removal of the 2nd, 3rd, 4th, etc. electrons from a species

what happens to the successive ionization energy as you move across a period

you need more energy for each one, the amount needed increases because the increase of positive charge binds electrons stronger

when does the energy jump occur

when core electrons are being removed instead of valence electrons because it takes more energy to break up stable electrons

why do cations get smaller and smaller the more electrons you lose

more nuclear charge, less electrons means it pulls them in better

what is electronegativity

ability of an atom in a molecule to attract shared electrons when forming a chemical bond

what happens to electronegativity when you go across periods

increases because increasing nuclear charge as protons increase also increase electron attracting power

what happens to electronegativity as you go down a group

it decreases because of shielding. the electrons in lower energy levels shield the positive charge of the nucleus from outer electrons, decreasing electron attracting power and outer electrons wotn be tightly bound to the atom

which types of elements dont have electronegaitvity

noble gases bc full shell and stable so they dont want to attract eelctrons when bonding