Worksheet 3-3 Periodic Trends
What trend in electron affinity do you see as you go down a group/family on the periodic table? What causes this trend?
Decreases as you go down because electron configurations.
What trend in ionization energy do you see as you go down a group/family on the periodic table? What causes this trend?
Decreases as you go down because the valance electrons are further from the nucleus
What trend in electronegativity do you see as you go down a group/family on the periodic table? What causes this trend?
Decreases as you go down, because valance electrons are further from the nucleus
What trend in atomic radius do you see as you go across a period/row on the periodic table? What causes this trend?
Decreases to the left due to increasing positive changes in nucleus
What trend in electron affinity do you see as you go across a period/row on the periodic table? What causes this trend?
Electron affinity increases as you go to the right because because there are more protons in the atoms.
What trend in electronegativity do you see as you go across a period/row on the periodic table? What causes this trend?
Electronegativity increases as you go to the right, because atoms would rather gain electrons to have a full shell.
Discuss the importance of Mendeleev's Periodic Law.
He arranged elements by atomic mass and noticed repeating trends
What trend in atomic radium do you see as you go down a group/family on the periodic table? What causes this trend?
Increasing as it goes down because the increasing energy levels
What trend in ionization energy do you see as you go across a period/row on the periodic table? What causes this trend?
Ionization energy increases as you go to the right, because greater positive charge leads to greater attraction of the electrons.
Is it easier to form a positive ion with an element that has a high ionization energy or an element that has a low ionization energy? explain.
Low ionization energy because they want to get rid of on electron to have a full valance shell
Use the concept of ionization energy to explain why sodium form a 1+ ion (Na+) but magnesium forms a 2+ ion (Mg2+)
Sodium has a low 1st ionization energy because it has 1 valance electron magnesium as a low 2nd ionization energy because it has 2 valance electrons
Define Ionization energy
The energy required to remove an electron form a neutral atom
Circle the atom in each pair that has the largest atomic radius: a) Al B b) S O c) Br Cl d) Na Al e) O F f) Mg Ca
a) Al b) S c) Br d) Na e) O f) Ca
Circle the atoms in each pair that has the greater ionization energy: a) Li Be b) Na K c) Cl Si d) Ca Ba e) P Ar f) Li K
a) Be b) Na c) Cl d) Ca e) Ar f) Li
Circle the atom in each pair that has the greatest electronegativity: a) Ca Ga b) Li O c) Cl S d) Br As e) Ba Sr f) O S
a) Ga b) O c) Cl d) Br e) Sr f) O
Give two examples of elements for each category a) noble gases b) halogens c) alkali metals d) alkaline earth metals
a) helium, neon, argon. krypton, xenon, or radon b) fluorine, chlorine, bromine, iodine, or astatine c) lithium, sodium, potassium, rubidium, cesium, or francium d) beryllium, magnesium, calcium, strontium, barium, or radium
Identify each element as a metal, metalloid, or nonmetal. a) fluorine b) germanium c) zinc d) phosphorus e) lithium
a) nonmetal b) metalloid c) metal d) nonmetal e) metal
Define electronegativity
the ability of an atom to remove an electron from another neutral atom
Define electron affinity
the energy change that occurs when a neutral atom gains an electron
