Flashcards Chemistry Periodic Trends: Atomic Radius, Ionization Energy & Reactivity
Call Kai
Learn
Practice Test
Spaced Repetition
Match
Flashcards
Knowt Play1/140
There's no tags or description
Looks like no tags are added yet.
141 Terms
What is an ion?
An atom or molecule that has gained or lost one or more electrons, resulting in a net electrical charge.
What is a cation?
A positively charged ion formed when an atom loses one or more electrons.
What is an anion?
A negatively charged ion formed when an atom gains one or more electrons.
What is a covalent bond?
A chemical bond formed by the sharing of electron pairs between atoms.
What is an ionic bond?
A chemical bond formed through the electrostatic attraction between oppositely charged ions.
What is ionization energy?
The energy required to remove an electron from an atom or ion in its gaseous state.
What is the ionization trend across a period?
Generally increases due to increasing nuclear charge.
What is the ionization trend down a group?
Generally decreases due to increased distance from the nucleus and electron shielding.
What is electronegativity?
A measure of an atom's ability to attract and hold onto electrons in a chemical bond.
Which element is the most electronegative?
Fluorine.
What is the trend for electronegativity across a period?
Increases across a period.
What is the trend for electronegativity down a group?
Decreases down a group.
How does reactivity for metals change down a group?
Increases down a group due to lower ionization energy.
How does reactivity for nonmetals change up a group?
Increases up a group.
What is atomic radius?
The distance from the nucleus of an atom to the outermost shell of electrons.
What is the trend for atomic radius down a group?
Increases down a group.
What is the trend for atomic radius across a period?
Decreases across a period.
What is ionic radius?
The radius of an ion in a crystal lattice.
Are cations larger or smaller than their original atoms?
Smaller, because they lose electrons.
Are anions larger or smaller than their original atoms?
Larger, because they gain electrons.
Why are cations smaller?
Losing electrons reduces repulsion and sometimes removes an energy level.
Why are anions larger?
More electrons create greater repulsion.
What does ionization energy measure?
Energy needed to remove an electron from an atom.
What is the trend for ionization energy across a period?
Increases across a period.
What is the trend for ionization energy down a group?
Decreases down a group.
Which element has the lowest ionization energy?
Francium (Fr).
Which element has the highest ionization energy?
Helium (He).
Rank Li, C, F by increasing atomic radius.
F < C < Li.
Rank Li, Na, K by increasing atomic radius.
Li < Na < K.
Rank Ge, P, O by increasing atomic radius.
O < P < Ge.
Rank C, N, Al by increasing atomic radius.
N < C < Al.
Rank Al, Cl, Ga by increasing atomic radius.
Cl < Al < Ga.
Which is larger: Mg2+ or Mg?
Mg.
Which is larger: N3- or N?
N3-.
Which is larger: K+ or Fr+?
Fr+.
Which is larger: O2- or N3-?
N3-.
Which is larger: F- or F?
F-.
What is the largest cation?
Fr+.
What is the smallest cation?
H+.
What is the largest anion on this review?
Te2-.
What is the smallest anion on this review?
F-.
Rank Mg, Si, S by increasing ionization energy.
Mg < Si < S.
What is the atomic symbol for Helium?
He
Rank Mg, Ca, Ba by increasing ionization energy.
Ba < Ca < Mg
Rank F, Cl, Br by increasing ionization energy.
Br < Cl < F
Rank Ca, Cu, Kr by increasing ionization energy.
Ca < Cu < Kr
Rank C, Si, Sn by increasing ionization energy.
Sn < Si < C
What does electronegativity measure?
An atom's ability to attract shared electrons.
Which direction does electronegativity increase?
Up and to the right.
Which element has the highest electronegativity?
Fluorine (F).
Which element has the lowest electronegativity?
Francium (Fr).
Do noble gases usually have electronegativity values?
Usually no. Their outer energy levels are full.
Rank Li, C, N by increasing electronegativity.
Li < C < N
Rank C, O, Ne by increasing electronegativity.
C < O; Ne has no standard value.
Rank C, Si, Pb by increasing electronegativity.
Si < Pb < C
Rank Cs, Ni, F by increasing electronegativity.
Cs < Ni < F
Rank S, F, He by increasing electronegativity.
S < F; He has no standard value.
Why are metals less electronegative than nonmetals?
Metals tend to lose electrons instead of attracting them.
What are metallic properties?
Shiny, malleable, ductile, good conductors, usually lose electrons.
Which direction do metallic properties increase?
Down and to the left.
Which element is least metallic?
Helium (He).
Which element is most metallic?
Francium (Fr).
Rank Li, B, N by increasing metallic properties.
N < B < Li
Rank Li, Na, K by increasing metallic properties.
Li < Na < K
Rank Si, P, S by increasing metallic properties.
S < P < Si
Rank Pb, Po, Rn by increasing metallic properties.
Rn < Po < Pb
Rank Ra, Sr, Mg by increasing metallic properties.
Mg < Sr < Ra
What is the shielding effect?
Inner electrons block some nuclear attraction from outer electrons.
What happens to shielding across a period?
It stays about the same.
Why is shielding nearly constant across a period?
Electrons are added to the same main energy level.
Why does shielding increase down a group?
More occupied energy levels are added.
Which elements have the most shielding?
Elements near the bottom of the periodic table.
Which elements have the least shielding?
Elements near the top of the periodic table.
What direction does shielding increase?
Down a group.
What does it mean for a metal to be reactive?
It easily loses electrons.
What does it mean for a nonmetal to be reactive?
It easily gains electrons.
Which direction does metal reactivity increase?
Down and to the left.
Which direction does nonmetal reactivity increase?
Up and to the right, excluding noble gases.
Rank N, O, F by increasing nonmetal reactivity.
N < O < F
Rank Li, Na, K by increasing metal reactivity.
Li < Na < K
Rank P, S, Cl by increasing nonmetal reactivity.
P < S < Cl
Rank Pb, Po, Rn by increasing metal reactivity.
Rn < Po < Pb
Rank He, I, F by increasing nonmetal reactivity.
He < I < F
What determines an element's chemical properties?
Number of valence electrons.
What are valence electrons?
Electrons in the outermost energy level.
How many valence electrons do Group 1 elements have?
1
How many valence electrons do Group 2 elements have?
2
How many valence electrons do Group 13 elements have?
3
How many valence electrons do Group 14 elements have?
4
How many valence electrons do Group 15 elements have?
5
How many valence electrons do Group 16 elements have?
6
How many valence electrons do Group 17 elements have?
7
How many valence electrons do Group 18 elements have?
8, except He which has 2.
What is the common charge of Group 1 ions?
+1
What is the common charge of Group 2 ions?
+2
What is the common charge of Group 13 ions?
+3
What is the common charge of Group 15 ions?
-3
What is the common charge of Group 16 ions?
-2
What is the common charge of Group 17 ions?
-1
What is the common charge of Group 18 ions?
0