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Chemistry Periodic Trends
Terms in this set (20)
a) K e)Br
b)Ca f) Ba
c)Ga g) Si
d) C h)Au
Which atom in each pair has the larger atomic radius?
a) Li or K e)Cl or Br
b)Ca or Ni f) Be or Ba
c)Ga or B g)Si or S
d)O or C h)Fe or Au
Top to bottom = increases due to adding energy levels
Left to right = decreases
What is the periodic trend for atomic size from top to bottom and from left to right?
The force of attraction is stronger due to increased nuclear charge and no shielding
Why do atoms get smaller as you move left to right in a period?
Each time you go down a group, you add an energy level. More energy levels take up more space
Why do atoms get larger as you move down a group?
Ar, P, Si, Mg, Na
Arrange the following in order of increasing atomic radius:
Mg, Na, P, Si, Ar
An atom with a charge (it has gained or lost electrons)
cation is a positive ion(it lost electrons)
anion is a negative ion (it gained electrons)
What is the difference between a cation and an anion?
1. cations (positive ions) are smaller than the neutral parent atoms. They have lost electrons and sometimes lose energy levels. (decreased distance=more attraction to the nucleus)
2. anions (negative ions) are larger than their neutral parent atoms. More electron repulsions = less attraction to the nucleus
Explain the relationship between the relative size of an ion to its neutral atom and the charge of the ions.
Which particle has the larger radius in each atom/ion pair?
b)S,S2- d) Al,Al3+
Which of the following is an isoelectronic series?
Arrange the following isoelectric series in order from smallest to largest radius.
ionization energy is the energy required to remove an electron from a gaseous atom.
1st ionization energy is the energy required to remove an electron from the valence shell(outermost shell)
What is ionization energy? What is first ionization energy?
as you go across a period left to right, ionization energy increases due to increased nuclear charge.
If you go down a group, ionization energy decreases due to increased distance from the nucleus and increased shielding
What is the periodic trend for first ionization energy?
Write an equation for the 1st ionization of Aluminum.
Write an equation for the 2nd ionization of aluminum.
a) O e) Ne
b) Be f) V
c) F g) Ca
d) Cu h) Se
Which element in each pair has a larger ionization energy?
a)Na or O e)I or Ne
b) Be or Ba f) K or V
c) Ar or F g) Ca or Fr
d) Cu or Ra h) w or Se
a) Sr, Mg, Be
b) Cs, Ba, Bi
c) Na, Al, S
Arrange the following groups of elements in order of increasing ionization energy.
the tendency for an element to attract electrons when chemically combined with another element.
It increases as you move from left to right because the increased nuclear charge attracts more electrons and decreases as you move down because electrons are less attracted to the nucleus due to increased energy levels.
What is the periodic trend for electronegativity?
What element in each pair has a higher electronegativity value?
a) Cl,F c)Mg,Ne
b) C,N d) As, Ca
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