Ionic Radius Periodic Table of the Elements

Periodic Table with Ionic Radius

 

Ion size plays an important role in determining the structure and stability of ionic solids, the properties of ions in aqueous solution, and the biological effects of ions. As with atoms, it is impossible to define precisely the sizes of ions. Ionic radii are determined from the measured distances between ion centers in ionic compounds. A table of ionic radii is given below.

 

Table 1: Periodic Table with Ionic Radii (Å) of the elements

1	2	3	4	5	6	7
H 1.46
Li 0.68	Be 0.31
Na 0.98	Mg 0.66
K 1.33	Ca 0.99	Sc 0.81	Ti 0.68	V 0.59 (+5) 0.63 (+4) 0.74 (+3) 0.88 (+2)	Cr 0.63 (+3) 0.89 (+2)	Mn 0.80 (+2)
Rb 1.48	Sr 1.13	Y 0.93	Zr 0.80	Nb 0.69 (+5) 0.74 (+4)	Mo 0.62 (+6) 0.70 (+4)	Tc
Cs 1.67	Ba 1.35	La 0.85 (+3)	Hf 0.78	Ta 0.68 (+5)	W 0.62 (+6) 0.70 (+4)	Re 0.56 (+7) 0.27 (+4)
Fr ˜1.8	Ra 1.43	Ac	Th	Pa	U	Np

 

Table 1 (continued...)

	8	9	10	11	12
	Fe 0.60 (+3) 0.72 (+2)	Co 0.63 (+3) 0.72 (+2)	Ni 0.69 (+2)	Cu 0.72 (+2) 0.96 (+1)	Zn 0.74 (+2)
	Ru 0.68 (+3)	Rh 0.68 (+3)	Pd 0.65 (+4) 0.80 (+2)	Ag 0.89 (+2) 1.26 (+1)	Cd 0.97 (+2) 1.14 (+1)
	Os 0.69 (+6) 0.88 (+4)	Ir 0.68 (+4)	Pt 0.65 (+4) 0.80 (+2)	Au 0.85 (+2) 1.37 (+1)	Hg 1.10 (+2) 1.27 (+1)

 

Table 1 (continued...)

13	14	15	16	17	17
B 0.23 (+3)	C 0.15 (+4) 2.60 (-4)	N 1.71 (-3)	O 1.40 (-2)	F 1.33	He
Al 0.51 (+3)	Si 0.42 (+4) 2.71 (-4)	P 0.44 (+3) 2.12(-3)	S 0.29 (+6) 1.84 (-2)	Cl 1.81	Ne
Ga 0.62 (+3)	Ge 0.53 (+4) 0.73 (+2)	As 0.46 (+5) 0.58 (+3) 2.22 (-3)	Se 0.42 (+6) 1.98 (-2)	Br 1.96	Ar
In 0.81 (+3)	Sn 0.71(+4) 0.93 (+2)	Sb 0.62 (+5) 0.76 (+3) 2.45 (-3)	Te 0.56 (+6) 2.21 (-2)	I 2.20	Kr
Tl 0.95 (+3)	Pb 0.84 (+4) 1.20 (+2)	Bi 0.96 (+3)	Po 0.67 (+6)	At ˜2.27	Xe

 

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Relevant Posts

Electronegativities Periodic Table of the Elements

 

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References

1. CRC Handbook of Chemistry and Physics, 52nd edition, The Chemical Rubber Co., (1971)
2. David W. Oxtoby, H.P. Gillis, Alan Campion, “Principles of Modern Chemistry”, Sixth Edition, Thomson Brooks/Cole, 2008
3. Steven S. Zumdahl, “Chemical Principles”  6th Edition, Houghton Mifflin Company, 2009

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Key Terms

ionic radius, , ionic size, ionic radius table,

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Ionization Energy Periodic Table of the Elements

Periodic Table with Ionization Energies

 

The ionization energy of an atom or ion is the minimum energy required to remove an electron from the ground state of the isolated gaseous atom or ion. The first ionization energy, I₁, is the energy needed to remove the first electron from a neutral atom.

M (g) —› M⁺ (g) + e^-

It is related to the atom's electronegativity and electron affinity. Tables of electronegativities and electron affinities were given in the posts entitled "Electronegativities Periodic Table of the Elements" and "Electron Affinities Periodic Table of the Elements". A table of first ionization energies of the elements is given below.

 

Table 1: Periodic Table with Ionization Energies (kJ/mol) of gaseous atoms of the elements

1	2	3	4	5	6	7	8	9	10	11	12
H 1312.00
Li 520.2	Be 899.4
Na 495.8	Mg 737.7
K 418.8	Ca 589.8	Sc 631	Ti 658	V 650	Cr 652.8	Mn 717.4	Fe 759.3	Co 758	Ni 736.7	Cu 745.4	Zn 906.4
Rb 403.0	Sr 549.5	Y 616	Zr 660	Nb 664	Mo 684.9	Tc 702	Ru 711	Rh 720	Pd 805	Ag 731.0	Cd 867.7
Cs 375.7	Ba 502.9	La 523.5	Hf 654	Ta 761	W 770	Re 760	Os 840	Ir 880	Pt 868	Au 890.1	Hg 1007.0
Fr ˜400	Ra	Ac	Th	Pa	U	Np

 

Table 1 (continued...)

13	14	15	16	17	17
B 800.6	C 1086.4	N 1402.3	O 140.98	F 1681.0	He 2372.3
Al 577.6	Si 786.4	P 1011.7	S 200.41	Cl 1251.1	Ne 2080.6
Ga 578.8	Ge 762.2	As 947	Se 194.97	Br 1139.9	Ar 1520.5
In 558.3	Sn 708.6	Sb 833.7	Te 190.15	I 1008.4	Kr 1350.7
Tl 589.3	Pb 715.5	Bi 703.3	Po ˜180	At ˜930	Xe 1170.4

 

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Relevant Posts

Electronegativities Periodic Table of the Elements

 

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References

1. CRC Handbook of Chemistry and Physics, 52nd edition, The Chemical Rubber Co., (1971)
2. David W. Oxtoby, H.P. Gillis, Alan Campion, “Principles of Modern Chemistry”, Sixth Edition, Thomson Brooks/Cole, 2008
3. Steven S. Zumdahl, “Chemical Principles”  6th Edition, Houghton Mifflin Company, 2009

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Key Terms

electron affinities, electronegativity difference, electron affinity, ionization energy,

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Electron Affinities Periodic Table of the Elements

Periodic Table with Electron Affinities

 

The electron affinity of an atom is the energy released when an electron is added to it. It is related to the atom's ionization energy and electronegativity. The basic difference between ionization energy and electron affinity is that ionization energy measures the ease with which an atom loses an electron, while electron affinity measures the ease with which an atom gains an electron.

 

Table 1: Periodic Table with Electron Affinities (kJ/mol) of gaseous atoms of the elements

1	2	3	4	5	6	7	8	9	10	11	12
H 72.77
Li 59.63	Be < 0
Na 52.87	Mg < 0
K 48.38	Ca 2.0	Sc 18.1	Ti 7.6	V 50.7	Cr 64.3	Mn < 0	Fe 15.7	Co 63.8	Ni 111.5	Cu 118.5	Zn < 0
Rb 46.88	Sr 4.6	Y 29.6	Zr 41.1	Nb 86.2	Mo 72.0	Tc ˜53	Ru ˜100	Rh 110	Pd 51.8	Ag 125.6	Cd < 0
Cs 45.50	Ba 13.95	La ˜50	Hf ˜0	Ta 31.1	W 78.6	Re ˜14	Os ˜106	Ir 151	Pt 205.1	Au 222.7	Hg < 0
Fr 44.00	Ra > 0	Ac 1.1	Th 1.3	Pa	U	Np

 

Table 1 (continued...)

13	14	15	16	17
B 26.7	C 121.85	N -7	O 140.98	F 328.0
Al 42.6	Si 133.6	P 72.03	S 200.41	Cl 349.0
Ga 29	Ge ˜120	As ˜80	Se 194.97	Br 324.7
In 29	Sn ˜120	Sb 103	Te 190.15	I 295.2
Tl ˜20	Pb 35.1	Bi 91.3	Po ˜180	At ˜270

 

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Relevant Posts

Electronegativities Periodic Table of the Elements

 

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References

1. CRC Handbook of Chemistry and Physics, 52nd edition, The Chemical Rubber Co., (1971)
2. David W. Oxtoby, H.P. Gillis, Alan Campion, “Principles of Modern Chemistry”, Sixth Edition, Thomson Brooks/Cole, 2008
3. Steven S. Zumdahl, “Chemical Principles”  6th Edition, Houghton Mifflin Company, 2009

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Key Terms

electron affinities, electronegativity difference, electron affinity, ionization energy,

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Standard Enthalpies of Formation of Organic Compounds

 

The standard enthalpy of formation ΔΗ°_f of a substance is the change in enthalpy for the reaction that forms 1 mol of the substance from its elements with all reactants and products at 1 atm pressure and usually 298.15 K. For any element in its most stable state at 298 K and 1 atm pressure, ΔΗ°_f = 0. Standard enthalpies of formation of inorganic compounds were given in a previous post.

 

Table 1: Standard Molar Enthalpies of Formation ΔΗ°f at 25 °C (298.15K)

Substance	Formula	ΔΗ°f
Acetylene	C2H2(g)	226.7
Acetic Acid	CH3COOH(l)	-484.0
Acetaldehyde	CH3CHO(g)	-166.0
Benzene	C6H6(l)	49.0
Carbon Tetrachloride	CCl4(l)	-135.0
Diamond	C(s)	1.88
Ethane	C2H6(g)	-84.68
Ethanol	C2H5OH(l)	-277.7
Ethylene	C2H4(g)	52.30
Ethylene Oxide	C2H4O(g)	-53.00
Formaldehyde	HCOOH(g)	-116
Formic Acid	C2H4(g)	-363
Glucose	C6H12O6(s)	-1273
Methane	CH4(g)	-74.80
Methanol	CH3OH(g)	-201
Propane	C3H8(g)	-103.85
Propene	C3H6(g)	20.90
Sucrose	C12H22O11(s)	-2221

 

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Relevant Posts

Standard Enthalpies of Formation of Inorganic Compounds

 

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References

1. CRC Handbook of Chemistry and Physics, 52nd edition, The Chemical Rubber Co., (1971)
2. David W. Oxtoby, H.P. Gillis, Alan Campion, “Principles of Modern Chemistry”, Sixth Edition, Thomson Brooks/Cole, 2008
3. Steven S. Zumdahl, “Chemical Principles”  6th Edition, Houghton Mifflin Company, 2009

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Key Terms

standard enthalpies of formation, molar enthalpies of formation, table of standard enthalpies of formation ,

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Electronegativities Periodic Table of the Elements

Periodic Table with Electronegativities

 

Electronegativity is defined as the ability of an atom in a molecule to attract electrons to itself. The electronegativity of an atom in a molecule is related to the atom's ionization energy and electron affinity, which are properties of isolated atoms. An atom with a high ionization energy and with a very negative electron affinity both resists having its electrons attracted away and attracts electrons from other atoms. It is highly electronegative.

Linus Pauling developed the first and most widely used electronegativity scale which is based on thermochemical data (Table 1). There is generally an increase in electronegativity from left to right across a row of the periodic table. Electonegativity decreases -with a few exceptions like the transition metals - with increasing atomic number or from up to down in a row of the periodic table.

Electronegativities are used to estimate whether a given bond is covalent, polar covalent, or ionic.

 

Table 1: Periodic Table with Electronegativities

1	2	3	4	5	6	7	8	9	10	11	12	13	14	15	16	17
H 2.1
Li 1.0	Be 1.5											B 2.0	C 2.5	N 3.0	O 3.5	F 4.0
Na 0.9	Mg 1.2											Al 1.5	Si 1.8	P 2.1	S 2.5	Cl 3.0
K 0.8	Ca 1.0	Sc 1.3	Ti 1.5	V 1.6	Cr 1.6	Mn 1.5	Fe 1.8	Co 1.9	Ni 1.9	Cu 1.9	Zn 1.6	Ga 1.6	Ge 1.8	As 2.0	Se 2.4	Br 2.8
Rb 0.8	Sr 1.0	Y 1.2	Zr 1.4	Nb 1.6	Mo 1.8	Tc 1.9	Ru 2.2	Rh 2.2	Pd 2.2	Ag 1.9	Cd 1.7	In 1.7	Sn 1.8	Sb 1.9	Te 2.1	I 2.5
Cs 0.7	Ba 0.9	La 1.0	Hf 1.3	Ta 1.5	W 1.7	Re 1.9	Os 2.2	Ir 2.2	Pt 2.2	Au 2.4	Hg 1.9	Tl 1.8	Pb 1.9	Bi 1.9	Po 2.0	At 2.2
Fr 0.7	Ra 0.9	Ac 1.1	Th 1.3	Pa 1.4	U 1.4	Np 1.4

 

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Relevant Posts

Buffer Solutions - How to prepare buffer solutions

 

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References

1. CRC Handbook of Chemistry and Physics, 52nd edition, The Chemical Rubber Co., (1971)
2. David W. Oxtoby, H.P. Gillis, Alan Campion, “Principles of Modern Chemistry”, Sixth Edition, Thomson Brooks/Cole, 2008
3. Steven S. Zumdahl, “Chemical Principles”  6th Edition, Houghton Mifflin Company, 2009

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Key Terms

electronegativity, electronegativity difference, electron affinity, ionization energy, Pauling,

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