Periodic Table with Bond Dissociation Enthalpies

Periodic Table with Bond Dissociation Enthalpies EH(A-A)

 

Bond dissociation enthalpies (energies) for bonds A-A at 298 K and 1 atm pressure are given in Table 1. Average values of bond dissociation enthalpies of the A-B bond in a series of different compounds are given in the post "Bond Dissociation Enthalpies"

 

Table 1: Bond Dissociation Enthalpies EH (A-A) (kJ/mol) at 298 K and 1 atm

1	2	3	4	5	6	7	8	9	10	11	12
H 436
Li 102.8	Be 9.46
Na 72.6	Mg
K 54.8	Ca	Sc	Ti	V	Cr	Mn	Fe	Co	Ni	Cu	Zn
Rb 51.0	Sr	Y	Zr	Nb	Mo	Tc	Ru	Rh	Pd	Ag	Cd
Cs 44.8	Ba	La	Hf	Ta	W	Re	Os	Ir	Pt	Au	Hg
Fr	Ra	Ac	Th	Pa	U	Np

 

Table 1 (continued...)

13	14	15	16	17
B 295	C 178	N 945	O 498	F 158
Al 167	Si 317	P 485	S 429	Cl 243
Ga 116	Ge 280	As 383	Se 308	Br 193
In 106	Sn 192	Sb 289	Te 225	I 151
Tl ˜63	Pb 61	Bi 194	Po	At 110

 

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Relevant Posts

Bond Dissociation Enthalpies EH(A-B)

 

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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

bond enthalpies, bond dissociation enthalpies, table with bond dissociation enthalpies,

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Atomic Radius Periodic Table of the Elements

Periodic Table with Atomic Radius

 

Atom size values cannot be specified exactly. These values can be obtained by measuring the distances between atoms in chemical compounds. Measurements of this type have led to the values of atomic radii for the elements shown below.

 

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

1	2	3	4	5	6	7	8	9	10	11	12
H 0.37
Li 1.52	Be 1.13
Na 1.86	Mg 1.60
K 2.27	Ca 1.97	Sc 1.61	Ti 1.45	V 1.31	Cr 1.25	Mn 1.37	Fe 1.24	Co 1.25	Ni 1.25	Cu 1.28	Zn 1.34
Rb 2.47	Sr 2.15	Y 1.78	Zr 1.59	Nb 1.43	Mo 1.36	Tc 1.35	Ru 1.32	Rh 1.34	Pd 1.38	Ag 1.44	Cd 1.49
Cs 2.65	Ba 2.17	La 1.72	Hf 1.56	Ta 1.43	W 1.37	Re 1.34	Os 1.34	Ir 1.36	Pt 1.37	Au 1.44	Hg 1.50
Fr ~2.7	Ra 2.23	Ac 1.88	Th 1.80	Pa 1.61	U 1.38	Np 1.30

 

Table 1 (continued...)

13	14	15	16	17
B 0.88	C 0.77	N 0.70	O 0.66	F 0.64
Al 1.43	Si 1.17	P 1.10	S 1.04	Cl 0.99
Ga 1.22	Ge 1.22	As 1.21	Se 1.17	Br 1.14
In 1.63	Sn 1.40	Sb 1.41	Te 1.43	I 1.33
Tl 1.70	Pb 1.75	Bi 1.55	Po 1.67	At 1.40

 

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Relevant Posts

Ionic Radius 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

atomic radius, periodic table with atomic radius,

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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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