HS anion

Formula: HS^-
Molecular weight: 33.073
CAS Registry Number: 15035-72-0
Information on this page:
Other data available:
- Gas phase ion energetics data
- Ion clustering data
Options:
- Switch to calorie-based units

Reaction thermochemistry data

Go To: Top, Constants of diatomic molecules, References, Notes

Data compiled as indicated in comments:
B - John E. Bartmess
M - Michael M. Meot-Ner (Mautner) and Sharon G. Lias

Note: Please consider using the reaction search for this species. This page allows searching of all reactions involving this species. A general reaction search form is also available. Future versions of this site may rely on reaction search pages in place of the enumerated reaction displays seen below.

Individual Reactions

HS^- + =

By formula: HS^- + H⁺ = H₂S

Quantity	Value	Units	Method	Reference	Comment
Δ_rH°	1470. ± 3.	kJ/mol	AVG	N/A	Average of 6 out of 7 values; Individual data points
Quantity	Value	Units	Method	Reference	Comment
Δ_rG°	1441. ± 13.	kJ/mol	H-TS	Rempala and Ervin, 2000	gas phase; B
Δ_rG°	1443. ± 8.4	kJ/mol	IMRE	Bartmess, Scott, et al., 1979	gas phase; value altered from reference due to change in acidity scale; B
Δ_rG°	1443.1 ± 0.42	kJ/mol	H-TS	Shiell, Hu, et al., 1900	gas phase; 0K:350.125±0.009 kcal/mol, corr to 298K from Gurvich, Veyts, et al., With EA( Breyer, Frey, et al., 1981)BDE(0K)=89.97±0.05; B
Δ_rG°	1446. ± 8.4	kJ/mol	IMRE	Cumming and Kebarle, 1978	gas phase; B
Δ_rG°	1432.2	kJ/mol	N/A	Check, Faust, et al., 2001	gas phase; MnO2-(t); ; ΔS(EA)=5.4; B

(HS^- • 4294967295) + = HS^-

By formula: (HS^- • 4294967295S) + S = HS^-

Quantity	Value	Units	Method	Reference	Comment
Δ_rH°	502.62	kJ/mol	N/A	Chaibi, Delsart, et al., 2006	gas phase; For H(32)S-. Given: 2.3147282(17) eV; B
Δ_rH°	502.83 ± 0.75	kJ/mol	Ther	Breyer, Frey, et al., 1981	gas phase; B
Δ_rH°	503.8 ± 9.2	kJ/mol	Ther	Bartmess, Scott, et al., 1979	gas phase; value altered from reference due to change in acidity scale; B
Δ_rH°	358.0	kJ/mol	Ther	Shiell, Hu, et al., 1900	gas phase; 0K:350.125±0.009 kcal/mol, corr to 298K from Gurvich, Veyts, et al., With EA( Breyer, Frey, et al., 1981)BDE(0K)=89.97±0.05; B

HS^- + = (HS^- • )

By formula: HS^- + C₂H₆O = (HS^- • C₂H₆O)

Quantity	Value	Units	Method	Reference	Comment
Δ_rH°	68.20 ± 0.42	kJ/mol	TDAs	Sieck and Meot-ner, 1989	gas phase; B,M
Δ_rH°	67.8 ± 4.2	kJ/mol	TDAs	Meot-ner, 1988	gas phase; B,M
Quantity	Value	Units	Method	Reference	Comment
Δ_rS°	79.5	J/mol*K	PHPMS	Sieck and Meot-ner, 1989	gas phase; M
Δ_rS°	82.8	J/mol*K	PHPMS	Meot-ner, 1988	gas phase; M
Quantity	Value	Units	Method	Reference	Comment
Δ_rG°	44.4 ± 1.7	kJ/mol	TDAs	Sieck and Meot-ner, 1989	gas phase; B
Δ_rG°	43.1 ± 4.2	kJ/mol	TDAs	Meot-ner, 1988	gas phase; B

HS^- + = (HS^- • )

By formula: HS^- + H₂O = (HS^- • H₂O)

Bond type: Hydrogen bond (negative ion to hydride)

Quantity	Value	Units	Method	Reference	Comment
Δ_rH°	59.4 ± 4.2	kJ/mol	TDAs	Meot-ner, 1988	gas phase; B,M
Δ_rH°	59.4	kJ/mol	PHPMS	Sieck and Meot-ner, 1989	gas phase; M
Quantity	Value	Units	Method	Reference	Comment
Δ_rS°	78.2	J/mol*K	PHPMS	Sieck and Meot-ner, 1989	gas phase; M
Δ_rS°	78.2	J/mol*K	PHPMS	Meot-ner, 1988	gas phase; M
Quantity	Value	Units	Method	Reference	Comment
Δ_rG°	36. ± 8.4	kJ/mol	TDAs	Meot-ner, 1988	gas phase; B

(HS^- • 2) + = (HS^- • 3)

By formula: (HS^- • 2H₂O) + H₂O = (HS^- • 3H₂O)

Bond type: Hydrogen bond (negative ion to hydride)

Quantity	Value	Units	Method	Reference	Comment
Δ_rH°	49.0	kJ/mol	PHPMS	Sieck and Meot-ner, 1989	gas phase; M
Δ_rH°	49.0	kJ/mol	PHPMS	Meot-ner, 1988	gas phase; M
Quantity	Value	Units	Method	Reference	Comment
Δ_rS°	98.3	J/mol*K	PHPMS	Sieck and Meot-ner, 1989	gas phase; M
Δ_rS°	98.3	J/mol*K	PHPMS	Meot-ner, 1988	gas phase; M

(HS^- • ) + = (HS^- • 2)

By formula: (HS^- • H₂O) + H₂O = (HS^- • 2H₂O)

Bond type: Hydrogen bond (negative ion to hydride)

Quantity	Value	Units	Method	Reference	Comment
Δ_rH°	52.7	kJ/mol	PHPMS	Sieck and Meot-ner, 1989	gas phase; M
Δ_rH°	52.7	kJ/mol	PHPMS	Meot-ner, 1988	gas phase; M
Quantity	Value	Units	Method	Reference	Comment
Δ_rS°	85.4	J/mol*K	PHPMS	Sieck and Meot-ner, 1989	gas phase; M
Δ_rS°	85.4	J/mol*K	PHPMS	Meot-ner, 1988	gas phase; M

HS^- + = (HS^- • )

By formula: HS^- + CHN = (HS^- • CHN)

Quantity	Value	Units	Method	Reference	Comment
Δ_rH°	87.9 ± 4.2	kJ/mol	IMRE	Meot-ner, 1988	gas phase; See also H2S..CN-; B,M
Quantity	Value	Units	Method	Reference	Comment
Δ_rS°	84.	J/mol*K	PHPMS	Meot-ner, 1988	gas phase; M
Quantity	Value	Units	Method	Reference	Comment
Δ_rG°	62.8 ± 4.2	kJ/mol	IMRE	Meot-ner, 1988	gas phase; See also H2S..CN-; B

HS^- + = (HS^- • )

By formula: HS^- + C₄H₁₀O = (HS^- • C₄H₁₀O)

Quantity	Value	Units	Method	Reference	Comment
Δ_rH°	70.3 ± 1.3	kJ/mol	TDAs	Sieck and Meot-ner, 1989	gas phase; B,M
Quantity	Value	Units	Method	Reference	Comment
Δ_rS°	83.3	J/mol*K	PHPMS	Sieck and Meot-ner, 1989	gas phase; M
Quantity	Value	Units	Method	Reference	Comment
Δ_rG°	45.6 ± 5.0	kJ/mol	TDAs	Sieck and Meot-ner, 1989	gas phase; B

HS^- + = (HS^- • )

By formula: HS^- + C₂H₃F₃O = (HS^- • C₂H₃F₃O)

Quantity	Value	Units	Method	Reference	Comment
Δ_rH°	112.1 ± 2.1	kJ/mol	TDAs	Sieck and Meot-ner, 1989	gas phase; B,M
Quantity	Value	Units	Method	Reference	Comment
Δ_rS°	94.6	J/mol*K	PHPMS	Sieck and Meot-ner, 1989	gas phase; M
Quantity	Value	Units	Method	Reference	Comment
Δ_rG°	84.1 ± 6.3	kJ/mol	TDAs	Sieck and Meot-ner, 1989	gas phase; B

HS^- + = (HS^- • )

By formula: HS^- + H₂S = (HS^- • H₂S)

Quantity	Value	Units	Method	Reference	Comment
Δ_rH°	55.2 ± 4.2	kJ/mol	TDAs	Meot-ner, 1988	gas phase; B,M
Quantity	Value	Units	Method	Reference	Comment
Δ_rS°	82.4	J/mol*K	PHPMS	Meot-ner, 1988	gas phase; M
Quantity	Value	Units	Method	Reference	Comment
Δ_rG°	31. ± 4.2	kJ/mol	TDAs	Meot-ner, 1988	gas phase; B

HS^- + = (HS^- • )

By formula: HS^- + C₄H₅N = (HS^- • C₄H₅N)

Quantity	Value	Units	Method	Reference	Comment
Δ_rH°	96.2 ± 4.2	kJ/mol	TDAs	Meot-ner, 1988	gas phase; B,M
Quantity	Value	Units	Method	Reference	Comment
Δ_rS°	102.	J/mol*K	PHPMS	Meot-ner, 1988	gas phase; M
Quantity	Value	Units	Method	Reference	Comment
Δ_rG°	65.7 ± 4.2	kJ/mol	TDAs	Meot-ner, 1988	gas phase; B

HS^- + = (HS^- • )

By formula: HS^- + C₆H₁₁NO₃ = (HS^- • C₆H₁₁NO₃)

Quantity	Value	Units	Method	Reference	Comment
Δ_rH°	115. ± 4.2	kJ/mol	TDAs	Meot-ner, 1988	gas phase; B
Quantity	Value	Units	Method	Reference	Comment
Δ_rG°	80.3 ± 8.4	kJ/mol	TDAs	Meot-ner, 1988	gas phase; B

HS^- + = (HS^- • )

By formula: HS^- + CH₄O = (HS^- • CH₄O)

Quantity	Value	Units	Method	Reference	Comment
Δ_rH°	71.1 ± 4.2	kJ/mol	TDAs	Meot-ner, 1988	gas phase; B
Quantity	Value	Units	Method	Reference	Comment
Δ_rG°	46.0 ± 4.2	kJ/mol	TDAs	Meot-ner, 1988	gas phase; B

HS^- + = (HS^- • )

By formula: HS^- + C₆H₁₁NO₃ = (HS^- • C₆H₁₁NO₃)

Quantity	Value	Units	Method	Reference	Comment
Δ_rH°	115.	kJ/mol	PHPMS	Meot-ner, 1988	gas phase; M
Quantity	Value	Units	Method	Reference	Comment
Δ_rS°	116.	J/mol*K	PHPMS	Meot-ner, 1988	gas phase; M

Constants of diatomic molecules

Go To: Top, Reaction thermochemistry data, References, Notes

Data compiled by: Klaus P. Huber and Gerhard H. Herzberg

Data collected through July, 1977

Symbols used in the table of constants
Symbol	Meaning
State	electronic state and / or symmetry symbol
T_e	minimum electronic energy (cm^-1)
ω_e	vibrational constant – first term (cm^-1)
ω_ex_e	vibrational constant – second term (cm^-1)
ω_ey_e	vibrational constant – third term (cm^-1)
B_e	rotational constant in equilibrium position (cm^-1)
α_e	rotational constant – first term (cm^-1)
γ_e	rotation-vibration interaction constant (cm^-1)
D_e	centrifugal distortion constant (cm^-1)
β_e	rotational constant – first term, centrifugal force (cm^-1)
r_e	internuclear distance (Å)
Trans.	observed transition(s) corresponding to electronic state
ν₀₀	position of 0-0 band (units noted in table)

Diatomic constants for ³²SH^-
State	T_e	ω_e	ω_ex_e	ω_ey_e	B_e	α_e	γ_e	D_e	β_e	r_e	Trans.	ν₀₀
X ¹Σ⁺	The analysis of the shape of the photodetachment cross section curve Steiner, 1968 leads to ground state constants which are indistinguishable from those of SH (X ²Π), confirming theoretical predictions by Cade, 1967.

Notes

From D₀⁰(SH) and the electron affinities of SH and S.

From the photodetachment cross section Steiner, 1968.

References

Go To: Top, Reaction thermochemistry data, Constants of diatomic molecules, Notes

Rempala and Ervin, 2000
Rempala, K.; Ervin, K.M., Collisional activation of the Endoergic Hydrogen Atom Transfer Reaction S-(2P) + H2 - SH- + H, J. Chem. Phys., 2000, 112, 10, 4579, https://doi.org/10.1063/1.481016 . [all data]

Bartmess, Scott, et al., 1979
Bartmess, J.E.; Scott, J.A.; McIver, R.T., Jr., The gas phase acidity scale from methanol to phenol, J. Am. Chem. Soc., 1979, 101, 6047. [all data]

Shiell, Hu, et al., 1900
Shiell, R.C.; Hu, X.K.; Hu, Q.J.; Hepburn, J.W., A determination of the bond dissociation energy (D-0(H-SH)): Threshold ion-pair production spectroscopy (TIPPS) of a triatomic molecule, J. Phys. Chem. A, 1900, 104, 19, 4339-4342, https://doi.org/10.1021/jp000025k . [all data]

Gurvich, Veyts, et al.
Gurvich, L.V.; Veyts, I.V.; Alcock, C.B., Hemisphere Publishing, NY, 1989, V. 1 2, Thermodynamic Properties of Individual Substances, 4th Ed. [all data]

Breyer, Frey, et al., 1981
Breyer, F.; Frey, P.; Hotop, H., High Resolution Photoelectron Spectrometry of Negative Ions: Rotational Transitions in Laser-Photodetachment of OH-, SH-, and SD-, Z. Phys. A, 1981, 300, 1, 7, https://doi.org/10.1007/BF01412609 . [all data]

Cumming and Kebarle, 1978
Cumming, J.B.; Kebarle, P., Summary of gas phase measurements involving acids AH. Entropy changes in proton transfer reactions involving negative ions. Bond dissociation energies D(A-H) and electron affinities EA(A), Can. J. Chem., 1978, 56, 1. [all data]

Check, Faust, et al., 2001
Check, C.E.; Faust, T.O.; Bailey, J.M.; Wright, B.J.; Gilbert, T.M.; Sunderlin, L.S., Addition of Polarization and Diffuse Functions to the LANL2DZ Basis Set for P-Block Elements, J. Phys. Chem. A,, 2001, 105, 34, 8111, https://doi.org/10.1021/jp011945l . [all data]

Chaibi, Delsart, et al., 2006
Chaibi, W.; Delsart, C.; Drag, C.; Blondel, C., High precision measurement of the (SH)-S-32 electron affinity by laser detachment microscopy, J. Molec. Spectros., 2006, 239, 1, 11-15, https://doi.org/10.1016/j.jms.2006.05.012 . [all data]

Sieck and Meot-ner, 1989
Sieck, L.W.; Meot-ner, M., Ionic Hydrogen Bond and Ion Solvation. 8. RS-..HOR Bond Strengths. Correlation with Acidities., J. Phys. Chem., 1989, 93, 4, 1586, https://doi.org/10.1021/j100341a079 . [all data]

Meot-ner, 1988
Meot-ner, M., Ionic Hydrogen Bond and Ion Solvation. ₆. Interaction Energies of the Acetate Ion with Organic Molecules. Comparison of CH₃COO^- with Cl^-, CN^-, and SH^-, J. Am. Chem. Soc., 1988, 110, 12, 3854, https://doi.org/10.1021/ja00220a022 . [all data]

Steiner, 1968
Steiner, B., Photodetachment of Electrons From SH^-, J. Chem. Phys., 1968, 49, 11, 5097, https://doi.org/10.1063/1.1670004 . [all data]

Cade, 1967
Cade, P.E., Hartree-Fock wavefunctions, potential curves, and molecular properties for OH-(¹Σ⁺) and SH-(¹Σ⁺), J. Chem. Phys., 1967, 47, 2390. [all data]

Notes

Go To: Top, Reaction thermochemistry data, Constants of diatomic molecules, References

Symbols used in this document:

Δ_rG° Free energy of reaction at standard conditions

Δ_rH° Enthalpy of reaction at standard conditions

Δ_rS° Entropy of reaction at standard conditions
Data from NIST Standard Reference Database 69: NIST Chemistry WebBook
The National Institute of Standards and Technology (NIST) uses its best efforts to deliver a high quality copy of the Database and to verify that the data contained therein have been selected on the basis of sound scientific judgment. However, NIST makes no warranties to that effect, and NIST shall not be liable for any damage that may result from errors or omissions in the Database.
Customer support for NIST Standard Reference Data products.

Δ_rG°	Free energy of reaction at standard conditions
Δ_rH°	Enthalpy of reaction at standard conditions
Δ_rS°	Entropy of reaction at standard conditions