Br2 CH3CH=CHCH3 = C4H8Br2 | Chemical Equation Balancer

= 1,2-Dibromobutane; 1,2-Butylene bromide

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Atomic_weight (g/mol) 159.8080

Density of solid (kg/m3) 3102

Boiling Point (°C) 58.8

Melting point (°C) -7.2

Electron negativity 2.96

First Ionisation Energy 1139.9


short form


Density of solid (kg/m3) 604

Boiling Point (°C) 2.25

Melting point (°C) -122.2



1,2-Dibromobutane; 1,2-Butylene bromide

Atomic_weight (g/mol) 215.9143

Combination reaction

Also known as a synthesis reaction. One kind of frequently occurring combination reaction is the reaction of an element with oxygen to form an oxide. Under certain conditions, metals and nonmetals both react readily with oxygen. Once ignited, magnesium reacts rapidly and dramatically, reacting with oxygen from the air to create a fine magnesium oxide powder.

O2 + S → SO2 PH3 + HClO4 → PH4ClO4 CaO + CO2 → CaCO3 Fe + S → FeS 2Al + 3I2 → 2AlI3 2H + NH2OH → NH4OH C2H2 + 2HCHO → HOCH2CCCH2OH View All Combination reaction

Decomposition reaction

Many decomposition reactions involve heat , light, or electricity to input energy. Binary compounds are compounds which consist of only two elements. The simplest sort of reaction to decomposition is when a binary compound breaks down into its elements. Mercury (II) oxide, a red solid, decomposes to form mercury and oxygen gas when heated. Also, a reaction is regarded as a decomposition reaction even if one or more of the products are still a compound. A metal carbonate breaks down to form a metal oxide and carbon dioxide gas. Calcium carbonate for example decomposes into calcium oxide and carbon dioxide.

2H2O2 → 2H2O + O2 Na2S2O7 → Na2SO4 + SO3 5O2 + C4H6Cl2 → 2H2O + 2HCl + 4CO2 2KClO3 → 2KCl + 3O2 CaCl2 → Ca + Cl2 Fe2(SO4)3 → Fe2O3 + 3SO3 2HI → H2 + I2 View All Decomposition reaction

Oxidation-reduction reaction

An oxidation-reduction (redox) reaction is a type of chemical reaction that involves a transfer of electrons between two species. An oxidation-reduction reaction is any chemical reaction in which the oxidation number of a molecule, atom, or ion changes by gaining or losing an electron. Redox reactions are common and vital to some of the basic functions of life, including photosynthesis, respiration, combustion, and corrosion or rusting.

2NH3 + 2B → 3H2 + 2BN 3Ca + 2P → Ca3P2 4C + Li → 4CO + BeS 2NO2 → N2O4 C + CO2 → 2CO 2NaClO → 2NaCl + O2 2HCl + Ni → H2 + NiCl2 View All Oxidation-reduction reaction

Single-replacement reaction

A + BC → AC + B Element A is a metal in this general reaction and replaces element B, a metal in the compound as well. If the replacement element is a non-metal, it must replace another non-metal in a compound, and it becomes the general equation. Many metals easily react with acids, and one of the reaction products when they do so is hydrogen gas. Zinc reacts to the aqueous zinc chloride and hydrogen with hydrochloride acid (see figure below).

2HCl + Zn → H2 + ZnCl2 4Cl2 + 2Fe2O3 → 4FeCl2 + 3O2 CH3COCl + 2C2H5NH2 → NH3 + C2H5Cl + CH3CONHC2H5 Zn + CuCl2 → Cu + ZnCl2 Cu(NO3)2 + Zn → Cu + Zn(NO3)2 H2SO4 + BaO2 → H2O2 + BaSO4 Mg + ZnCl2 → Zn + MgCl2 View All Single-replacement reaction

Double-replacement reaction

AB + CD → AD + CB A and C are positive charged cations in this reaction, while B and D are negative charged anions. Double-replacement reactions typically occur in aqueous solution between the compounds. To cause a reaction, one of the products is usually a solid precipitate, a gas, or a molecular compound like water. A precipitate forms in a double-replacement reaction when the cations from one reactant combine to form an insoluble ionic compound with the anions from the other reactant. The following reaction occurs when aqueous solutions of potassium iodide and lead ( II) nitrate are blended.

BaCl2 + MgSO4 → MgCl2 + BaSO4 NaOH + NaHS → H2O + NaKS Ca(OH)2 + H2SO4 → 2H2O + CaSO4 H2SO4 + NaNO3 → HNO3 + NaHSO4 H2S + Li2O → H2O + Li2S Ca3N2 + 3H2O → 3Ca(OH)2 + 2NH3 2KOH + Mg(NO3)2 → 2KNO3 + Mg(OH)2 View All Double-replacement reaction

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