The molecule of chlorine has a covalent bond the the charge being equal distributed.
its simple
Cl4 doesn't exist. It should be Cl2 and there will be 4 pairs of non bonding electrons on each chlorine.
Cl2 has a stronger intermolecular forces, London dispersion forces, as there are more electrons in Cl2 than in F2 It is the electrons that cause the instantaneous dipole-induced dipole interactions, more electrons = more dipoles and more easily induced dipoles = more london forces.
A lone chlorine atom has 7 electrons in its outer shell or valence shell, with 3 pairs and 1 unpaired electron. This is an unstable configuration. A stable outer shell contains 8 electrons in 4 pairs. So, two chlorine atoms will form a covalent bond, each sharing its unpaired electron. This bond forms a full pair of electrons that is shared between the two atoms, effectively giving each atom a stable shell of 8 electrons.
Chlorine is a stronger reducing agent than bromine. The bromine is forced to accept electrons from chlorine. Cl2 + 2KBr --> Br2 + 2KCl
Place C in the center and attach 2 Cl atoms to it, and attach 2 H atoms to it. Then place 3 lone pairs of electrons around each Cl atom. That is the Lewis structure.
Cl4 doesn't exist. It should be Cl2 and there will be 4 pairs of non bonding electrons on each chlorine.
Cl2 has a stronger intermolecular forces, London dispersion forces, as there are more electrons in Cl2 than in F2 It is the electrons that cause the instantaneous dipole-induced dipole interactions, more electrons = more dipoles and more easily induced dipoles = more london forces.
Oxidation is loss of electrons and reduction is gain of electrons. In this case the Cl2 molecule is changed to two Cl- ions by gaining electrons, so the Cl2 is reduced. The Br in the NaBr salt is in the form of Br- ions. The Br- ions are changed to neutral Br atoms (a Br2 molecule) by losing electrons and so are oxidised.
H2 O2 Cl2 Br2 N2 I2 F2
A lone chlorine atom has 7 electrons in its outer shell or valence shell, with 3 pairs and 1 unpaired electron. This is an unstable configuration. A stable outer shell contains 8 electrons in 4 pairs. So, two chlorine atoms will form a covalent bond, each sharing its unpaired electron. This bond forms a full pair of electrons that is shared between the two atoms, effectively giving each atom a stable shell of 8 electrons.
Chlorine has 7 electrons, so in order to both have 8, they need to share 2 electrons.:)
How many molecules are present in 42.0g of Cl2
Chlorine is a stronger reducing agent than bromine. The bromine is forced to accept electrons from chlorine. Cl2 + 2KBr --> Br2 + 2KCl
Place C in the center and attach 2 Cl atoms to it, and attach 2 H atoms to it. Then place 3 lone pairs of electrons around each Cl atom. That is the Lewis structure.
It is covalent bond. Cl2 is formed by the sharing of electrons with each other.
At STP, Cl2 gas has a density of 0.0032g/mL. (Wikipedia article, "Chlorine") 0.30g Cl2 x (1mL Cl2/0.0032g) = 93.75mL Cl2
Thiosulfate: 2 S2O32- --> S4O62- + 2e-equivalency to:Chlorine: 1 Cl2 + 2e- --> 2Cl-31.6 ml * 0.141 mmol/ml S2O32- = 4.456 mmol S2O32-= 4.456 *(2 electron / 2 S2O32-) = 4.456 mmol (electrons) == 4.456 *(1 Cl2 / 2 electron) = 2.228 mmol Cl2 == 2.228 * 70.90 mg/mmol Cl2 = 158 mg == 0.158 g Chlorine