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Nt1310 Unit 1 Research Paper

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Q1.
(i)

I have depicted the 3 naturally accruing isotopes of hydrogen. Hydrogen-1, sometimes known as Protium or just hydrogen, hydrogen-2, also known as Deuterium and finally Hydrogen-3, which is also known as Tritium. Although each isotope has a different number of neutrons; 0, 1 and 2, respectively. This has no impact on their chemical properties.
But, it does however affect the physical properties. Namely their mass. Whereas Hydrogen-1 has an atomic mass of 1amu, Hydrogen-2 has an atomic mass of 2, due to the presence of a neutron in addition to the proton within the nucleus. And Hydrogen-3 has an atomic mass of 3amu as a result of another additional neutron. Each isotope also differs in its’ nuclear binding energy, this is a result …show more content…
Non-bonding pair of electrons, also known as lone pair of electrons are those pairs of electrons that are not used in the covalent bonding between the atoms.
All the above Lewis dot structures are of covalent bonds between atoms. The attraction in covalent bonds are an electrostatic one between the positive charge of the nuclei and the negative charge of the electrons. The first molecule of H-Cl has a bond order of 1, a single bond. The molecule of H2C=CH2 has a bond order of two, the bond itself is short that a single bond and therefore is stronger. The third molecule of N2 has a triple bond, which is shorter than a single or double bond and subsequently stronger than them both.
(iv)
Ionic bonding takes place between a metal and a non-metal. It is where an atom with lower electronegativity loses an electron to an atom with higher electronegativity in order to fulfil the octet rule. Like in the case of NaF; Na which has 1 electron in its valence shell, loses it to F which has 7 electrons in its valence shell. By losing an electron sodium has become a cation, which is positively charged. And fluorine by gaining an electron has become a negatively charged anion. The cation, Na+ and the anion, F- now electrostatically attract to each other. This attraction is known as an ionic …show more content…
Six H2O molecules attract to Na+ with their slightly negative oxygens. And six H2O molecules also attract to the Cl- anion but with the hydrogen atom.
The bond between ionic compounds is stronger than the bond between covalent compounds. This being so, it means ionic compound have a higher melting point and a higher boiling point. And covalent compounds have the opposite, a lower melting point and boiling point. Ionic compounds tend to be soluble it polar solvents. Whereas covalent compounds tend to be soluble in non-polar solvents. This can be understood if we look back at NaCl, an ionic compound which dissolves in H2O, which is polar.
The components of a solution of NaCl and H2O can be separated through electrolysis. Once the electrodes are placed in the solution and the electricity is turned on the process on electrolysis will begin. H(g) will start to form around the cathode, Cl(g) around the anode. A NaCl solution will also form around the anode. A solution of sodium hydroxide will also be formed.
(iii)
Mercury (I) Oxide Mercury (II) Oxide Mass Mercury 1.00g

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