Oliver W. A Level Chemistry tutor, GCSE Chemistry tutor, A Level Math...

Oliver W.

£22 - £24 /hr

Currently unavailable: for regular students

Studying: Physical Natural Sciences (Chemistry) (Masters) - Cambridge University

5.0
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21 reviews| 33 completed tutorials

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About me

Hi, my name is Oliver. I study Natural Sciences at Cambridge, with a primary focus on Chemistry, and achieved all A* in my A levels of Maths, Chemistry and Biology. My studies at Cambridge, in addition to many years of tutoring core maths and chemistry, have led to a high understanding of the material required for the A level and GCSE course, and I'm eager to help you understand it too. I fully understand how the prospect of taking A levels can seem daunting, however I don't believe this has to be the case. With the right preparation, you can be much more assured in your capabilities. I believe that I can help you prepare by guiding you to make your studying not easier, but more enjoyable. I look forward to teaching you.  

Hi, my name is Oliver. I study Natural Sciences at Cambridge, with a primary focus on Chemistry, and achieved all A* in my A levels of Maths, Chemistry and Biology. My studies at Cambridge, in addition to many years of tutoring core maths and chemistry, have led to a high understanding of the material required for the A level and GCSE course, and I'm eager to help you understand it too. I fully understand how the prospect of taking A levels can seem daunting, however I don't believe this has to be the case. With the right preparation, you can be much more assured in your capabilities. I believe that I can help you prepare by guiding you to make your studying not easier, but more enjoyable. I look forward to teaching you.  

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Ratings & Reviews

5from 21 customer reviews
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Tanya (Parent)

September 2 2016

Excellent as usual

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Tanya (Parent)

March 2 2016

excellent !

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Tanya (Parent)

February 24 2016

After just 2 lessons with Oliver, my son went from near the bottom of the class to 2nd best in his latest Chemistry test ! Many thanks !

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Tanya (Parent)

February 10 2016

Fantastic first session - Tor was really buzzing after the lesson and very keen to do another. The best thing is that he already feels that, with Oliver's help, he'll definitely be able to get hold of the subject properly and master it. Many thanks Oliver !

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Qualifications

SubjectQualificationGrade
MathsA-level (A2)A*
ChemistryA-level (A2)A*
BiologyA-level (A2)A*
ChemistryDegree (Masters)2.1

Subjects offered

SubjectQualificationPrices
ChemistryA Level£24 /hr
ChemistryGCSE£22 /hr
MathsGCSE£22 /hr

Questions Oliver has answered

Why do group 3 metals form more acidic aqueous solutions than group 2 metals?

The equation of a metal ion forming a metal hexaaqua ion in aqueous solution is as follows.

Mn+ + 6H2O > [M(H2O)6)]n+

These are acidic because the metal is positively charged, and so attracts electron density away from the oxygen and from the O-H bonds. The O-H bonds therefore become weaker, and are easier to break. When the O-H bond breaks, a proton is given off which means that the metal hexaaqua ion is more acidic than regular water.

Because group 3 metals form 3+ cations, and group 2 metals form 2+ cations, group 3 metals form more positive ions than group 2 metals. This means that group 3 metals attract more electron density from the O-H bonds than group 2 metals, and so the O-H bonds become even weaker. The protons are therefore released easier causing the pH to decrease further.

The equation of a metal ion forming a metal hexaaqua ion in aqueous solution is as follows.

Mn+ + 6H2O > [M(H2O)6)]n+

These are acidic because the metal is positively charged, and so attracts electron density away from the oxygen and from the O-H bonds. The O-H bonds therefore become weaker, and are easier to break. When the O-H bond breaks, a proton is given off which means that the metal hexaaqua ion is more acidic than regular water.

Because group 3 metals form 3+ cations, and group 2 metals form 2+ cations, group 3 metals form more positive ions than group 2 metals. This means that group 3 metals attract more electron density from the O-H bonds than group 2 metals, and so the O-H bonds become even weaker. The protons are therefore released easier causing the pH to decrease further.

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3 years ago

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