AP Biology – Chapter 2 Basic Chemistry (Worksheet)



AP Biology – Chapter 2 Basic Chemistry (Worksheet)

Lookabaugh – Campbell Seventh Edition

Objectives:

✓ Know the 3 subatomic particles, their properties and signficance to organisms.

✓ Know the types of bonds, how they form and their relative strengths

Concept: Matter

1. Matter is anything that has ____________ and takes up space.

2. An ____________ is a substance that cannot be broken down inot other substances by ___________ reactions. Examples are: _______________ _______________ ________

3. A __________________ is a substance consisting of two or more ____________ combined in a fixed ratio like: H2O or NaCl or even glucose ______________

4. C, H, O, and __ make up ________ % of all living matter. Most consider their to be about 25 of the 92 natural elements to be essential to life however about ________ of those are found in trace amounts in living organisms.

5. _____________ elements are those required by organisms in __________ quantities

Examples are _______________ which helps with ________________ and __________ which helps with __________________________.

Concept: An Element’s properties are determined by their atoms

6. __________ are the smallest unit of an element that still retains the property of the element. Atoms are comprised of _____________ _________________ & __________

7. Protons are _________ charged and are found ____________________________

8. Electrons are _________ charged and are found __________________. They are what determines the chemical properties and ____________ or an element.

9. __________________ have no charge. They are found in the ____________ and provide ____________ or weight to the element. The number can vary in an element’s atoms. This results in ______________________ like carbon which has 12 C and 14 C. Both of these atom forms have the same number of protons which is ______ but a different number of ____________________.

10. The atomic _______________ of an element is equal to the number of ____________ it has and is unique to every element and determines the placement in the periodic chart of elements.

11. The atomic mass of an element is the sum of its protons and _______________.

(Make sure you know how to find the information on a periodic chart)

Concept: Chemical bonding

12. Chemical bonds are determined by _________________ electrons in the outer shells of atoms.

13. ______________ bonds are between electrons of atoms that share electrons.

14. ___________ covalent bonds are between atoms which share the e- equally. Atoms will vary in their ________________________ and are often driven to pull on electrons from covalent bonds.

15. In _____________ covalent bonds one atom has a greater _____________________ than another so the result is uequal _____________ of electrons. An example is water which finds the _______________ end to be more negative and the ____ ends to be more positive. Draw this molecule below and show the – and + symbols.

16. Ionic bonds also show unequal charges in bonding. However, due to the strong electronegativity of one atom, the e- will actually be pulled away leaving ___________ on the two atoms. This creates _____________. These are often created in water in organisms to carry out metabolic functions. Give an example: ______________

17. ______________ bonds are weak bonds that form between positively charged _______________ bonds of an atom of one molecule and the strongly electronegative oxygen or nitrogen of another molecule. Draw below 5 water molecules and show how the weak hydrogen bonding between the molecules.

18. Van der Waals interactions or bonds are created due to _____________ _____________________ of electrons within molecules due to their uneven distribution. These help to contribute to the 3 D shape of a molecule. *** Remember this when referring to proteins later.

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