BIO 120 Grossmont College Biology Terms Discussion

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bio 120

Grossmont College

BIO

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Briefly define the following terms:

Matter:

Element:

Compound:

Atom:

Proton:

Electron:

Neutron:

Nucleus:

Atomic number:

Mass number:

Atomic mass:

Fill in the blank:

  1. Atoms of a particular element that differ in mass number are called __________________________.
  2. The different mass number is due to different numbers of _____________________ in the nucleus.
  3. Write down the name of one type of carbon isotope: ________________________________.
  4. How many protons does it have? __________________
  5. How many neutrons does it have? ________________
  6. How many electrons does it have? ________________
  7. What is its mass number? ________________
  8. Write down the name of a different type of carbon isotope: __________________________.
  9. What is its mass number? ________________
  10. Does the mass number differ from that of the first carbon isotope? Why?
  11. Explain how electrons determine the chemical properties of an atom:
  12. Tell me something you now know about hydrogen bonds and do not just copy the title of the section in the book.

Teach yourself how to draw an electron distribution diagram. (No response needed. For this one, you’re on the honor system. Trust me though; you will need to know this.)

13. Why is life’s molecular diversity based on carbon? Your explanation should demonstrate and understanding of bonding, and it should include an example of an organic molecule that is based on a carbon chain.

14.What is an isomer?

15. Describe each of the chemical groups listed here. Name one type of biological molecule that contains each chemical group.

Phosphate group:

Amino Acid:

16. How are polymers made in cells? How are they broken down? Demonstrate your understanding of each process.

17. What is a polysaccharide?

18. How do phospholipids associate with water to provide structure to cell membranes?

19. Explain the relationship between structure and function for proteins. Include the term denaturation in your explanation. Name one secondary structure of proteins.

20. How do nucleotide polymers form? Name two nucleic acids and explain their respective roles in gene expression.

21. List and describe the fifteen different structures found within eukaryotic cells.

22, Group these fifteen structures on the basis of four main functions.

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Explanation & Answer

Please find the final answer in the attachment. Thanks

Briefly define the following terms:
Matter:
The matter is defined as anything that has mass and takes up space (it has volume). For
example- atoms and compounds are all made of very small parts of matter.
Element:
Element is a pure substance that cannot be broken down by chemical means, consisting of
atoms that have identical numbers of protons in their atomic nuclei. For example: Carbon (C ),
sodium (Na) etc.
Compound:
The compound is a chemical substance composed of many identical molecules composed of
atoms from more than one element held together by chemical bonds. A molecule consisting of
atoms of only one element is therefore not a compound. For example methane (CH4).

Atom:
The atom is the smallest unit of matter that retains all of the chemical properties of an element.
... Most atoms contain all three of these types of subatomic particles—protons, electrons, and
neutrons. Hydrogen (H) is an exception because it typically has one proton and one electron,
but no neutrons.
Proton:
Proton is a subatomic particle with a positive electric charge of +1e elementary charge and a
mass slightly less than that of a neutron. It is represented by a symbol p or p+ or we can say
that an elementary particle that is identical with the nucleus of the hydrogen atom, that along
with the neutron is a constituent of all other atomic nuclei, that carries a positive charge
numerically equal to the charge of an electron, and that has a mass of 1.673 × 10−27 kilogram.
For example, Hydrogen (H) is an exception because it typically has one proton and one
electron, but no neutrons.

Electron:
Electron is a subatomic particle whose electric charge is negative one elementary charge and
it is represented by a symbol e- ⁻or β⁻.
The electron has a mass that is
approximately 1/1836 that of the proton. For example- The hydrogen atom has just
one electron and one proton.
Neutron:

A neutron is a sub-atomic particle with no net electrostatic charge, with a very similar mass to
a proton. Neutrons are thought to comprise of one up quark of charge +2/3 and two down
quarks of charge -1/3 each, resulting in a net charge of zero. Neutrons are present in almost all
atomic nuclei except for Hydrogen.

Nucleus:
The nucleus is the positively charged center of the atom consisting of protons and neutrons.
It's also known as the atomic nucleus. It is discovered in 1911 by Ernest Rutherford based on
the 1909 Geiger–Marsden gold foil experiment. The average nuclear density is about 2.3 x
1017 kg/m3.

Atomic number:
Atomic number (Z) of a chemical element is the number of protons found in the nucleus of
every atom of that element. The atomic number uniquely identifies a chemical element. It is
identical to the charge number of the nucleus. For example, carbon's atomic number (Z) is 6
because it has 6 protons.

Mass number:
Mass number (A) is the sum of the number of protons and the number of neutrons. The small
contribution of mass from electrons is disregarded in calculating the mass number. This
approximation of mass can be used to easily calculate how many neutrons an element has by
simply subtracting the number of protons from the mass number. For example-an atom of
carbon has 6 protons and 6 neutrons. Thus, its mass number is 12.

Atomic mass:
Atomic mass is a weighted average of all of the isotopes of that element, in which the mass of
each isotope is multiplied by the abundance of that particular isotope. Although the SI unit of
mass is the kilogram, the atomic mass is often expressed in the non-SI unit Dalton where 1
Dalton is defined as¹⁄₁₂ of the mass of a single carbon-12 atom, at rest. For an example-the
atomic mass of a carbon-12 atom is about 1.998467052×10−26 kg.
Fill in the blank:
1. Atoms of a particular element that differ in mass number are called
isotopes__________________________.

2. The
different
mass
number
is
due
to
different
numbers
of
_neutrons____________________ in the nucleus.
3. Write down the name of one type of carbon isotope: ___________carbon12_____________________.
4. How many protons does it have? _6 proton_________________
5. How many neutrons does it have? __6 neutron______________
6. How many electrons does it have? __6 electron______________
7. What is its mass number? ______12__________
8. Write down the name of a different type of carbo...


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