CHEMISTRY OF LIFE Flashcards

1
Q

is any substance that
occupies space and has mass.

A

Matter

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2
Q

are unique forms of
matter with specific chemical and
physical properties that cannot be
broken down into smaller
substances by ordinary chemical
reactions.

A

Elements

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3
Q

how many elements are there?

A

118

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4
Q

how many elemts only occur naturally

A

92

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5
Q

what are the four elements common to all living organisms

A
  • oxygen (O),
  • carbon (C),
  • hydrogen (H), and
  • nitrogen (N).
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6
Q

is the smallest unit of matter that retains all
of the chemical properties of an element.

A

atom

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7
Q

All atoms contain

A

protons, electrons, and neutrons.

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8
Q

is a positively charged particle
that resides in the nucleus of an atom and
has a mass of 1 and a charge of +1.

A

proton

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9
Q

is a negatively charged particle
that travels in the space around the
nucleus. It has a negligible mass and has a
charge of –1.

A

electron

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10
Q

like protons, reside in the
nucleus of an atom. They have a mass of 1
and no charge.

A

Neutrons

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11
Q

charges balance each other in a
neutral atom, which has a net zero charge.

A

Neutrons

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12
Q

The ——— of an element is equal to the
number of protons that element contains.

A

atomic number

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13
Q

it is the number of protons plus the
number of neutrons of that element.

A

mass number

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14
Q

the —- of an atom is equal to the number of protons and neutrons of
that atom.

A

mass of an atom

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15
Q

These numbers provide information about the elements
and how they will react when combined.

A

atomic number and atomic mass

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16
Q

A chart of the elements that includes the atomic number and relative atomic mass of each element.

A

The Periodic
Table

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17
Q

provides key
information about the
properties of elements.

A

The Periodic
Table

18
Q

shows how the electrons in each element are organized and provides important details about how atoms will react with each other to form molecules.

A

The Periodic
Table

19
Q

are different forms of the same element that have the
same number of protons, but a different number of neutrons.

20
Q

the most common isotope of carbon, contains six protons and
six neutrons. Therefore, it has a mass number of 12 (six protons and six neutrons) and an atomic number of 6 (which makes it carbon).

21
Q

contains six protons and eight neutrons. Therefore, it has a
mass number of 14 (six protons and eight neutrons) and an atomic number of 6, meaning it is still the element carbon.

22
Q

are isotopes that are Unstable and will lose
protons, other subatomic particles, or energy to form more
stable elements.

A

Radioactive isotopes or radioisotopes

23
Q

The closest shell can hold up to how many electrons?

A

two electrons

24
Q

The second and third energy levels can hold up to how many electrons

A

8 electrons

25
are interactions between two or more of the same or different elements that result in the formation of molecules.
Chemical bonds
26
The tendency of atoms with low atomic numbers (Elements with atomic numbers up to 20 except Hydrogen and Helium) to prefer to have eight electrons in the valence shell
The octet rule:
27
It is when some atoms are more stable when they gain or lose an electron(s) and form ions.
Ionic Bonds
28
are positive ions that are formed by losing electrons.
Cations
29
Negative ions are formed by gaining electrons and are called
anions
30
This movement of electrons from one element to another is referred to as electron transfer.
Ionic Bonds
31
Another way the octet rule can be satisfied is by the sharing of electrons between atoms to form
Covalent Bonds
32
These bonds are stronger and much more common than ionic bonds in the molecules of living organisms.
Covalent Bonds
33
is the most abundant gas in the atmosphere.
N2
34
The formation of water molecules provides an example of
covalent bonding
35
what are the two types of covalent bond
polar and nonpolar
36
form between two atoms of the same element or between different elements that share the electrons equally.
Nonpolar covalent bonds
37
it is when a covalent bond when the electrons shared by the atoms spend more time closer to one nucleus than to the other nucleus.
polar bond
38
the unequal distribution of electrons between the different nuclei, a slightly positive (δ+) or slightly negative (δ–) charge develops.
polar bond
39
this bond provide many of the critical, life-sustaining properties of water and also stabilize the structures of proteins and DNA, the building block of cells.
Hydrogen Bonds
40
Weaker bonds can also form between molecules. Two weak bonds that occur frequently are:
* hydrogen bonds and * van der Waals interactions.