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Bio 189 > Chapter 2 > Flashcards

Chapter 2 Flashcards

1
Q

Matter

A

Anything that takes up space and has mass

Living or non living

Matter is made up of elements

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2
Q

Element

A

A substance that cannot be broken down into other substances by chemical reactions

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3
Q

Compound

A

A substance consisting of 2 or more different elements

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4
Q

States of matter

A

Liquid, solid, gas, plasma

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5
Q

How many natural elements are there?

A

92

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6
Q

What elements make up 96% of all living matter?

A

Oxygen, carbon, hydrogen and nitrogen

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7
Q

Essential elements

A

Elements an organism need to live a healthy life and reproduce

20-25% of elements are essential

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8
Q

Trace elements

A

Required by organism but in limited quantities

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9
Q

Atom

A

Smallest unit of matter that still retains the properties of an element

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10
Q

Subatomic particles

A

Tiny bits of matter, smaller parts of an atom

Neutrons
Protons and
Electrons

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11
Q

Atomic nucleus

A

Center of an atom

Holds protons and neutrons

Has a positive charge which attracts the negative charge from surrounding electrons which keeps electrons in vicinity of nucleus

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12
Q

Dalton

A

Unit of measurement for atoms and subatomic particles

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13
Q

Atomic number

A

Number of protons unique to that element

23 NA
11 - atomic number

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14
Q

Mass number

A

Total number of protons and neutrons in nucleus

23 NA - mass number
11

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15
Q

Atomic mass

A

Total mass of an atom

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16
Q

Isotope

A

Different atomic forms of same element

Different number of neutrons of other atoms of same element

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17
Q

Radioactive isotope

A

Nucleus decays spontaneously giving off particles and energy

Can lead in to change of element if a neutron turns into a proton

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18
Q

Half life

A

Time it takes 50% of isotope to decay

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19
Q

What determines an atoms identity?

A

Number of protons

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20
Q

What determines an atoms ability to form bonds?

A

An atoms electrons distribution

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21
Q

Radiometric dating

A

Measure the ratio of different isotopes to calculate how many half lives have passed since the organism was fossilized or rock was formed

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22
Q

Energy

A

Capacity to cause change

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23
Q

Potential energy

A

Energy that matter possesses because of its location or structure

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24
Q

The more distant an electron from the nucleus the greater it’s …

A

Potential energy

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25
Q

Electron shells

A

Outside part of an atom where electrons are found. Circles

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26
Q

The first electron shell is..

A

Closet to nucleus and has the least amount of energy

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27
Q

Can electrons move between electron shells?

A

Yes but only by absorbing or losing an amount of energy equal to the difference in potential energy between its position in old shell and that in new shell.

Speed up or slow down?

28
Q

What’s an example of a way an electron can get energy to a higher energy level and therefore move electron shells?

A

Light energy can excite an electron to move to a higher energy shell

29
Q

How is the chemical behavior of an atom determines?

A

By the distribution of electrons in atoms electron shells

30
Q

How many electrons can each shell hold?

A

First shell can hold 2
Second shell can hold 8
Third shell can hold 8

31
Q

The chemical behavior of an atom depends mostly on

A

The number of electrons in its outermost shell or valence shell

32
Q

Valence shell

A

An atoms outermost shell

33
Q

Valence electrons

A

Electrons in an atoms outermost shell

34
Q

An atom with a complete valence shell is

A

Interactive. Will not interact readily with other atoms

35
Q

Inert

A

Chemically in reactive

Full valence shells

36
Q

Orbital

A

3 dimensional space where electron is found 90% of the time

37
Q

How many orbitals are in the first electron shell and what is it called?

A

One spherical orbital called 1s

38
Q

How many orbitals are in 2nd shell?

A

4 orbitals. One large spherical orbital called 2s and 3 dumbbell shaped orbitals called 2p

39
Q

How many electrons can occupy a single orbital?

A

No more than 2

40
Q

How many orbitals are in 3rd shell and What are orbitals in 3rd shell called?

A

9 orbitals and 3s and 3p 3d

41
Q

Chemical bonds

A

Atoms held close together by an attraction

2 strongest bonds are:
Covalent bonds
Ionic bonds

42
Q

Covalent bond

A

Sharing a pair of valence electrons by 2 atoms

43
Q

Molecule

A

2 or more atoms held together by a covalent bond

44
Q

What does H:H represent?

A

The dots represent the valence electrons and the letters represent the element

45
Q

What does H-H represent?

A

The dash represents a single bond aka a shared pair of electrons

46
Q

What does O=O represent?

A

A double bond where 2 atoms share 2 pair of valence electrons

47
Q

What is an atoms valence?

A

Bonding capacity which equals the number of electrons required to complete a atoms outermost shell

48
Q

Electro negativity

A

Electrons are not shared equally

The atom with stronger electronegativity the more strongly it pulls the electrons to itself. Winning the tug of war

49
Q

Non polar covalent bond

A

A covalent bond between 2 atoms of same element share the electrons because their electronegativity is the same

Stand off in tug of war

50
Q

Polar covalent bond

A

Electrons are not shared equally

The stronger atom pulls more

51
Q

Ion

A

As a result of having lost or gained an electron the atom or molecule is positively or negatively charged

Anytime a molecule has an uneven amount of protons and electrons

52
Q

Cation

A

Positively charged ion

53
Q

Anion

A

Negatively charged ion

54
Q

Ionic bond

A

Attraction between cations and anions

55
Q

Can any 2 ions of opposite charge for an ionic bond? Even if they didn’t electron transfer with each other?

A

Yes

56
Q

Atoms that lose an electron will have a _______ charge

A

Positive

57
Q

An atom that gains an electron will have a ______ charge?

A

Negative

58
Q

Ionic compounds or salts

A

Compounds formed by ionic bonds

59
Q

What makes a molecule electrically charged?

A

When protons and electrons stop being equal

60
Q

Hydrogen bond

A

Non covalent attraction between a hydrogen atom and a electronegative atom

61
Q

Van der waals interactions

A

Unevenly distributed electrons creating ever changing regions of positive and negative charge that enable all atoms and molecules to stick together

Weak and only occur when atoms and molecules are very close to each other

62
Q

Chemical reactions

A

Making and breaking of chemical bonds leading to a change in composition of matter

63
Q

Reactants

A

Starting material

64
Q

Products

A

Resulting material

65
Q

Chemical equilibrium

A

Point which the reactions offset one another exactly

Bio 189 (22 decks)

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