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Chapter 2 Flashcards

1
Q

Matter

A

Anything that takes up space and has mass. Matter is made up from atoms

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2
Q

Element

A

A pure substance made up of only one kind of atom

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3
Q

Molecule

A

2 or more atoms bonded together

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4
Q

Compound

A

A substance consisting of two or more different elements combined in a fixed ratio. Table salt for example is Na(sodium) and Cl(chloride)

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5
Q

Essential elements

A

A chemical element required for an organism to grow, survive and reproduce. 25of the 92 natural elements are essential for humans. Plants need 17

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6
Q

What makes up 96% of living matter? And the other 4%?

A

Oxegyn, hydrogen, carbon, nitrogen

Calcium phosphorus, potassium, sulfur and a few others

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7
Q

Trace elements

A

Elements required by an organism but only in minute quantities.

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8
Q

Atom

A

The smallest functional units of matter.. Make up all chemical substances and ultimately all organisms

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9
Q

Subatomic particles

A

The smaller parts that make up an atom. Neutrons protons and electrons are examples

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10
Q

Protons

A

Electrically and positively charged. Packed tightly with electrons into the atomic nucleus at the center of an atom

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11
Q

Electron

A

Electrically and negatively charged. Also in the atomic nucleus with the protons. Electrons move rapidly forming a cloud of electric charge around the nucleus. It is the attracting of opposite charged that keeps the electrons in the vicinity of the nucleus.

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12
Q

Neutron

A

Electrically neutral

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13
Q

Dalton

A

The unit of measurement for atomic mass equal to roughly the mass of s proton. named after John dalton the British scientist who helped developed atomic theory around 1800.

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14
Q

Atomic mass

A

It is approximately the equivalent of the usual number of protons and neutrons. Allowing for differences with isotopes

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15
Q

Atomic number

A

The number of protons an atom has in their nuclei. It is written as a subscript to the left of an elements abbreviation. Unless other wise indicated, an atom is neutral in electrical charge so if it has 2 protons then it has 2 electrons also. Atomic number tells us he number of protons and electrons an electrically neutral atom has

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16
Q

Simplest atom

A

Hydrogen. Helium is #2

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17
Q

Atomic nucleus

A

Small dense region consisting of protons and neutrons which gives the atomic nucleus a slight positive charge

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18
Q

Electron speed

A

An electron could orbit the earth in less than 20 seconds

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19
Q

Orbital

A

Area where an electron can be found. First one is s shape, second layer is one s and 3 p orbitals

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20
Q

Energy

A

The capacity to do work to cause change

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21
Q

Lowest energy electrons go

A

In the first she’ll

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21
Q

Valence electrons

A

Electrons in the outermost she’ll

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22
Q

Net electric charge of zero

A

With the exception of ions, the number of protons and electrons is equal which results in a net electric charge of zero

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23
Q

Rows in periodic table

A

Known as periods, go up and down. They indicate the number of electron shells with the least being at the top

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24
Columns in periodic table
Aka groups read left to right and indicate the number of electrons in the outer shell
25
Weight vs mass
Weight is the gravitational pull on mass. It is different on earth or the moon but mass is always the same
26
Mole
Amount of a substance that has as many atoms/molecules/ions/ electrons or photons as atoms in 12 grams of carbon.
27
Isotope
An element that has a different amount of neutrons than it usually would
28
Radioisotope
Unstable; how long now they last is measured in half lives ( the time it takes for 50% of the isotope to decay) they emit radiation which in turn makes them more stable
29
2 ways radioisotopes are used for good
H
30
Water makes up
60% of humans, 95% of plants
31
Carbon is* nitrogen is*
A major building block for all living matter,* a vital element in all proteins
32
Mineral elements essential for life
Calcium, chlorine, magnesium, potassium, phosphorus, sodium, sulfur
33
Key regulators of water and electric current
Potassium and sodium
34
Makes skeletons and shells
Calcium and phosphorus
35
Molecular formula
When the chemical symbols for all atoms present are written out. H20 is and example. The 2 next to h tells you there is 2 hydrogen
36
Emergent properties
The properties of a compound differ greatly from the properties of the elements that make it up
37
Covalent bonds
Bond where atoms share electrons. They are strong because the shared electrons act as if they belong to each atom
38
Structural formula
H-O-H covalent Bonds are shown with a line
39
Octet rule
Many atoms are most stable when they have 8 electrons in their outer shell
40
Double bond
When atoms share two pairs(4 electrons) written with two lines
41
Electronegativity
The measure of an atoms ability to attract electrons in a bond with another atom
42
Polar covalent bonds
A bond in which electrons are shared, but not equally. The atom with a higher electronegativity hordes the shared electrons
43
Kinetic energy
The energy of moving matter
44
Water and how it's polar/ electronegative
Oxegyn is more electronegative than hydrogen so the shared electrons pull closer to the nucleus of oxegyn than to the hydrogen. This unequal distribution of electrons gives the molecule a region of partial negative charge
45
Nonpolar covalent bonds
Two atoms of similar electronegativity covalently bond and share the electrons equally
46
Hydrogen bond
Hydrogen atom from one polar molecule is attracted to an electronegative atom such as oxegyn or nitrogen from another polar molecule
47
Enzymes
Type of protein found in all cells that facilitates or catalyzes many important chemical reactions
48
Can see waals dispersion forces
Also a weak molecular attraction. Because the atoms are always moving around they end up sometimes being in a position that gives the atom a electric charge that doesn't last. This electric charge causes attraction but dies quickly
49
Ion
When an atom gains or loses an electron it acquires a net electric charge
50
Cation
Ions with a net positive charge ( this would be an ion with maybe 11 protons and 10 electrons
51
Anion
Ions with a net negative charge, more electrons than protons
52
Ionic bond
Occurs when a cation bonds to an anion. An example is na+ and Cl- which form table salt.
53
Free radical
A molecule containing an atom with a single unpaired electron in its outer shell. In an attempt to get an electron they may steal one from another molecule which in turn makes that molecule a free radical, it's a chain reaction.
54
Antioxidant
molecules that can donate an electron without becoming highly reactive. Examples of this of vitamin c and e found in fruits, veggies and plant compounds called flavonoids
55
Chemical reaction
When one or more substances are changed into other substances by the making or breaking of chemical bonds
56
All chemical reactions
Need Energy to make the molecules encounter eachother, a catalyst of some sort. And they all proceed in a particular directional until they reach chemical equilibrium. Also most happen in watery substances
57
Chemical equilibrium
When the rate of formation of product equals the rate of formation of reactants aka. The concentration of products and reactants stops changing.
58
Water: brain, blood, lungs
Brain: 70%, blood: 80%, lungs:90%
59
Solute
Substance dissolved in water
60
Solvent
The liquid dilutes are dissolved into. Water is the most abundant solvent in nature
61
Solution
When a solute is dissolved into a solvent this is the product
62
Why do some things dissolve in water
The covalent bonds linking hydrogen and oxegyn are POLAR. This leaves oxegyn with a slight negative charge and the hydrogen a with a slight positive charge. To dissolve in water the substance must be electrically attracted to h2o. Generally molecules with ionic or polar bonds will dissolve
63
Hydrophilic
Water loving, molecules that are attracted to water
64
Hydrophobic
Water fearing. Molecules that have mostly carbon or hydrogen will be hydrophobic because their bonds are non polar and therefor not attracted to h2o, oils are hydrophobic.
65
Amphipathic; what they do in water
Molecules with hydrophobic and hydrophilic regions. In water they form spheres called micelles which put all the hydrophobic parts inside the sphere and all the hydrophilic parts on the outside touching the water. Detergents are an example. They can also form linear structures with two layers, the two outer layers are hydrophilic and the inside is hydrophobic.
66
Concentration
The amount of dissolved solute per volume. 1 g of Nacl dissolved in 1 liter of water the concentration is 1g/L
67
Molarity of a solution
F
68
The three states h2o exists in and the effect the bonds breaking has
Solid(ice) occurs when temperatures fall and the hydrogen bonds break less frequently causing larger and larger clusters of water until it freezes into a crystalline matrix. Liquid(water) most common with hydrogen bonds continuously being broken and formed again. If the temp rises the bonds break quicker and molecules of water escape into a gaseous state, becoming water vapor.
69
Density of water vs ice
H2o molecules are more orderly and further away in ice which makes ice less dense and allows it to float on water
70
Heat of vaporization(and for water)
The heat needed to vaporize 1 mole of any substance. This is high for water because all the hydrogen bonds need to be broken
71
Heat of fusion
The amount of heat that must be withdrawn from a substance to turn it from liquid to solid. This is also high for water.
72
Specified heating
The amount of energy needed to raise the temperature of 1 gram of a substance by 1degree Celsius
73
Heat capacity
The amount of heat needed to raise the temp of an entire object or substance. A large container of water has a higher heat capacity than a cup of water
74
Colligative properties
Properties that depend on the total number of dissolved solutes instead of the type of solutes. Water will freeze at a lower temp than 0degrees if a solute is added and higher than 100 degrees for vaporizing.
75
Hydrolysis reactions
A chemical reaction that utilizes water to break apart molecules
76
water is incompressible
It's volume does not significantly decrease when subjected to high pressure. This is important because many organisms use water to provide support
77
Cohesion/ adhesion
The phenomenon of water molecules being attracted to eachother The ability of water to be attracted to and therefor adhere to a surface that is not electrically neutral
78
Surface tension
A measure of the attraction between molecules at the surface of a liquid
79
Acid
Substances that release hydrogen ions into solutions
80
Hydrochloric acid
Strong acid. Almost complety dissolves into H+ and Cl- when mixed with water
81
Carbonic acid
Weak acid because some of it stays in its H2CO3 state when dissolves in water
82
Base
Has the opposite effect when dissolved in water, it decreases the concentration of H+
83
Ph
The measure of the H+ concentration of a solution
84
Polarity
The unequal sharing of electrons within a molecule
85
Acidic/ Alkaline
Ph of 6 or less//// A substance with a ph above 7
86
Normal ph for living cells, and for blood
Living cells= 6.5 to 7.8, in blood 7.35 to 7.45

Biology (11 decks)

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