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Anatomy > Chemistry > Flashcards

Chemistry Flashcards

Fundamentals of chemistry

1
Q

Atoms

Definition + components

A

The most basic unit of all matter. Neucleus surrounded by subatomic particles.

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2
Q

Subatomic particles

List them

A
  1. Protons
  2. Neurons
  3. Electrons
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3
Q

Protons

charge / mass / location on atom

A

Subatomic particle
+1 charge / 1 mass / stuck in the in nucleus
* Number dictates it’s element

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4
Q

Electrons

A

Subatomic particle
-1 charge / «<1=0 / travels around the nucleus
- moves easily between atoms
- charge changes when added or removed

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5
Q

Neurons

A

Subatomic particle
0 charge / 1 mass / stuck in the nucleus

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6
Q

What is the charge of an atom?

A

protons - electrons
= charge

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7
Q

What is the mass of an atom?

A

of protons - # of neurons

= mass

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8
Q

What are elements?

A

Different types of atoms that have different chemical properties.
The # of protons determines what element an atom is and the charge of its nucleus.
The # of neurons and electrons can be different between different atoms of the same element.

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9
Q

Periodic table of elements

A

Table that shows all elements known to man, each square is a different element.
Contains:
* Name of element (not always)
* Atomic # = # of protons in the nucleus
* Atomic symbol = 1 capital letter or 1 capital + 1 lower case
* Atomic mass = mass of atom, #protons + #neurons

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10
Q

Electron Shells

A

3 orbiting shells of electrons around the nucleus.
1st shell has 2 electrons
2nd shell has 8
3rd has 8

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11
Q

What do atoms want?

A

2 things:
1. The outer shell to be full
2. A neutral charge (# of protons = # of electrons)

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12
Q

What are right column atoms?

A

Noble gasses
Generally don’t interact with other elements & have a full outer shell (same # of protons and electrons)

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13
Q

What are ions?

A

Atoms on a small molecule with an electrical charge.
The # of protons + electrons are different but make a full outer shell.

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14
Q

Anions

A

Ions with a negative cahrge.
protons < electrons

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15
Q

Cations

A

Ions with a positive charge
protons > electrons

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16
Q

Ionic bond

A

When possitive and negative ions attract and form a bond.
(-)Anion + (+)Cation –> negative attracts positive

ex: table salt - NaCl

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17
Q

List of important ions

Name + Periodic lable

A
  • Sodium - Na+
  • Chloride - Cl-
  • Potassium- K+
  • Calcium - Ca++
  • Magnesium - Mg ++
  • Iron - Fe (2+ or 3+)
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18
Q

What is a covalant bond?

A

2 atoms held together by sharing electrons.
This allows atoms to have a full outer shell with a neutral charge, forming a bond stronger than ionic bonds.

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19
Q

Single bond

A

2 atoms sharing 2 electrons

ex: H-H / H-O-H

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20
Q

Double bond

A

2 atoms sharing 4 electrons

ex: O=O (molecular oxygen)

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21
Q

What are molecules?

A

2 or more atoms held together by a covalant bond

22
Q

Molecular formula

A

Refers to how many atoms in each element are found in molecules. It’s expressed at the bottom right

23
Q

Polar Covalent Bonds

A

Covalent bond where 2 atoms don’t share electrons equally
* Atom pulls more has slight negative (-) charge
* Atom that less has slight positive charge

24
Q

Chemical Reactions

A

Occur when molecules change into different molecules.
The arrangement of atoms into molecules changes but the number of atoms of each element doesn’t change.

25
Q

Water

Components

A
  • Made of 2 hydrogen + 1 oxygen
  • Hydrogens are at an angle from each other, not on opposite sides of oxygen
26
Q

Dipole

A

A polar bond with one molecule slightly positive and one slightly negative.

27
Q

Hydrogen Bonds

A

Bonds between (not within) different water molecules + in other places too.

Like ionic bonds + attracts =weaker

28
Q

Hydrophilic

A

Water-loving substances that disolve in water.
* Charged on polar substances
* Slight charges on water molecules are attracted to charges on hydrophilic substances

29
Q

Hydrophobic

A

water-fearing
* Substances that don’t disolve in water.
* non-polar substances

30
Q

Acids

A

Substances that release H+
More H+ released, the more acidic + lower the pH

31
Q

Bases

A

Chemicals that absorb H+ with a high pH.

32
Q

pH

A

Refers to the measure of how acidic or basic a solution is.
1. Acidic: pH <7, #H+ > OH-, lower pH = more acidic
2. Neutral: pH = 7, pure water
3. Basic: pH > 7, #H- < OH- higher pH = less acidic

33
Q

Organic Molecules

A

Molecules with Carbon and Hydrogen bonds.
Living things are made of organic molecules.
(I Carbon makes 4 bonds, forming the backbone of all organic molecules
Hydrogen makes 1 bond, found all over all organic molecules
C-C and C-H bonds are non-polar)

34
Q

Other elements in biological organic molecules

A
  • Oxygen (O) - 2 bonds
  • Nitrogen (N) - 3 bonds
    In many organic molecules but not all
    Both form polar bonds
    Molecules with lots of O + N = hydrophobic
  • Phosphorus (P)
  • Sulfur (S)
    Not as common as O + N
35
Q

Inorganic carbon molecule

A

Carbon Dioxide (CO2)

36
Q

What is energy?

A

Doing things or the ability to do things
* Can never be created or destroyed
* Can be changed from one form to another

Ex: drop something
Loses gravitational energy as it gets lower
Gains kinetic energy as it goes faster
Turning gravitational energy into kinetic energy

37
Q

Kinetic Energy

A

The energy of something moving.
The faster something goes + the more it weights = + kinetic energy it has

Heat energy is a form of kinetic energy
ex: How fast chemicals are moving in the solution/ substance

38
Q

Electromagnetic radiation

A

Light

39
Q

Potential Energy

A

Energy based on something’s position.

40
Q

Gravitational Energy

A

Energy based on somethings relationship to Earth’s core.
further from Earth -> ^ gravitational E

41
Q

Chemical Energy

A

Energy in chemical bonds
* Bigger molecules have more energy - How we get energy from food
* Different bonds have different amounts of E
* Breaking bonds to make new ones changes the amount of E in molecules

42
Q

Reactants

A

Chemicals at the beginning of a process.

43
Q

Products

A

Chemicals at the end of reactions.

44
Q

Exergonic reactions…

A

release Energy.
* E of reactants > E of products

Spontaneous reactions - can happen without any other E

45
Q

Endergonic reactions…

A

take in Energy.
E of reactants < E of products

46
Q

Metabolism

A

refers to all chemical reactions that happen in the body.
1. Anabolism
2. Catabolism

47
Q

Catabolism

A

breaks big molecules into smaller ones.
Exergenic reaction = releases E

48
Q

Anabolism

A

makes big molecules out of smaller molecules.
Endergonic reaction = requires E

49
Q

Metabolism

In relation to digestion

A
  1. Catabolism - to get energy
  2. Move things
  3. Build large molecules (Anabolism)
50
Q

Electrochemical Gradient

A

Energy from there being different concentrations of chemicals + different charges on either side of the plasma membrane.

51
Q

Chemical Equilibrium

A

When reactions reach a certain ratio of reactants to products and stop.

The further you are from equilibrium - the faster the reactions
^ Reactants –> Equilibrium –> ^ rate of reaction
V Products –> Equilibrium–> ^ rate of reaction

Anatomy (15 decks)

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