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Bio190 > Week 2 - Chemistry Part 1 > Flashcards

Week 2 - Chemistry Part 1 Flashcards

(58 cards)

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1
Q

Every substance that exists is made of

A

Matter

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2
Q

What is Matter?

A
  • Anything that takes up space and has mass
  • A pure substance
    Requires at least 1 subatomic particle
  • Ex: protons, atoms, molecules, compounds
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3
Q

What is an element?

A

The simplest substance that cannot be broken down further using chemical reactions
- They are arranged on the Periodic Table

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4
Q

What is an Atom?

A

One unit of element

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5
Q

Combining two or more atoms together to form chemical bonds are called

A

Molecules

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6
Q

All molecules have ___ properties

A

Special

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7
Q

Molecules are written as ____.

A

Formulas

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8
Q

Molecule formulas show ____, ____.

A
  • Types of atoms

- Amount of each type of atom

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9
Q

What is a subscript?

A

Amount of each type of atom in a molecular formula

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10
Q

What is the Atomic structure composed of?

A
  • Core nucleus

- Electron Cloud

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11
Q

What are the 3 subatomic particles?

A
  • Electron
  • Proton
  • Neutron
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12
Q

Location and charge for: Electron

A
  • Electron cloud

- Negative

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13
Q

Location and charge for: Neutron

A
  • Nucleus

- Neutral

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14
Q

Location and charge for: Proton

A
  • Nucleus

- Positive

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15
Q

What takes up 99% of MASS of an atom?

A

Core nucleus that contains proton and neutrons

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16
Q

What takes up 99% of SPACE of an atom?

A

Electron cloud that contains electrons

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17
Q

What are 4 elements that make up human body?

A
  • Carbon
  • Oxygen
  • Hydrogen
  • Nitrogen
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18
Q

3.5% of elements of the Human body

A
  • Calcium
  • Phosphorus
  • Potassium
  • Sulfur
  • Sodium
  • Chlorine
  • Magnesium
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19
Q

What are TRACE minerals in the body and percentage?

A
  • 0.5%

- iron, iodine, manganese, selenium

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20
Q

What deficiency causes thyroid malfunctions?

A

Low iodine

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21
Q

Deficiency leading to low red blood cell count?

A

Low iron

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22
Q

Define Atomic structure

A
  • Elements listed on the periodic table are in the ‘perfect state’
  • But they can vary in terms of subatomic particle content
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23
Q

What is an Isotope?

A

When the number of neutrons is different in the nucleus than another atom of the same element

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24
Q

How often do radioactive isotopes release a neutron?

25
The process of dating fossils and diagnosing medical disorders
Carbon dating
26
Where do electrons orbit in an atom?
Orbit around the nucleus
27
What is the Octet Rule
8 electrons can fill each shell
28
How many electrons are able to be in the first shell?
Only 2!
29
What is the outermost/most important shell?
Valence shell
30
Lewis Dot Diagrams: Why are valence electrons the most improtant?
To figure out how many atoms pair up with other atoms
31
Lewis Dot Diagrams: Electrons will always try to ___
Pair up
32
Lewis Dot Diagrams: Lone electrons
= bad = free radical | - will try to find other atoms with other lone elctrons to pair them up
33
Lewis Dot Diagrams: Define process of drawing
- write out atom symbol - Draw dots around symbol representing number of electrons in the atoms valence shell - North, South, East, West - Dots must fill every side around the atom - Try to pair up as many atoms as you can - make sure each side has at least 1 electron
34
Lewis Dot Diagrams: Atoms want to have ____, ____
Complete variance shells! They have to find a buddy!
35
Different methods of atom bonding
- Ionic bonding - Covalent bonding - Polar - Non-polar - Weak interactions
36
Bonding: Atoms will give or take electrons 'electron transfer'
Ionic bonding
37
Ionic bonding happens between ___
Ions = charged particles
38
Why does ionic bonding happen?
Some atoms are really close to having filled Valence shells
39
Atoms that have __ # of electrons prefer to 'take' an electron to become more ___
7, stable (filled shell)
40
Atoms that ___ electrons do so to jump down to the next ____ valence shell
lose, lowest
41
Transferring electrons in atoms (gain/lose) ionic charges on the atoms - why?
gain, because the number of electrons do NOT equal # of protons anymore
42
___ = ions that gained electrons and thus a ___ charge
Anion, negative
43
Elements ending with ' -ide ' in name are identified as ____
Anions
44
Cations are ions that have ____ electrons and become more positive
lost
45
Covalent bonding: Atoms ___ electrons with other ___
share, atoms
46
Covalent bonding: Much ____ and more ____ than ____ bonding
stronger, common, ionic
47
Covalent bonding: atom contributes how many electrons to each other atom
at least 1, 2 or three
48
Covalent bonding: Why does it happen?
- Atoms generally have between 2-6 valence atoms | - harder to fill just by electron transfer
49
Covalent bonding: allows for very large, ____ ____ to form
stable molecules
50
Three compound mixtures
- Solution - Solute - Solvent
51
Compound mixtures: Solution
liquid, solid, or gas - made up of different molecules
52
Compound mixtures: ____ = substance dissolved in another
Solute
53
Compound mixtures: ____ = the liquid that solutes dissolve in
Solvent
54
Two types of classifications for compounds in chemistry
Organic, Inorganic
55
Organic compounds are anything that contains =
CARBON
56
Examples of organic compounds
biomocules > glucose, fats/lipids, proteins
57
____ Compounds that does NOT contain CARBON
inorganic
58
Examples of inorganic compounds
salt, water, many other salts/acids

Bio190 (3 decks)

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