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Bio190 > Week 2 - Chemistry Part 1 > Flashcards

Week 2 - Chemistry Part 1 Flashcards

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?

A

Periodically

25
Q

The process of dating fossils and diagnosing medical disorders

A

Carbon dating

26
Q

Where do electrons orbit in an atom?

A

Orbit around the nucleus

27
Q

What is the Octet Rule

A

8 electrons can fill each shell

28
Q

How many electrons are able to be in the first shell?

A

Only 2!

29
Q

What is the outermost/most important shell?

A

Valence shell

30
Q

Lewis Dot Diagrams: Why are valence electrons the most improtant?

A

To figure out how many atoms pair up with other atoms

31
Q

Lewis Dot Diagrams: Electrons will always try to ___

A

Pair up

32
Q

Lewis Dot Diagrams: Lone electrons

A

= bad = free radical

- will try to find other atoms with other lone elctrons to pair them up

33
Q

Lewis Dot Diagrams: Define process of drawing

A
  • 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
Q

Lewis Dot Diagrams: Atoms want to have ____, ____

A

Complete variance shells! They have to find a buddy!

35
Q

Different methods of atom bonding

A
  • Ionic bonding
  • Covalent bonding
    - Polar
    - Non-polar
  • Weak interactions
36
Q

Bonding: Atoms will give or take electrons ‘electron transfer’

A

Ionic bonding

37
Q

Ionic bonding happens between ___

A

Ions = charged particles

38
Q

Why does ionic bonding happen?

A

Some atoms are really close to having filled Valence shells

39
Q

Atoms that have __ # of electrons prefer to ‘take’ an electron to become more ___

A

7, stable (filled shell)

40
Q

Atoms that ___ electrons do so to jump down to the next ____ valence shell

A

lose, lowest

41
Q

Transferring electrons in atoms (gain/lose) ionic charges on the atoms - why?

A

gain, because the number of electrons do NOT equal # of protons anymore

42
Q

___ = ions that gained electrons and thus a ___ charge

A

Anion, negative

43
Q

Elements ending with ‘ -ide ‘ in name are identified as ____

A

Anions

44
Q

Cations are ions that have ____ electrons and become more positive

A

lost

45
Q

Covalent bonding: Atoms ___ electrons with other ___

A

share, atoms

46
Q

Covalent bonding: Much ____ and more ____ than ____ bonding

A

stronger, common, ionic

47
Q

Covalent bonding: atom contributes how many electrons to each other atom

A

at least 1, 2 or three

48
Q

Covalent bonding: Why does it happen?

A
  • Atoms generally have between 2-6 valence atoms

- harder to fill just by electron transfer

49
Q

Covalent bonding: allows for very large, ____ ____ to form

A

stable molecules

50
Q

Three compound mixtures

A
  • Solution
  • Solute
  • Solvent
51
Q

Compound mixtures: Solution

A

liquid, solid, or gas - made up of different molecules

52
Q

Compound mixtures: ____ = substance dissolved in another

A

Solute

53
Q

Compound mixtures: ____ = the liquid that solutes dissolve in

A

Solvent

54
Q

Two types of classifications for compounds in chemistry

A

Organic, Inorganic

55
Q

Organic compounds are anything that contains =

A

CARBON

56
Q

Examples of organic compounds

A

biomocules > glucose, fats/lipids, proteins

57
Q

____ Compounds that does NOT contain CARBON

A

inorganic

58
Q

Examples of inorganic compounds

A

salt, water, many other salts/acids

Bio190 (3 decks)

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