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Science 10-1 PIB > Chemistry > Flashcards

Chemistry Flashcards

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1
Q

Atomic Models in Chronological Order

A
  1. John Dalton
  2. J.J. Thompson
  3. Ernest Rutherford
  4. Niels Bohr
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2
Q

What Expirenment Did J.J. Thompson Perform To Create His Model

A

Cathode Ray Tube Experiment
- Glass Tube (vacuum inside) containing negatively-charged electrode (cathode) and a positively-charged electrode (anode)
- Two oppositely-charged plates and magnets were placed around the cathode ray
- Cathode rays were attracted to the positively-charged plate, indicating that the cathode rays were negatively-charged

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3
Q

Difference Between John Dalton’s and J.J. Thompson’s Atomic Model

A

J.J. Thompson’s atomic model had electrons

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4
Q

What Expirenment Did Ernest Rutherford Perform To Create His Model

A

Gold Foil Experiment
- Alpha particles were shot at gold foil
- Most went straight through – Indicating the atom was mostly empty space
- Some were deflected – Indicating that there was a small, dense, positively-charged nucleus at the center of the atom

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5
Q

Difference Between J.J. Thompson’s and Ernest Rutherford’s Atomic Model

A

Ernest Rutherford’s atomic model had an electron orbit, most the atom was empty space, and a nucleus

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6
Q

What Expirenment Did Niels Bohr Perform To Create His Model

A

Atomic Line Spectra Experiment
- A diffraction grating can be used to separate light into its component wavelengths
- When a hot gas was used with a diffraction grating, it emitted particular lines of light (emission spectrum). When the same gas was cooled, it absorbed the same lines of light (absorption spectrum)
- Shows the electron structure of an atom is quantized and electrons can emit or absorb energy in the form of photons to move between energy levels

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7
Q

Difference Between Ernest Rutherford’s and Niels Bohr’s Atomic Model

A

Electrons orbit the nucleus in energy levels, electrons can jump between energy levels

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8
Q

Alkali Metals Properties

A
  • Most reactive metals
  • Not found freely in nature
  • React with air and moisture
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9
Q

Alkaline-Earth Metals Properties

A
  • 2 valence electrons
  • Highly reactive
  • Low electronegativity
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10
Q

Transition Metals Properties

A
  • Good conductors of heat and electricity
  • High melting points
  • Unreactive
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11
Q

Halogens Properties

A
  • High electronegativity
  • Most reactive non-metals
  • All form acids when combined with hydrogen
  • Have 7 valence electrons
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12
Q

Noble Gases Properties

A
  • Almost non-reactive (stable octet)
  • Very low electronegativities
  • Low boiling points
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13
Q

Subatomic Particles

A

Electron:
- 1- charge, no mass (0 amu)
- Found outside the nucleus
Proton:
- 1+ charge, 1amu
- Found inside the nucleus
Neutron:
- No charge, 1amu
- Found inside the nucleus

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14
Q

What charge does an ATOM have

A

An atom is electrically neutral, the number of protons and electrons are the same

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15
Q

How to find the number of protons in an atom

A

Atomic number = number of protons

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16
Q

How to find the number of neutrons in an atom

A

Mass number - number of protons (atomic number)

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17
Q

How to find mass number

A

Number of protons + number of neutrons

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18
Q

Isotopes

A

Different number of neutrons

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19
Q

Atomic Mass

A

Average mass of all isotopes

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20
Q

Bohr Model Diagrams

A
  • 1’st energy level can have 2 electrons
  • 2’nd and 3’rd energy can have 8 electrons
  • 4’th energy level can have 18
  • For the first energy level, place 2 electrons in the North position
  • 2’nd to 4’th energy level, place single electrons North to West, then pair up electrons going North to West
  • Bohr Model Diagrams are only used for the first 20 elements
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21
Q

Groups and Periods

A

Groups are horizontal, Periods are vertical

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22
Q

Stable Octet

A

Full valence energy level

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23
Q

Valence Electrons

A

Electrons found in the outermost occupied energy level

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24
Q

Cation

A
  • Lost electrons
  • More protons than electrons
  • Positively charged
  • Can only be formed by metals
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25
Q

Anion

A
  • Gained electrons
  • More electrons than protons
  • Negatively charged
  • Can only be formed by non-metals
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26
Q

Ionic Compounds

A

Form when an electron or electrons are transferred from a metal to a non-metal
- Electrically neutral because the ions always occur in such a ratio

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27
Q

Ionic Bond

A

The electrostatic attraction between the cations and anions in an ionic compound

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28
Q

Polyatomic Ionic Compounds

A

Ionic compounds in which one or both of the ions are polyatomic

29
Q

Molecular Compounds

A
  • Form when electrons are shared between two non-metal atoms
  • Atoms are linked together in very tiny, discrete, electrically neutral particles called molecules
30
Q

Covalent/Molecular Bond

A
  • A chemical bond that involves the sharing of pairs of electrons between atoms
31
Q

3 Types of Covalent Bonds

A
  • Single Bond - Sharing of one pair of electrons
  • Double Bond - Sharing of two pairs of electrons
  • Triple Bond - Sharing of three pairs of electrons
32
Q

7 Diatomic Elements

A
  • Hydrogen - Chlorine
  • Nitrogen - Bromine
  • Oxygen - Iodine
  • Fluorine
32
Q

2 Polyatomic Elements

A
  • Phosphorus
  • Sulfur
33
Q

Molecular Structure

A

The three-dimensional structure or arrangement of atoms in a molecule

34
Q

Vespr Theory

A

A model used to predict the molecular shape from the Louis structure
- According to VESPR, electron pairs repel each other
- Lone pairs repel more than bond pairs

35
Q

Electronegativity

A

The relative attraction of an atom for the electrons in a bond
- Increases Bottom to Top and Left to Right

36
Q

Non-polar covalent bond

A

In a covalent bond between identical atoms, the bonding pair of electrons is shared equally
Eg. Diatomic elements

37
Q

Polar covalent bond

A

A covalent bond between non-identical atoms with different electronegativities, where the bonding electron is shared unequally

  • The unequal sharing gives the bond partial positive and partial negative poles
38
Q

Molecular Polarity

A

The overall distribution of electronic charge in a molecule
- Opposite Molecular Polarities, eg. CO2 cancel each other out, making the overall molecule nonpolar

39
Q

Properties of Ionic Compounds

A
  • Solid at room temperature
  • High melting points
  • Hard and brittle
  • Some are soluble (use solubility table)
  • Don’t conduct electricity in solid state
  • Conduct electricity in liquid form
40
Q

Properties of Molecular Compounds

A
  • Lower melting points
  • State depends on size (water is an exception due to hydrogen bonding)
  • Solubility depends on the polarity of the molecular compound
  • Don’t conduct electricity in any state
41
Q

Electrolytes

A

Aqueous solutions that conduct electricity

42
Q

Nonelectrolyte

A

Aqueous solution that doesn’t conduct electrcity

43
Q

Acids

A

Molecular compounds that contain a covalently bonded H atom
- Have a hydrogen cation

44
Q

Bases

A

Ionic compounds that contain a OH (hydroxide) ion
- Have a hydroxide anion

45
Q

pH of Ionic and Molecular compounds

A

Ionic and Molecular compounds both have a pH of 7

46
Q

Physical Change

A

When a substance undergoes a change in its physical form, but the chemical composition stays the same

47
Q

Chemical Change

A

When a substance undergoes a change in its chemical composition resulting in the formation of a new substance

48
Q

Evidence of a Chemical Change

A
  • Energy Change
  • Formation of a Gas
  • Formation of a Precipitate
  • Color, odour, or temperature change
49
Q

System

A

Part of the universe we focus on

50
Q

Surroundings

A

Everything in the universe except the system

51
Q

Boundary

A

What separates the system from its surroundings

52
Q

Law of Conservation of Energy

A

The energy of the universe is constant; it can be neither created nor destroyed, but only transferred and transformed

53
Q

Chemical potential energy

A

The energy stored in the chemical bonds that hold compounds together

53
Q

Chemical potential energy

A

The energy stored in the chemical bonds that hold compounds together

54
Q

Law of Conservation of Mass

A

Matter in a closed or isolated system is constant; it can neither be created, but only rearranged into different combinations or forms

55
Q

Balancing Combustion Reactions

A
  1. Balance hydrogen so that the H2O coefficient is a even number
  2. Balance Carbon
  3. Balance Oxygen
56
Q

Endothermic Reaction

A

Energy is absorbed from the surroundings

57
Q

Exothermic Reaction

A

Energy is released into the surroundings

58
Q

Formation (Synthesis) Reaction

A

Two elements combine to form a compound
- A + B => AB

59
Q

Decomposition Reaction

A

A compound is broken down into elements
- AB => A + B

60
Q

Single Replacement Reaction

A

A compound reacts with an element to produce a new compound and a new element
- Either a metal will replace the metal cation in a ionic compound
- A non-metal will replace the non-metal anion in a ionic compound
- Often take place in aqueous solutions
- AB + C => AC + B

61
Q

Double Replacement Reaction

A

Two compounds react to produce two new compounds
- Often occur between two ionic compounds and take place in aqueous solutions
- The cation of the first ionic compound replaces the cation of the second ionic compound
- AB + CD => AD + CB

62
Q

Precipitation Reaction (Double Replacement)

A

A chemical reaction in which two soluble ionic compounds form an insoluble product, a precipitate

63
Q

Neutralization Reaction (Double Replacement)

A

Special kind of double replacement reaction that occurs when an acid or base react to produce a neutral ionic salt and water

64
Q

Hydrocarbon Combustion Reaction

A

A hydrocarbon fuel (CₓHᵧ) is burned in the presence of oxygen to produce carbon dioxide and water vapor
- Always exothermic, so the water is released as a gas

65
Q

Incomplete Combustion Reaction

A

Occurs when there is a poor supply of oxygen, results in carbon monoxide being released instead of carbon dioxide

66
Q

Mole

A

6.02 x 10²³

67
Q

Molar Ratios

A

Ratio between the amounts in moles of any two compounds involved in a balanced chemical reaction

Science 10-1 PIB (5 decks)

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