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Level 3: Chemistry > Chapter 1 > Flashcards

Chapter 1 Flashcards

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1
Q

Atomic Structure

A
  1. Dalton - Solid Spheres
  2. Thomson - Electrons
  3. Rutherford - Nucleus
  4. Chadwick - Neutrons
  5. Bohr - Energy Levels
  6. Schrödinger - Electron Clouds
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2
Q

Octet Rule

A
  • Atoms are stable when the valence shell is full
  • For many common elements they are stable with 8 electrons so this is generalized with the octet rule
  • Atoms will form bonds or ions to achieve a complete valence shell
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3
Q

Cations

A

+

  • Cations form when an atom loses its electrons
  • Metals form cations
  • The energy required to “lose” an electron is called ionization energy
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4
Q

Anions

A

-

  • Anions form when electrons are gained by an atom
  • Non-metals form anions
  • The energy released with the electron is called electron affinity
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5
Q

Isoelectronic

A

When atoms form ions, they often have a “noble gas-like” arrangement and atoms/ions end up with the same number of electrons. This is called isoelectronic.

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6
Q

Isotopes

A
  • A form of an element in which the atoms have the same number of protons but a different number of neutrons. So they have different masses
  • You can determine the isotopic abundance of a sample using a mass spectrometer.
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7
Q

Radioactive Decay

A

Radioactive Decay is the spontaneous disintegration of an unstable isotope

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8
Q

Nuclear Radiation

A

Nuclear Radiation is energy or small particles emitted from a radioisotope as it decays

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9
Q

Radioisotopes

A

Radioisotopes is an isotope that spontaneously decays to produce 2 or more smaller nuclei and radiation

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10
Q

Radioactive

A

Radioactive means that a substance has the potential to emit nuclear radiation on decay

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11
Q

Types of Radiation

A

Alpha Particle - a positive charged particle with the same structure as the helium particle
Beta Particle - a negative charged particle that is identical to an electron
Gamma Ray - a form of high-energy particle electromagnetic radiation emitted by some radioisotopes

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12
Q

Equations

A

Check document

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13
Q

Determining Atomic Mass of Elements

A

Atomic mass = (% abundance of isotope 1 x mass of isotope 1) + (% abundance of isotope 2 x mass of isotope 2) / 100

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14
Q

Groups

A
  • Elements show similar chemical properties

- Elements show similar trends in their chemical properties

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15
Q

Periods

A
  • As you move across periods, changes in the chemical and physical properties that are repeated in the next period
  • This is what “period” and “periodic” refers to
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16
Q

Physical Properties

A 
Identify and explain the trends in the physical properties of the first 20 elements including:
Atomic radius
Ionic radius
First ionization energy
Electronegativity
Melting point
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17
Q

Atomic Radius

A
  • This is the size of the atom
  • There is no simple measure as atoms do not have a well defined “edge”
  • We use the: covalent radius
    • This is half the distance between the nuclei of two atoms in a covalent bond
    • This means we do not have values for the noble gases as they do not form bonds
  • The main factors influencing atomic radius are:
    • Number of shells (the principal quantum number)
    • The charge of the nucleus
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18
Q

Periodic Trends - Atomic Radius

A
  • Bottom-left - large atomic radius

- Top-right - small atomic radius

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19
Q

Ionic Radius

A
  • This is the “size” of an ion and is measured in a similar way to atomic radius
  • The main factors influencing ionic radius are:
    • Number of shells (the principal quantum number)… don’t forget this can be affected by the type of ion formed
    • The charge of the nucleus
20
Q

Periodic Trends - Ionic Radius

A
  • Positive ions
    • Smaller than the ion they are derived from (Na bigger than Na+)
  • Isoelectronic positive ions
    • More protons, smaller radius, pull in electrons
  • Negative ions
    • Bigger than the ion they are derived from (Cl smaller than Cl-)
  • Isoelectronic negative ions
    • More protons, smaller radius, pulls in electrons
21
Q

First Ionization Energy

A
  • This is the energy required to remove one mole of electrons from one mole of gaseous atoms to form positive ions
    • Ex: Ag (g) → Ag+ (g) + e-
  • Values are positive because this is an endothermic process
  • Values are influenced by:
    • Number of inner electron shells (and their shielding)
    • Charge on the nucleus
22
Q

Periodic Trends - First Ionization Energy

A
  • Lower ionization energy in lower left corner

- Higher ionization energy in upper right corner

23
Q

Electron Affinity

A
  • Define as the enthalpy change when an electron is added to an isolated atom in the gaseous state
    • Ex: X (g) +e- → X- (g) measured in KJ mol-1
24
Q

Periodic Trends - Electron Affinity

A
  • Lower electron affinity in lower left corner

- Higher electron affinity in upper right corner

25
Q

Electronegativity

A
  • This is a measure of the degree to which an element attracts the shared oaur if electrons in a covalent bond
    • Again, this means there are no values for the noble gases
  • Values range over:
    • 4.0 for Fluorine
    • 0.7 for Francium
  • Values are influenced by
    • Number of inner electron shells (and their shielding)
    • Charge on the nucleus
26
Q

Periodic Trends - Electronegavity

A
  • Lower electronegativity in lower left corner

- Higher electronegativity in upper right corner

27
Q

Melting Point

A
  • This is the temperature (in Kelvin… i.e. Celsius +273) at which an element melts
  • Values are influenced by:
    • Nature of bonding: giant covalent, giant ionic metallic
    • Strength of bonding
    • Strength of intermolecular forces
28
Q

How Ionic Compounds Form

A
  • Metals lose their electrons to form positive ions
  • Nonmetals gain electrons to form a negative ion
  • The + ion and the - ion are held together by an electrostatic force. We call this an ionic bond
29
Q

Ionic bond

A

Electrostatic attraction between two oppositely charged ions

30
Q

Naming Binary Ionic

A

Compounds

The name of the metal come first, non-metal ending changes to “ide”

31
Q

Writing Formulas - Use the Criss-Cross

A

Look up charges on PT. Write them as superscripts, criss-cross (reduce if necessary) to get subscripts.

32
Q

Naming Multivalent Metals

A

Need to use Roman Numerals to indicate which form of the metal is being used

33
Q

Writing Formulas for Multivalent Metals

A

Use the charge given in the Roman Numerals and use the criss-cross rules

34
Q

Hydrates

A
  • Have water as part of its crystal structure

- Provide the name of the ionic compound, then use prefixes from covalent compounds to indicate the number of “hydrate”

35
Q

Polyatomic Ions

A

An ion that has more than one element bonded together

36
Q

Important Polyatomics (Need to Know)

A 
NO3 - → nitrate
SO4 2- → sulfate
OH - → hydroxide
PO4 3- → phosphate
CO3 2- → carbonate
NH 4+ → ammonium
37
Q

Naming Ionic Compounds with Polyatomic Ions

A
  • Name the metal (use Roman Numerals if necessary) and then the name of the polyatomic ion from the cart… don’t change the ending
    • Note ammonium would come first because it’s positively charged and then the non-metals would change to -ide
38
Q

Writing Formulas with Polyatomics

A

Put the polyatomic ion in brackets, use the criss-cross method. Leave the polyatomic in brackets if there is a subscript

39
Q

Covalent Bonds Make Molecular Compounds

A
  • When the nuclei of two atoms are both attracted to one or more pairs of shared electrons, the electrostatic attraction is called a covalent bond
40
Q

Covalent bond

A
  • Electrostatic attraction between the nuclei of two atoms and one/more shared pair(s) of electrons
41
Q

Multiple Bonds

A
  • Sometimes, atoms can share more than one pair of electrons between each other. This can result in double and triple bonds
42
Q

Molecular Elements

A
  • A pure substance composed of molecules made up of two or more atoms of the same element
  • Most common are our diatomic elements (BrOHFINCl)
    • Suffixes -gen and -ine are diatomic elements
43
Q

Molecular Compounds

A
  • Compounds made up of two or more nonmetals

- H2O → 1 x 2 + 6 = 8 e-

44
Q

Naming Molecular Compounds

A
  • Use the prefixes (except we don’t use mono on the first element)
  • No change to the first element and the ending of the second element changes to -ide
45
Q

Writing Formulas

A
  • The prefixes tell you the numbers (DO NOT CRISS-CROSS)
46
Q

Rules for Drawing Lewis Structures

A
  • Add up the valence electrons for all the elements involved
    • If there is a - charge add the appropriate number of electrons
    • If there is a + charge subtract the appropriate number of electrons
  • Arrange the atoms evenly around the central atom
  • Start with a single bond between each element
  • Fill the octet of the outer elements (remember some just need 2)
  • Then fill the central atom octet… you may need to use double or triple bonds!
    • Just don’t exceed 8 electrons around each atom
47
Q

So how do we determine if a substance contains covalent or ionic bonds?

A
  • EN diff
  • We need to calculate the electronegativity difference
    • 0.0 → 0.4 = pure covalent bond
    • 0.4 → 1.8 = polar covalent bond
    • 1.8 → 4.0 = ionic bond

Level 3: Chemistry (2 decks)

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