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Thanatochemistry > Atomic structure and radiation chemistry > Flashcards

Atomic structure and radiation chemistry Flashcards

1
Q

Refer to the number of valance electrons in an atom.

A

Groups (vertical columns)

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2
Q

Electrons on the outermost shell.

A

Valance electrons

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3
Q

16O, 17O and 18O

A

Three stable isotopes of oxygen

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4
Q

Tells you how many shells an element has.

A

Horizontal row

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5
Q

Atoms that tend to give away electrons to other atoms.

- groups I, II and III

A

Electropositive

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6
Q

Electron greedy, tend to pull electrons from other elements.

- groups V, VI and VII

A

Electronegative

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7
Q

When the valance shell is full, the element is stable and is :

A

Not reactive

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8
Q

When the valance shell is incomplete, the element is:

A

Reactive - it wants to donate, receive or share electrons with other elements.

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9
Q

These are located on the far right of the periodic table of elements and have full outer electron shells (not reactive).

A

Nobel gases

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10
Q

Matter can neither be created nor destroyed.

A

Law of conservation of energy

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11
Q
  • Covalent bonding
  • 1 or more different atoms.
  • Usually smaller
  • Always covalent bonding
  • Same or different types of atoms involved
A

Molecules

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12
Q
  • Can be ionic or covalent bonding

- Must always be two different atoms involved.

A

Compounds

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13
Q

Involve the attraction of opposite electrical charges.

  • One atom donates an electron to another atom, making both atoms ions.
  • The opposite charges created become attracted to one another
  • Molecules composed of these are most stable as crystals.
A

Ionic bonds

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14
Q

Elements that have an electrical charge.

- By either gaining or losing electrons

A

Ions

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15
Q

Positively charged ions.

A

Cations

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16
Q

Negatively charged ions.

A

Anions

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17
Q

Form between two atoms when they share electrons.

  • number of electrons shared varies depending on how many the atom needs to fill its outermost electron shell.
  • Stronger than ionic bonds.
A

Covalent bonds

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18
Q

Equal sharing of electrons.

- Hydrophobic

A

Non-polar covalent bonds

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19
Q

Unequal sharing of electrons.

  • Hydrophilic
  • The nucleus that spends more time with the electron will have a partial negative charge, the one spending less time has a positive partial charge.
  • High electronegativity = more likely to form this kind of bond.
A

Polar Covalent bonds

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20
Q

Shorthand representation of the full name of an element.

A

Symbols

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21
Q

A group of ions that function as a single like a single atom.
- do not split them up

A

Polyatomic ions

22
Q

Represent the number of atoms in the molecule in the formula.
- when there is no number, assume it is 1.

A

Subscript

23
Q

Represents the charge of an atom in a formula.

A

Superscript

24
Q

Help keep track of electrons that are lost or gained.

  • The sum of these in a compound is 0.
  • The sum of these in polyatomic ions is equal to the charge of the ion.
A

Oxidation numbers

25
Q

Elements that have two oxidation numbers. (especially true for transition metals)

A

Bivalent

26
Q

Determined by adding up the atomic mass of each atom in the formula.

A

Molecular mass (formula weight)

27
Q

In a compound containing a metal and polyatomic ion, this is named first, and then this is named second.

A

The metal is named first, the polyatomic ion is second.

28
Q

In a compound containing a metal and one other non metal, this is named first, and then this is named second and given the suffix -ide.

A

The metal is first, the non-metal is second and given the suffix -ide

29
Q

Usually in the case of oxides, this number will influence the naming of the compound.
- Number prefix + name of the 1st element (usually the metal) + number prefix of the second element + ide suffix.

A

The subscript number.

30
Q

This suffix is used for the bivalent compound with the lower oxidation number.

A

Ous

31
Q

This suffix is used for the bivalent compound with the higher oxidation number.

A

-Ic

32
Q

copper is changed to this when naming for the high or low number.

A

Cupr - ous or ic

33
Q

Iron is changed to this when naming for the high or low number.

A

Ferrous or ferroic

34
Q
  • Cu (copper) +1 or +2
  • Hg (mercury) +1 or +2
  • Fe (iron) +2 or +3
A

Bivalent elements

35
Q

When atoms or molecules interact to form new molecules.

A

Chemical reaction

36
Q

The abbreviation for the chemical change.

A

Chemical equations

37
Q

The process of building or breaking chemical bonds.

A

Chemical reactions

38
Q

The forming of a new compound from two or more reactants.

A

Synthesis equations

39
Q

Represent reactions where a compound is broken down into the simpler parts that made it.

A

Decomposition equations

40
Q

1 ionic compound and 1 element are mixed together.

  • The element will replace an ion in the ionic compound and release the other ion.
  • If the element is + charged, it will replace the cation, if it is - charged, it will replace the anion.
  • Results in two new compounds.
A

Single replacement reactions

41
Q 
Represent neutralization (as in acids and bases) and hydrolysis.
- Two compounds as reactants and two different compounds as products when you are done.
A

Double replacement reactions (metathesis)

42
Q

Nuclear change, the decay in the nucleus of an atom.

A

Radioactivity

43
Q

Two protons and two neutrons decaying from the nucleus of an atom.
- Stopped by a piece of paper.

A

Alpha Radiation

44
Q

An electron is emitted or a positron is emitted.

- Stopped by a thin sheet of metal.

A

Beta radiation

45
Q

Usually emitted during alpha or beta decay (as wavelengths)

- Most damaging, requires thick lead to stop it.

A

Gamma rays

46
Q

The amount of time that it takes for half of the initial amount of radioactive material to decay
- The longer this is, the more stable the radioactive compound is- meaning it hangs around longer.

A

Half Life

47
Q

The result of building or breaking chemical bonds.

- The end result of a reaction.

A

Product

48
Q

Atoms or molecules that will interact.

A

Reactant

49
Q

Carries enough energy to ionize or rip electrons from an atom.
- Shorter wavelength and higher in energy.

A

Ionizing radiation

50
Q

The process of making an ion. (donating or receiving electrons).

A

Ionization

51
Q
  • Time
  • Distance
  • Shielding
A

Protecting yourself from radiation

Thanatochemistry (12 decks)

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