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Perryland Chemistry - Theory (2005 Standards) > Midterm > Flashcards

Midterm Flashcards

1
Q

The three types of radiation and their penetration abilities:

A
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2
Q

Properties of Ionic Compounds

A

Crystalline Structure High Melting Point Rigid Strong Bond Conduct Electricity (when dissolved or melted) Good Insulators

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3
Q

Conductor

A

A material which permits the flow of energy. A material which allows the flow of charged particles is an electrical conductor. A material which allows the transfer of thermal energy is a thermal conductor or heat conductor.

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4
Q

Photon

A

Energy given off in the form of light by an excited electron. Otherwise known as a “quanta of light”.

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4
Q

Charge of Group 2 or 2A (Be, Mg, Ca, Sr, Ba):

A

Charge = 2+

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5
Q

Sublevel

A

Principal energy levels are broken down into sublevels designated s, p, d, or f upon which electrons travel.

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5
Q

Proton

A

Positively charged subatomic particle. Contained inside the nucleus. Neutrons and Protons weigh roughly the same (1 atomic mass unit).

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5
Q

Cations

A

Positively Charged Ions. In general, cations are metals.

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6
Q

Hund’s Rule

A

When filling sublevels other than s, electrons are placed in individual orbitals before they are paired up.

Electrons fill like people do on a bus. You would never sit right next to someone you do not know if there are free seats available, unless of course all the seats are taken then you must pair up.

So, when working with the p sublevel, electrons fill like this…up, up, up….down, down, down…

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7
Q

Ionic Compound Formulas

A
  1. Metal written first Nonmetal written second 2. Use criss-cross method and subscripts to insure sum of charges = 0
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8
Q

Predict the element formed and write a balanced nuclear equation for the following statement:

Uranium-238 decays by alpha emission to form __________.

A
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8
Q

Anion

A

Negatively charged Ions. Anions are negatively charged because they have gained an electron(s) (electrons are negative). In general, anions are nonmetals.

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8
Q

Intramolecular Forces

A

Attractive forces WITHIN a molecule (Ionic & Covalent Bonds)

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10
Q

Fission

A
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11
Q

Radioactivity

A

When the nucleus of an atom becomes unstable and decays. This tends to happen to large atoms (larger than atomic number 83) becuase the number of protons to neutrons in the nucleus is unbalanced.

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11
Q

Naming Covalent Compunds

A

You DO NOT use the “criss-cross” method. Use prefixes. The only time you do not use a prefix is when there is only one of the first nonmetal. Remember : 1-Mono 2-Di etc…

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12
Q

Rules for Writing Lewis Dot Structures

A
  1. Total the Valence Electrons and Update during each step.
  2. Form a single bond between the central atom and each surrounding atom (each bond uses two electrons).
  3. Place electrons around the outer atoms until you run out or they each have eight electrons around them. (Hydrogen and Helium can only have two electrons around them).
  4. Place any remaining electrons around the central atom.
  5. Does each atom other than hydrogen have eight electrons around it?
  6. Rearrange (share) electrons so that all atoms other than hydrogen have eight electrons around them.
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13
Q

Orbital

A

Sublevels can be broken down into regions called “orbitals”. An orbital is defined as the most probable location for finding an electron. Each orbital holds 2 electrons.

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13
Q

Greek Prefixes used in nomenclature 1= 2 = 3 = 4= 5 = 6= 7= 8= 9= 10=

A

1= mono 2 =di 3 =tri 4=tetra 5 = penta 6=hexa 7=hepta 8=octa 9=nona 10=deca

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15
Q

Pauli Exclusion Principle

A

If there are two electrons in an orbital, they must have opposite (paired) spins.

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17
Q

Atomic Size

A

Size of an atom.

Depends on the number of energy levels and the overall charge of the nucleus (the nucleus’s charge depends on the number of protons).

As you go down a group you are adding energy levels (rings around the nucleus) so the atomic size increases.

As you go across a period the atomic size decreases because the energy levels (which contain negative electrons) are increasingly attracted to the positive protons in the nucleus of the atom.

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18
Q

Period

A

Horizontal row on the periodic table.

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19
Q

How to calculate neutrons:

A

of Neutrons = Atomic Mass Number - Atomic Number

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20
Q

Hydrogen

A

Group 1 Nonmetal

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20
Polar Covalent
A type of covalent bond between two atoms in which electrons are shared unequally. Because of this, one end of the molecule has a slightly negative charge and the other a slightly positive charge.
21
Fusion
22
Metals
To the left side of the periodic table (left of the zig zag line). Usually, solids at room temperature. Good conductors of heat and electricity. High melting and boiling points. Malleable. Ductile.
22
Transition Metals
22
Malleable
Able to be hammered or pressed permenately out of it's original shape without breaking or cracking.
22
Covalent or Molecular Compounds (Molecules)
The first word gives name of the element that appears first preceded by a prefix that shows number of atoms in that element. Do NOT use the prefix mono before the name of the first element. The second word consists of a prefix designating the number of atoms of that element, the stem name of the second element, and the suffix -ide.
23
Electrons
Negatively charged subatomic particles. Electrons can be found in the space around the nucleus. This area is often called the electron cloud. Electrons have NO mass.
24
Polyatomic Ionic Formulas
1. Metal written first, Polyatomic Ion is written second 2. Use criss-cross method and subscripts to insure sum of charges = 0 3. When using a subscript for polyatomic ions: place a parentheses around the polyatomic formula, put the subscript outside of the parentheses
26
Orbital Diagram
Shorthand method of writing the location of electrons by orbital.
27
Writing Formulas for Ionic Bonds
Absolute Value Criss Cross Oxidation #'s
28
Ions
Atoms or groups of atoms with a charge. To have a charge an atom must have gained or lost electrons. If an atom gains electrons it becomes negatively charged. If an atom loses electrons it will become positively charged.
30
Principle Energy Level
The possible locations around an atom where electrons having specific energy values (quantum number) may be found. Divided into sublevels s, p, d, and f.
31
Covalent/Molecular Bonding
Nonmetals SHARE electrons
32
Roman Numerals
Above groups/families Roman Numerals represent the number of valence electrons. When writing the name of an ionic compound which includes a transition metal a Roman Numeral is used to denote the quantity of positive charge associated with that transition metal.
33
Isotopes
Atoms of the same element which have a different Mass Number due to a differing number of neutrons. The symbol for an Isotope is the element symbol followed by the Mass Number, for example: Na-23 and Na-24
35
Half Life
The time it takes for the amount of a radioactive element to decay by half.
36
Charge of Group 1 or 1A (H, Li, Na, K, Rb, Cs):
Charge = 1+
38
Electron Configuration
A shorthand method of writing the location of electrons by sublevels.
38
Polyatomic Ion
Polyatomic Ions ions made up of more than one atom; acts as an individual ion in a compound; charge applies to entire group of atoms.
39
VSPER
Valence Shell Electron Pair Repulsion Most important aspect of determining the shape or geometry of a molecule. The molecule will adopt the shape which minimizes te electron pair repulsion.
40
Nucleus
The center of an atom. Contains the protons and neutrons. Since neutrons have no charge and protons are positively charged, the nucleus has an overall positive charge.
41
Charge of Group17 or 7A (F, Cl, Br, I)
Charge: 1-
42
Polyatomic Ion
A group of atoms that acts like an ion (has a charge)
43
Neutrons
Neutrally charged subatomic particle. (No charge) Contained inside the nucleus. Neutrons and Protons weigh roughly the same (1 atomic mass unit)
44
Octet Rule
All atoms other than hydrogen and helium bond to fill their valence shell with eight electrons.
46
Group or Family
Vertical Column on the periodic table. Elements in the same family have similar properties.
47
Naming Ionic Bonds
State the name of the metal followed by the nonmetal with the ending changed to "ide". If the metal is a transition metal, add a (Roman numeral). AlCl₃ = Aluminum Chloride CuCl₃ = Copper (III) Chloride
48
Violations of the Octet Rule
Be - 4 B - 6 P - 8 or 10 S - 8, 10, or 12 Xe - 8, 10, or 12
49
Ionic Compounds
two words, first names cation second names anion. Indicate charge of transition metal cation by Roman Numeral. MgCl₂ = Magnesium Chloride Cr(NO₃)₃ = Chromium(III) Nitrate SnCl₂ = Tin(II) Chloride
50
Charge of Group 16 or 6A (O,S, Se, Te):
Charge: 2-
51
Anions
Anions are named by adding the suffix -ide to the stem of the name of the nonmetal from which they are derived. N³⁻ = Nitride O²⁻ = Oxide F⁻ = Flouride
53
Duet Rule
Hydrogen bonds to fill it's valence shell with two electrons. Helium already has two electrons and thus does not need to form bonds to increase stability.
54
Oxidation Number
Ion Charge - number of electrons transferred to or away from an atom when it becomes an ion.
56
Metalloid
Have properties of both metals and nonmetals. Semiconductors.
57
Chain Reaction
58
Valence Electrons
Electrons found on the outer energy level. Represented by Roman Numerals. Transition Elements do not have Roman Numerals which denote their valence electrons.
60
Lone Pairs
Electron pairs which are not involved in bonding. They do however, affect the shape because electron pairs repel other electron pairs.
61
Electronegativity
Tendency of an atom to attract electrons to itself when it combines with another element. Electronegativity increases from left to right across a period on the periodic table. Electronegativiy decreases as you go down a group on the periodic table.
61
Ionic Bond
Metals GIVE electrons, Nonmetals TAKE electrons
62
What are both of the symbols for each of the following types of nuclear decay: Alpha, Beta, Gamma
64
Atomic Number
Identifies an element. The number of protons. For a neutral atom, the number of electrons will equal the number of protons. For an ion (charged atom) the number of electrons will not be the same as the atomic number.
65
Atomic Mass Number
Also known as the Mass Number or Atomic Mass.
66
Charge of Group15 or 5A (N, P, As):
Charge = 3-
68
Oxidation Numbers
In Order +1 +2 Break until Boron +3 +4 -4 -3 -2 -1 0 at Helium
69
Write the formula for Mg²⁺ and PO₄³⁻
Using the criss-cross method and subscripts to insure sum of charges is zero: Mg₃(PO₄)₂
70
Quantum of Energy
Absorbed when an electron moves from its ground state to its excited state.
71
Intermolecular Forces
Attractive forces BETWEEN molecules
72
Group/Family Names
73
Non Polar Covalent
A type of covalent bond between two atoms in which electrons are shared equally.
74
Ductile
Capable of being drawn out into a wire or thread.
75
Bond Pairs
Pairs of electrons which form a bond.
76
Nonmetals
To the right hand side of the periodic table (right of the zig zag line). Not good conductors. Low melting and boiling points. Brittle.

Perryland Chemistry - Theory (2005 Standards) (13 decks)

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