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Chemisty > Unit 4 (Electron Configuration, Nomenclature, Energy Diagrams, Stoichiometry) > Flashcards

Unit 4 (Electron Configuration, Nomenclature, Energy Diagrams, Stoichiometry) Flashcards

1
Q

What’s the Quantam Model?

A

Current model of atom. Stated that electrons don’t exist in fixed orbits, but they do occupy regions of space called orbitals because electrons move very fast and are very small.

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2
Q

What is an orbital?

A

Region in space in which there is a high probability of finding an electron.

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3
Q

What are the 4 sublevels?

A

S (1 orbital, 2 electrons)
P (3 orbitals, 6 electrons)
D (5 orbitals, 10 electrons)
F (7 orbitals, 14 electrons)

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4
Q

What do the coefficients tell us?

A

Principle energy level (period #)

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5
Q

What does the exponent tell us?

A

Number of electrons

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6
Q

What does electron configuration give us?

A
  • the address for the atom in the PTOE
  • shows which principle energy levels are occupied
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7
Q

How can you tell if a substance is covalent?

A

All the elements would be non-metals

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8
Q

How can you tell if a substance is ionic?

A

It would have atleast on metal.

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9
Q

How do you name Ionic compounds?

A
  1. Write the cation before the anion
  2. Change the other element’s ending to “ide”
    *use the criss cross method for ionic compounds
    *oxidation state is represented by a roman number for transition metals
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10
Q

What are the prefixes?

A
  1. Mono
  2. Di
  3. Tri
  4. Tetra
  5. Pentra
  6. Hexa
  7. Hepta
  8. Octa
  9. Nona
  10. Deca

Mother, did the turkey pass Henry’s Heavy notioned diet?

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11
Q

How do you name Covalent compounds?

A
  1. Write the prefix for the first atom if there is more than one atom.
  2. A prefix and a suffix of “Ide” is added to the #2 element
    *NO CRISS CROSS
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12
Q

Why do polyatomic Ions occur?

A

The atoms in polyatomic Ions have a stable electron configuration full shell.

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13
Q

NO3

A

Nitrate

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14
Q

ClO3

A

Chlorate

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15
Q

OH

A

Hydroxide

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16
Q

CO3

A

Carbonate

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17
Q

SO4

A

Sulfate

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18
Q

SO3

A

Sulfite

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19
Q

PO4

A

Phosphate

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20
Q

PO3

A

Phosphite

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21
Q

NH4

A

Ammonium

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22
Q

What is Aufbau Principle?

A

FIll low to high energy levels.

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23
Q

What is Pauli Exclusion Principle?

A

There is a maximum of 2 electrons per orbital, and they must have opposite spin (electrons represented in up and down arrows)

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24
Q

What is Hund’s rule?

A

Electrons fill orbitals of p,d, or f sublevels must have one electron in each orbital before “doubling up”

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25
Q

What is a Covalent bond?

A

An electrostatic attraction between two nonmetals where electrons are SHARED.

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26
Q

Whats a Covalent compound?

A
  1. Between two nonmetals
  2. Made up of individual molecules
  3. Doesn’t dissociate, only break down to molecules (ex: sugar covalent compound)
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27
Q

What is the Lewis Dot Diagram/Structure?

A

A visual representation of an atoms valence electrons.

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28
Q

What is an ion?

A

A charged particle that has loosed or gained an electron.
2 types: anion (negative), cation (positive)

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29
Q

What happens in Ionic bonds?

A

Electrostatic attractions that binds oppositely charged icons (metals and non-metals). Electrons are EXCHANGED

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30
Q

What are Ionic compounds?

A

Composed of positive and negative ions stuck together by Ionic bonds (Yin Yang)

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31
Q

Why do bonds form?

A

All atoms want to be as stable as possible (filled/full energy levels)

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32
Q

What happens when an ionic compound is placed in water?

A

The ionic compound disassociates and dissolves. (new ionic compounds form) ex: salt in water

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33
Q

What are electrolytes?

A

Ionic Solutions (can conduct electricity)

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34
Q

What are the steps for Balancing Chemical Equations?

A
  1. Determine the correct formulas for the productions and reactants.
  2. Determine the number of atoms of each element in the reactants and products.
  3. Balance the elements on at a time by using coefficients.
  4. Make sure all coefficients are in the lowest possible ratio.
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35
Q

What do chemical bonds contain?

A

Potential energy (stored energy) To break bonds energy must be absorbed (endo)

36
Q

What is an Energy Diagram?

A

Displays the energy that is added or released into a system during a chemical reaction

37
Q

What is the y and x axis on an Energy Diagram?

A

y-axis: energy
x-axis: progress/time

38
Q

Where is the activated complex on an Energy Diagram?

A

The highest point on the curve (peak)

39
Q

What is Activation Energy and it’s symbol?

A

Ea - the energy necessary to break bonds in the reactants so a chemical reaction can occur/ to reach the activation complex.

40
Q

What is collision theory?

A

Atoms ions and molecules can react to form products when they collide.

41
Q

What is Enthalpy?

A

The measure of heat in a system.

42
Q

If the reactants have more energy then the products then what type of reaction is it?

A

Exothermic with a lower activation energy

43
Q

if the reactants have a lower energy than the products then what type of reaction is it?

A

Endothermic with a higher activation energy

44
Q

For chemical equations to be useful, qualities of reactants and products must be what?

A

Measurable

45
Q

What is Stoichiometry?

A

Stoichiometry allows for the quantification of chemical relationships. It shows the relationship between masses of elements in compounds or between the reactants and products of chemical reactions. (mole to mole ratio)

46
Q

What is the mole to mole ratio?

A

Another conversion factor derived from balanced chemical equations (Stoichiometry)

47
Q

How do you draw a model for a balanced equation?

A

Arrows and make sure to use BrINClHOF

48
Q

Does the oxidation state number effect how you write it’s electron configuration?

A

Yes subtract the lost electrons or add the gained electrons and then use the new number when writing the electron configuration.

49
Q

What does it mean for an atom to be in a ground state?

A

All of its electrons are in the lowest available energy levels.

50
Q

What are principle energy levels(n)?

A

specific distances from the nucleus (rings)

51
Q

What does the period (row) correspond to?

A

The highest energy level occupied by the valence electrons in an element (row=ring)

52
Q

What does the group/family (column) correspond to?

A

The number of valence electrons in an element.

53
Q

What are valence electrons and why are they so important?

A

The outermost electrons in an atom. They are the electrons that are involved in chemical reactions and determine the element’s chemical properties.

54
Q

What is an oxidation number/state?

A

The total number of electrons that an atom either gains or loses in order to form a chemical bond with another atom.

55
Q

What does it mean for an atom to be in an excited state?

A

Electron absorbs energy and jumps to a level of higher energy.

56
Q

What is a formula unit?

A

The chemical formula of an ionic compound that lists the ions in the lowest ratio that equals a neutral electrical charge.

57
Q

What is dissolving?

A

A physical change that involves heat. (dissolving and dissociation can be represented by an equation)

58
Q

What is conductivity?

A

the transfer of energy through contact with a material or materials.

59
Q

What is nomenclature?

A

the process of naming chemical compounds with different names so that they can be easily identified as separate chemicals.

60
Q

What is BrINClHOF?

A

(pronounced “Brinklehoff”) lists all of the diatomic elements in the name.

61
Q

What does aqueous (aq) mean?

A

dissolved in water

62
Q

What is a solution?

A

a homogeneous mixture made up of very tiny particles (molecules, atoms, ions)

63
Q

What is group 18?

A

Noble gases (all non metal, unreactive, colorless, odorless) filled valence shell.

64
Q

What are groups 3-12?

A

Transition metals (moderate range or reactivity, wide range of properties, usually shiny, good conductors of heat and electricity).

65
Q

What is the octet rule?

A

Completely filled energy level (8 valence electrons in the valence shell). Ions want to achieve this in order to be stable.

66
Q

What is molar mass?

A

The mass of one mole of any element in grams (the same as atomic mass but with a unit)

67
Q

What is Mole used for?

A

A standard scientific unit for measuring large quantities of very small entities such as atoms, molecules, particles.

68
Q

What is Avogandro’s Number?

A

the number of atoms contained in one mole, 6.02 x 1023

69
Q

What are endothermic reactions?

A

absorbs heat
bonds broken
making substance warmer with kinetic energy

70
Q

What are exothermic reactions?

A

release energy (as heat)
bonds formed
making substance cooler with potential energy

71
Q

Whats the correct name for SnCl2

A

tin(II) chloride

72
Q

Cu2SO3

A

copper(I) sulfite

73
Q

MgCO3

A

magnesium carbonate

74
Q

barium sulfate

A

BaSO4

75
Q

tin(II) hydroxide

A

Sn(OH)2

76
Q

aluminum nitrate

A

Al(NO3)3

77
Q

CoSO3

A

cobalt(II) sulfite

78
Q

RbF

A

rubidium fluoride

79
Q

Be3(PO4)2

A

beryllium phosphate

80
Q

When do you use the crisscross method for covalent compounds?

A

Never! Covalent compounds use the prefix system only.

81
Q

What is Irons symbol?

A

Fe

82
Q

What is Silvers symbol?

A

Ag

83
Q

What is Golds symbol?

A

aU

84
Q

What is Tins symbol?

A

Sn

85
Q

What is Bismuths symbol?

A

Bi

86
Q

What is Leads symbol?

A

Pb

87
Q

Whats Sodiums symbol

A

Na

Chemisty (16 decks)

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