Brainscape's Knowledge GenomeTM

Browse over 1 million classes created by top students, professors, publishers, and experts.


See full index

(SLU) PHARMA 113: Chem Lec > UNIT 5 > Flashcards

UNIT 5 Flashcards

You may prefer our related Brainscape-certified flashcards:
Periodic Table flashcards Chemistry 101 flashcards AP® Chemistry flashcards Organic Chemistry 101 flashcards
1
Q
  • swedish scientist who introduced the modern system of chemical symbols
  • represented the elements using one or two letters from their Latin names.
A

Jöns Jakob Berzelius

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
2
Q
  • shorthand ways to represent elements in chemistry.
  • an element cannot be broken down into simpler substances.
A

chemical symbols

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
3
Q

Importance of Chemical Symbols

A
  • provide standardised ways of representing elements, making communicating information about elements and compounds easier.
  • offer a concise and simple way to represent elements in chemical equations, eliminating the need to spell each element’s name.
How well did you know this?
1
Not at all
2
3
4
5
Perfectly
4
Q
  • Derived from the Greek ‘hydro’ and ‘genes’, which means water forming
  • Most abundant element in the universe
A

Hydrogen

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
5
Q
  • Name comes from the Greek ‘oxy’ and ‘genes’, which means acid forming
  • Essential for life
A

Oxygen

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
6
Q
  • Derived from the Latin ‘carbo’, meaning charcoal
  • Found in all known life forms
A

Carbon

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
7
Q
  • Comes from the Greek ‘nitron’ and ‘genes’, meaning nitre forming
  • Constitutes about 78% of Earth’s atmosphere
A

Nitrogen

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
8
Q
  • Derived from the Latin ‘natrium’
  • Soft metal that easily tarnishes when exposed to air
A

Sodium

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
9
Q
  • Name derived from the Greek ‘chloros’, which means greenish yellow
  • Widely used in disinfectants and cleaning products
A

Chlorine

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
10
Q

often named based on their characteristics, the substances they were extracted from, how they were found, mythological beings, locations or notable individuals.

A

elements

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
11
Q

There are _____ chemical elements listed in the periodic table in a specific order.

Rules on how to name new elements in the periodic table are set up by the __________________.

A

118

International Union of Pure and Applied Chemistry (IUPAC).

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
12
Q
  • responsible for establishing unambiguous and consistent naming systems (also known as ___________) and terminology.
  • It has a system for naming chemical compounds that provides a standard language for scientists worldwide.
A

nomenclature

IUPAC

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
13
Q

____________: substance containing two or more elements that are chemically bonded.

____________: an expression showing the elements in a compound and their relative proportions. It contains a combination of chemical symbols and numbers.

A
  • compound
  • chemical formula
How well did you know this?
1
Not at all
2
3
4
5
Perfectly
14
Q

___________: composed of a metal and non-metal

RULES:
1. A metal will always come first in a chemical formula, followed by a non-metal.
* sodium chloride (NaCl)

  1. An ionic compound with two elements will have a name that ends with -ide.
    * copper sulfide (CuS)
  2. A compound with three elements, including oxygen, will have a name that ends with - ate
    or -ite.
    * sodium sulphate (NaSO₄)
A

ionic compound

NaCl
CuS
NaSO₄

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
15
Q

__________: has two or more non-metals.

RULES:
1. The non-metal furthest to the left on the periodic table comes first.
* carbon dioxide (CO₂)

  1. A covalent compound with two elements will have a name that ends with -ide.
    * sulfur dioxide (SO₂)
  2. Use the prefixes (mono-, di-, tri-, tetra-) to indicate the number of that element in the molecule.
    * carbon tetrachloride (CCl₄)
A

covalent compounds

CO₂
SO₂
CCl₄

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
16
Q

H2O

NH3

CH4

A

water

ammonia

methane

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
17
Q
  • potassium bromide
  • lithium iodide
  • carbon monoxide
  • sulfuric acid
  • potassium nitrate
A
  • KBr
  • LiI
  • CO
  • H2SO4
  • KN3
How well did you know this?
1
Not at all
2
3
4
5
Perfectly
18
Q

Latin Name

  • Potassium
  • Sodium
  • Silver
  • Gold
  • Iron
  • Lead
A
  • Kalium (K)
  • Natrium (Na)
  • Argentum (Ag)
  • Aurum (Au)
  • Ferrum (Fe)
  • Plumbum (Pb)
How well did you know this?
1
Not at all
2
3
4
5
Perfectly
19
Q
  • Mercury
  • Tungsten
  • Tin
  • Copper
  • Antimony
A
  • Hydrargyrum (Hg)
  • Wolfranium (W)
  • Stannum (Sn)
  • Cuprum (Cu)
  • Stibium (Sb)
How well did you know this?
1
Not at all
2
3
4
5
Perfectly
20
Q

Contain an element with more than one oxidation state

A

multivalent compounds

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
21
Q

Low oxidation state:
* affix –ous

High oxidation state:
* affix –ic

A

Old Method

22
Q
  • Low OS – indicate using roman numerals
  • High OS – enclosed in parenthesis
A

New Method

23
Q

Old Method and New Method

  • FeCl2
  • FeCl3
  • PbO
  • PbO2
A

Old Method
- Ferrous Chloride
- Ferric Chloride
- Plumbous Oxide
- Plumbic Oxide

New Method
- Iron (II) Chloride
- Iron (III) Chloride
- Lead (II) Oxide
- Lead (III) Oxide

24
Q

Hydrogen + Non metal

A

hydroacids

25
Q

HYDROACIDS

Give the name of the compound and name of the acid

  1. HCl
  2. HF
  3. HBr
A

Name of the Compound
hydrogen + nonmetal + ide

  1. Hydrogen Chloride
  2. Hydrogen Fluoride
  3. Hydrogen Bromide

Name of the Acid
1. Hydrochloric Acid
2. Hydrofluoric Acid
3. Hydrobromic Acid

26
Q

___________: Compounds with 3 different elements

_______: Hydrogen + Nonmetal + Oxygen (nonmetal)

A

ternary compounds

oxyacids

27
Q

OS of Middle Elements

+7
+6; +5
+4; +3
+1

  1. HClO4
  2. HClO3
  3. HClO2
  4. HClO
A

Per + root + ic + acid
root + ic + acid
root + ous + acid
hypo + root + ous + acid

  1. Perchloric acid
  2. Chloric acid
  3. Chlorous acid
  4. hypochlorous acid
28
Q
  • named by using prefixes to indicate the no. of oxygen atoms in the compound
  1. CO
  2. CO2
  3. SO3
  4. P2O5
A

OXYGEN CONTAINING COMPOUNDS

  1. Carbon Monoxide
  2. Carbon Dioxide
  3. Sulfur Trioxide
  4. Phosphorous Pentaoxide
29
Q
  • A combination of symbols of elements constituting a compound
  • Represents the number of atoms present in the molecule of a compound
A

Formula

30
Q
  • Combining the capacity of an element
  • No. of e- (electrons) lost/gained/shared by an atom
  • Shown only when atoms are combined
A

Valence/Oxidation No. or State

31
Q

Charged particles
* Positive ion (Cation)
* Na+, Ca++, Al+3
* Negative ion (Anion)
* Cl-, S-

A

Ions

32
Q
  • Contain more than 1 element either positive (+) charged or negatively (-) charged
A

Polyatomic Ions/ Radical

33
Q

Rules in Formula Writing

A
  1. Write the symbols side by side
  2. Above each symbol, write the valence
  3. Criss cross the valences
  4. Omit subscript whenever it equals to one
  5. When the radical needs a subscript enclose it with a parenthesis nos.
  6. Reduce subscripts to small whole
  7. When a radical already contains a parenthesis, enclose it with a bracket
34
Q

Rules in assigning Oxidation State

A
  1. The oxidation state of an uncombined item/gas is equal to zero
  2. The algebraic sum of the positive (+) and negative (-) oxidation states in the formula of a compound is equal to zero.
  3. The algebraic sum of the + and - oxidation states in the formula of a polyatomic ion is equal to the charge of the ion
35
Q
  • State in which the rate of the forward chemical reaction equals the rate of the reverse reaction
  • At equilibrium, the concentrations of the reactants and products remain constant over time, though the reactions themselves continue to occur.
A

chemical reaction

36
Q
  • Substance that undergoes change during a chemical reaction
  • interact with each other to form products
A

REACTANT

37
Q

A substance that is formed as
a result of a chemical reaction

A

PRODUCT

38
Q
  • Refers to the state in which the rate of forward chemical reaction equals the rate of the reverse reaction
  • At _________, the concentrations of the reactants and products remain constant over time, though the reactions themselves continue to occur
A

chemical equilibrium

39
Q
  • A numerical value that expresses the ratio of the concentrations of products to reactants at equilibrium.
  • This value is constant for a given reaction at a specific temperature.
A

equilibrium constant

40
Q
  • A rule that states that if a dynamic equilibrium is disturbed by changing the conditions (like pressure, temperature, or concentration), the system will adjust to counteract the disturbance and restore equilibrium.
A

Le Chatelier’s Principle

41
Q

types of chemical reactions

A
  • synthesis reaction
  • decomposition reaction
  • single replacement reaction
  • double replacement reaction
42
Q
  • TWO reactants combine to give ONE product
  • Union or combination of simple substances to form complex substances (compounds)
  • Metal + Oxygen —> Metal Oxide
    Mg (s) + O2 —> MgO (s)
  • Metal + Nonmetal —> Salt
    Na (s) + Cl2(g) —> NaCl (s)
A

synthesis reaction

A + B —> AB

MgO
NaCl

43
Q
  • Breakdown of a more complex substance/compound into its simpler form
  • A single substance is broken to give TWO or MORE different substances
  • Metal Oxide
    HgO (s) —> Hg + O2
  • Carbonates and Bicarbonates decompose to yield CO2 when heated
    NaHCO3 —> Na2CO3(s) + H2O + CO2
A

decomposition reaction

AB —> A + B

Hg + O2

44
Q
  • An element replaces another in a compound
  • One element reacts with a compound to take the place of the element of that compound

NaOH + HCl —> NaCl + H2O

A

single replacement reaction

AB + CD —> AD + CB

45
Q
  • TWO compounds exchange partners with each other to produce TWO different compounds (2 or more)
  • Combination of 2 or more compounds forming 2 or more different compounds
  • Metal: A + BC —> AC + B
    Zn + H2SO4 —> ZnSO4 + H2
  • Non-metal: A + BC —> BA + C
    F2 + HI —> HF + I2
A

Double replacement reaction

46
Q

Writing a Chemical Equation

A
  1. Identify the reactants and products
  2. Write the chemical formulas
  3. Check for state symbols if necessary (e.g. s, l, g, aq)
  4. Balance the equation
47
Q

——->
<—–>

arrow up
arrow down

triangle
+

A
  • yields, produces (points to products)
  • reversible reactions
  • gas evolved (written after the substance)
  • solid ppt formed (written after the substance)
  • heat
  • plus/added to (placed between substances)
48
Q

_________: contains same no. of each kind of atom on each side of the equation.

It obeys the Law of Conservation of Mass.

Thus, the mass of reactants = mass of products or mass before reaction = mass after reaction

A

balanced equations

49
Q

type of chemical reaction that involves the transfer of electrons between two substances

GEROA
LEORA

A

REDOX REACTIONS

50
Q
  • substance loses electrons
  • increasing oxidation state of the substance
A

OXIDATION

51
Q
  • substance gains electrons
  • decreasing oxidation state of the substance
A

REDUCTION

(SLU) PHARMA 113: Chem Lec (13 decks)

Brainscape helps you reach your goals faster, through stronger study habits.
© 2024 Bold Learning Solutions. Terms and Conditions