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A++ SPM Chemistry Definitions > Chemistrizz Terms > Flashcards

Chemistrizz Terms Flashcards

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1
Q

What is Matter?

A

Something that has mass and occupies space

Matter is the substance of which physical objects are made.

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2
Q

What is Proton Number?

A

Number of protons in the nucleus of an atom

The proton number defines the identity of an element.

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3
Q

What is Nucleon Number?

A

Total number of protons and neutrons in the nucleus of an atom

The nucleon number reflects the atomic mass of an element.

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4
Q

What are Isotopes?

A

Atoms of the same element with the same number of protons but different number of neutrons

Isotopes have similar chemical properties but different physical properties.

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5
Q

What is Natural Abundance?

A

Percentage of isotopes present in a natural sample of an element

Natural abundance affects the relative atomic mass of an element.

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6
Q

What is Relative Atomic Mass?

A

Average mass of an atom of the element compared to 1/12 of the mass of one carbon-12 atom

This is a dimensionless quantity.

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7
Q

What is Relative Molecular Mass?

A

Average mass of the molecule compared to 1/12 of the mass of one carbon-12 atom

It is calculated by summing the relative atomic masses of the constituent atoms.

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8
Q

What is Relative Formula Mass?

A

Average mass of the ionic compound compared to 1/12 of the mass of one carbon-12 atom

This term is often used for ionic compounds.

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9
Q

What is the Avogadro Constant?

A

Number of particles contained in one mole of substance that is 6.02 x 10^23 mol^-1

This constant is crucial for converting between moles and number of particles.

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10
Q

What is Molar Mass?

A

Mass of one mol of a substance

Molar mass is expressed in grams per mole (g/mol).

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11
Q

What is Molar Volume?

A

Volume occupied by 1 mole of a gas

At standard temperature and pressure, this is approximately 22.4 liters.

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12
Q

What is a Chemical Formula?

A

Representation of a chemical substance using alphabets to represent the atoms and subscript numbers to show the number of each type of atoms

It conveys the composition of a compound.

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13
Q

What is an Empirical Formula?

A

Chemical formula that shows the simplest whole number ratio of the number of atoms of each element in a compound

Example: The empirical formula for glucose (C6H12O6) is CH2O.

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14
Q

What is a Molecular Formula?

A

Chemical formula that shows the actual number of atoms of each element found in a molecule of a compound

It provides more specific information than the empirical formula.

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15
Q

What is the Modern Periodic Table of Elements?

A

A form of systems classification of elements in ascending order of proton numbers from left to right and from top to bottom

This arrangement reflects the periodic law.

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16
Q

What are Groups in the Periodic Table?

A

Vertical columns in the Periodic Table of Elements

Elements in the same group often exhibit similar chemical properties.

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17
Q

What are Periods in the Periodic Table?

A

Horizontal rows in the Periodic Table of Elements

Each period corresponds to the principal energy level of the electrons.

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18
Q

What are Hydrogen Bonds?

A

Attractive forces between a hydrogen atom bonded with an atom of high electronegativity and another electronegative atom

Commonly found in water and biological molecules.

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19
Q

What is a Dative bond?

A

A type of covalent bond where the electron pair that is shared comes from one atom only

Also known as a coordinate bond.

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20
Q

What are Acids?

A

Chemical substances that ionize in water to produce hydrogen ions

Acids can vary in strength and concentration.

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21
Q

What is Basicity?

A

Number of hydrogen ions that can be produced by an acid molecule that ionizes in water

This indicates the strength of the acid.

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22
Q

What is an Alkali?

A

Substance that reacts with acids to produce salt and water only

Alkalis are usually soluble bases.

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23
Q

What is pH?

A

Logarithmic measure of the concentration of hydrogen ions in an aqueous solution

pH values range from 0 to 14, with lower values indicating higher acidity.

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24
Q

What is a Strong Acid?

A

An acid that ionizes completely in water to produce a high concentration of hydrogen ions

Examples include hydrochloric acid and sulfuric acid.

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25
What is a Weak Acid?
An acid that ionizes partially in water to produce a low concentration of hydrogen ions ## Footnote Examples include acetic acid and citric acid.
26
What is a Strong Alkali?
An alkali that ionizes completely in water to produce a high concentration of hydroxide ions ## Footnote Examples include sodium hydroxide and potassium hydroxide.
27
What is a Weak Alkali?
An alkali that ionizes partially in water to produce a low concentration of hydroxide ions ## Footnote Examples include ammonia.
28
What is Concentration?
A measurement that shows the quantity of solute dissolved in a unit volume of solution ## Footnote Concentration can be expressed in various units, including molarity.
29
What is Concentration in g dm^-3?
Mass of solute found in 1 dm³ solution ## Footnote This unit is commonly used in chemistry to express concentration.
30
What is the Heat of Displacement?
Heat change when one mole of s is displaced from its salt solution by a more electropositive metal. ## Footnote This process involves the exchange of ions in a solution.
31
What is the Heat of Neutralisation?
Heat change when one mole of water is formed from the reaction between an acid and an alkali. ## Footnote This reaction typically involves the formation of water and a salt.
32
What is the Heat of Combustion?
Heat released when one mole of a substance is completely burnt in excess oxygen. ## Footnote This measurement is important for understanding the energy content of fuels.
33
What is a Fuel?
Substances that burn in the air to produce heat energy. ## Footnote Fuels can be solids, liquids, or gases.
34
What is the Fuel Value of a Fuel?
Amount of heat energy released when one gram of fuel is completely burnt in excess oxygen. ## Footnote This value helps determine the efficiency of different fuels.
35
Define Polymer.
Long chain molecule that is made from a combination of many repeating basic units. ## Footnote Polymers can be natural or synthetic.
36
What is a Monomer?
Basic unit of a polymer. ## Footnote Monomers link together to form polymers through chemical reactions.
37
What are Natural Polymers?
Polymers that are naturally available and can be obtained from our surroundings. ## Footnote Examples include cellulose, proteins, and natural rubber.
38
What are Synthetic Polymers?
Polymers that are man-made through chemical reactions in laboratories or factories. ## Footnote Examples include nylon, polyester, and polystyrene.
39
What are Thermoplastic Polymers?
Polymers that can be repeatedly remoulded upon heating and can be recycled. ## Footnote Common examples include polyethylene and polyvinyl chloride (PVC).
40
What are Thermosetting Polymers?
Polymers that cannot be remoulded after heating. ## Footnote These polymers are typically used in applications requiring durability.
41
What are Elastomer Polymers?
Polymers that can be stretched and can return to their original shape when released. ## Footnote They are commonly used in rubber products.
42
What is Vulcanisation?
Process of producing rubber that is more elastic and with better quality through the production of cross-links between polymer chains. ## Footnote This process enhances the strength and elasticity of rubber.
43
Define Synthetic Rubber.
Synthetic polymer that is elastic in nature or elastomer polymer. ## Footnote Common types include styrene-butadiene rubber (SBR) and neoprene.
44
What are Oils and Fats?
Esters produced through the reaction between fatty acids and glycerol (propan-1,2,3-triol). ## Footnote These compounds are used in cooking and food preservation.
45
What are Soaps?
Sodium or potassium fatty acid salts. ## Footnote Soaps are used as cleaning agents due to their ability to emulsify oils.
46
What are Detergents?
Sodium salts of sulphonic acids. ## Footnote Detergents are synthetic cleaning agents that work in hard water.
47
What are Food Additives?
Natural or synthetic ingredients added to food to prevent damage or to improve the appearance, taste, or texture. ## Footnote Examples include preservatives, colorants, and flavor enhancers.
48
What are Medicines?
Chemical used to help with the treatment or prevention of diseases. ## Footnote Medicines can be prescription or over-the-counter.
49
What are Cosmetics?
Materials or products that are used externally to cleanse, protect, or enhance one's appearances. ## Footnote This category includes skincare, makeup, and haircare products.
50
What is Nanoscience?
Study on processing of substances of nanoscale that are between 1 nanometer to 100 nanometers. ## Footnote This field explores properties and applications of materials at the nanoscale.
51
What is Nanotechnology?
Development of substances or gadgets using the properties of nanoparticles. ## Footnote Applications include medicine, electronics, and materials science.
52
What is Green Technology?
Technology or application developed to minimize the negative effects of harmful human activities. ## Footnote This includes renewable energy sources and sustainable practices.
53
What is Wastewater?
Liquid waste that consists of human waste, food waste, oil, and chemicals. ## Footnote Treatment is necessary to prevent environmental contamination.
54
What is Effluent?
Waste in the liquid form discharged into the drainage system or water source. ## Footnote Effluent must be treated to meet environmental regulations.
55
What is a redox reaction?
Chemical reaction where oxidation and reduction occur simultaneously.
56
Define electropositivity.
Tendency of atoms to release electrons to form cations.
57
What is the electrochemical series?
Series of metal arrangements according to the standard electrode potential in the order of most negative to most positive.
58
What does electrode potential refer to?
Potential difference produced when an equilibrium is established between metal M and the aqueous solution containing metal M+ ions in a half-cell.
59
Describe a simple chemical cell.
Two different metal plates are dipped into an electrolyte and connected with connecting wires.
60
What are electrolytes?
Substances that can conduct electricity in either the molten state or aqueous solution and undergo chemical changes.
61
What are non-electrolytes?
Substances that cannot conduct electricity in all states.
62
Define conductor in the context of electricity.
Substances that conduct electricity in solid or molten state, but do not undergo chemical changes.
63
What is electrolysis?
Process whereby compounds in the molten state, or an aqueous solution decompose into their constituent elements by passing electricity through them.
64
What is corrosion of metal?
Redox reaction where the metal is oxidized spontaneously when the metal atoms release electrons to form metal ions.
65
What are carbon compounds?
Compounds that contain carbon as their constituent element.
66
Define organic compound.
Compounds originating from living things that contain the carbon element bonded covalently with other elements such as hydrogen, nitrogen, sulfur, and phosphorus.
67
What are inorganic compounds?
Compounds originating from non-living materials such as oxides of carbon, carbonate compounds, and cyanide compounds.
68
Fill in the blank: Organic compounds containing only hydrogen and carbon are called _______.
Hydrocarbon
69
What are non-hydrocarbons?
Organic compounds containing carbon and hydrogen and other elements, such as oxygen, nitrogen, phosphorus or halogens.
70
Define saturated hydrocarbon.
Hydrocarbons containing only single bonds between carbon atoms.
71
What is an unsaturated hydrocarbon?
Hydrocarbons containing at least one double bond or triple bond between carbon atoms.
72
What is cracking in chemistry?
Process of breaking long chain hydrocarbons into smaller hydrocarbons.
73
What is a molecular formula?
Chemical formula that shows the type and actual number of atoms of each element in a molecule.
74
Define structural formula.
Chemical formula that shows the type of bond and how the atoms in a molecule are bonded to each other.
75
What is structural isomerism?
Phenomenon where a compound has the same molecular formula but with two or more different structural formulas.
76
Fill in the blank: Molecules that have the same molecular formula but different structural formula are called _______.
Isomers
77
What is chain isomerism?
Isomers that have different arrangements of carbon chains; either straight chain or branched chain.
78
Define position isomerism.
Isomers that have different positions of functional groups on the same carbon chain.
79
What is an exothermic reaction?
Chemical reactions that release heat to surrounding.
80
True or False: An endothermic reaction absorbs heat from the surroundings.
True
81
What is the heat of reaction?
Heat change of one mole of reactant that reacts or one mole of product that is formed.
82
What is the heat of precipitation?
Heat change when one mole of precipitate is formed from their ions in an aqueous solution.
83
What is the definition of "Concentration in mol dm³"?
Number of moles of solute found in 1 dm³ solution.
84
What is a "Standard Solution"?
A solution with a known concentration
85
What happens during "Neutralization"?
A: A reaction between an acid and an alkali to produce salt and water only.
86
What is "Titration"?
A: A qualitative analysis method to determine the volume of acid needed to completely neutralize a given volume of alkali and vice versa.
87
What is the "End Point" in titration?
A: The point in titration at which the acid-base indicator changes color.
88
Q: What is a "Salt"?
A: An ionic compound formed when the hydrogen ion from the acid is replaced with the metal ion or the ammonium ion.
89
Q: What are "Soluble Salts"?
A: Salts that dissolve in water at room temperature.
90
Q: What are "Insoluble Salts"?
A: Salts that do not dissolve in water at room temperature.
91
Q: What is "Qualitative Analysis"?
A: A technique used to identify the cation and anion present in a salt by analyzing its physical and chemical properties.
92
Q: What is the "Rate of Reaction"?
A: Changes in quantity of the reactant per unit time or changes in quantity of product per unit time.
93
Q: What is the "Average Rate of Reaction"?
A: The average value for the rate of reaction that occurs in a particular time interval.
94
Q: What is the "Instantaneous Rate of Reaction"?
A: The rate of reaction at a particular point of time.
95
Q: What is an "Alloy"?
A: A mixture of two or more elements where the main element is a metal.
96
Q: What is a "Ceramic"?
A: A solid made up of inorganic and non-metallic substances.
97
0: What are "Composite Materials"?
A: Materials made from combining two or more non-homogeneous substances, consisting of a matrix substance and a strengthening substance.
98
0: What are "Composite Materials"?
A: Materials made from combining two or more non-homogeneous substances, consisting of a matrix substance and a strengthening substance.

A++ SPM Chemistry Definitions (1 decks)

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