Alfred Ajibola
- 09th November, 2020 @ 12:38 PM
Topics in Chemistry
Gas laws in chemistry Charles's law explained Calculation questions on Charles's law Examples of Charles's law in real life Boyle's law explained Calculation questions on Boyle's law Examples of Boyle's law in real life Summary on the kinetic molecular theory of gases Postulates of kinetic theory of gases Avogadro's number explained with worked examples Mole and Avogadro's Number explained Le Chatelier's Principle: Changes in concentration and pressure in dynamic equilibrium Chemical Equilibrium: Dynamic Equilibrium in Chemistry Static and Dynamic Equilibrium explained with their differences Chemistry Scheme of Work, SS1, First Term Chemistry Scheme of Work, SS1, Second Term Chemistry Scheme of Work, SS1, Third Term Compounds in Chemistry: Characteristics of Compounds Types of Mixture: Homogenous and Heterogeneous Mixtures What are mixtures? Characteristics of mixturesAcademic Questions in Chemistry
_____ electron(s) is a term that describes the number of electron(s) in the outermost shell of an atom.
A. Outer
B. Excess
C. Valence
D. Positive
E. Negative
F. Last
_____ is the negative electrode in electrolysis.
A. Anode
B. Anion
C. Cathode
D. Cation
E. Ion
F. Electrolyte
The above diagram shows the _____ type of bond.
A. Covalent
B. Polar covalent
C. Coordinate covalent
D. Metallic
E. Van dear walls
F. Ionic
Metals are referred to as _____ in their impure state.
A. Diluted
B. Consecrated
C. Coloured
D. Ores
E. Stained
F. Strained
Metals generally have the quality to shine, glow, sparkle, glitter, reflect light and be polished. This characteristic of metals is termed _____.
A. State
B. Ductility
C. Luster
D. Malleability
E. Hardness
F. Inflorescence
The _____ spectrometry experiment conducted on isotopic elements gave a confirmation for the existence of isotopes.
A. Mole
B. Volume
C. Weight
D. Number of moles
E. Mass
F. Amount of substance
John Dalton's first atomic theory was modified based on a discovery made by _____.
A. Sir Isaac Newton
B. Albert Einstein
C. Avogadro
D. Rutherford
E. Boyle and Charles
F. Gay Lussac
Which of the following isn't an element of the periodic table.
A. J
B. Y
C. W
D. B
E. U
F. K
In chemistry, chemical equilibrium is also referred to as dynamic equilibrium. Recall that the word 'equilibrium' in English refers to a state of balance or stability. However, dynamic equilibrium in chemistry focuses on the stability of reaction rate between reactants and products in a chemical reaction.
You can read on the differences between static and dynamic equilibrium here.
Chemical or dynamic equilibrium will only occur in a reversible reaction which is always denoted by the forward and backward arrow signs (⇌). An instance is shown in the formation of ammonia (NH3) via the Haber process.
N2(g) + 3H2(g) ⇌ 2NH3(g)
Reversible reaction is a type of reaction whereby the reaction can proceed in both directions (forward and backward direction).
You can read on periodic table and classification of elements here.
Dynamic equilibrium is said to be reached in chemical reaction when the rate of forward reaction equals that of the backward reaction and as such, the concentration of the reactants and products remain constant with time even though the movement of substances still occurs between both (reactants and products); while the system shows no further change in properties.
The image below shows the processes that results into dynamic equilibrium:
You can read on chemical properties of matter explained with examples here.
Dynamic equilibrium does not commence at the beginning of a reaction. The forward reaction must first proceed. This implies that the reactants collide or react in order to form the products. After some time, the backward reaction also proceeds as the products begin to react, forming back the reactants. This forward and backward reaction continues differentially until the both reactions proceed at the same rate. At this point, dynamic equilibrium is said to be reached.
You can read on elements and their characteristics here.
A reversible reaction must occur in a closed system for dynamic equilibrium to be attained. This ensures that neither the reactants nor products are lost during the chemical reaction. As an instance, iodine is a substance that sublimes; that is, it changes directly from solid to a gaseous state when heated.
When iodine is heated in an open container, it sublimes into gaseous iodine which escapes into the atmosphere; and there will be no way for the backward reaction to proceed.
I2(s) -> I2(g)
You can read on the states of matter and characteristics of solids here.
However, if the heated container was sealed (in a closed system), the iodine crystals sublime into a purple iodine vapour, and both the crystals and vapour remains inside the container until a chemical equilibrium is reached.
I2(s)⇌I2(g)
Please read on sublimation and other separation techniques here.
It is noteworthy to state that the concentrations of both the reactants and products must remain constant and not necessarily the same when dynamic equilibrium is reached in a system.
Also, it is important to state that factors such as a change in concentration, pressure or temperature will affect or alter the dynamic equilibrium in a system. This was explained by a French chemist named Henry Louis Le Chatelier. It was his principle - 'Le Chatelier’s Principle', also known as the 'Equilibrium Law' that explains the aformentioned changes, predicting their effects on a system in dynamic or chemical equilibrium.
Please read more on Le Chatelier’s principles and the factors that affects dynamic equilibrium here.
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Amazing facts in Chemistry
Plastic and Glass can decompose, but not in our lifetimes. It takes an average time of 450 years for plastics to decompose. As for the decomposition of glasses, it takes about 4,000 years
The only letters that failed to appear on the periodic table are letters:
Gold and copper are the only two non-silvery colored metals.
Copper is the only metal that is naturally antibacterial. For this reason, some children utilize 'copper water bottles' in schools
Water freezes faster when it’s warm than when it’s cold
Most element in their pure state exists physically in different forms. For instance, pure carbon can exist as both diamond and graphite. This phenomenon is called allotropy
If you pour a handful of salt into a full glass of water, the water level will go down rather than overflowing the glass.
Similarly, if you mix half liter of water and half litre of alcohol, the total volume of the liquid will be les than one litre
NOTABLE POINTS IN Chemistry
The periodic table, also called periodic table of elements or Mendeleev's table, is a table that shows an organized arrangement of the 118 chemical elements according to their atomic number.
Out of the 118 elements; elements 1 - 94 are present in nature while elements 95 - 118 are synthesized artificially.
The manner at which elements are arranged on this table reveals some similarities in their electronic configurations and chemical properties.
A compound composed of iron (Fe) and oxygen (O) was analyzed and found to contain 69.94% iron and 30.06% oxygen. Find the empirical formula of the compound. (Molar mass of Fe=55.85, O=16)
Step 1: Identify the given parameter from the question.
Fe = 69.94%, O = 30.06%.
Empirical formula = Fe?O?
Step 2: Convert the percentages to gram. (just attribute grams to the %).
Step 3: To get the mole ratio of each element, convert the gram to moles using the formula (mole = mass/molarmass). Please merorize this formula because we always work with moles in emperical formula.
Mole of Fe: 69.94/55.85 = 1.252mol
Mole of O: 30.06/16 = 1.879mol
Step 4: Divide both sides by the smallest mole ratio.
Iron has the smallest mole ratio in our case, therefore: 1.252/1.252 = 1, 1.879/1.252 = 1.5
We now have the formula = Fe1O1.5
Step 5: Multiply each of the moles by the smallest whole number that will convert each into a whole number. (In our case, the number '2' is the smallest whole number that will make '1.5' and '1' whole numbers when multiplied by it.
For iron (Fe), we will have 1 x 2 = 2
For oxygen (O), we will have 1.5 x 2 = 3
Step 6: Write the empirical formula.
The empirical formula= Fe2O3
Iron(III)tetraoxosulphate(VI)
In chemistry, hydrocarbons can be classified as either aliphatic or aromatic. Recently, both classifications of hydrocarbon were based on their structure rather than their origin.
Aliphatic hydrocarbons are put into three main groups according to the types of bonds they possess. These are:
Alkanes
Alkenes
Alkynes
They are shown in the image below:
It's important to note the followings:
Alkanes have single bonds (only) in their structures.
Alkenes always have a carbon-carbon double bond present in their structure.
Alkynes always have a carbon-carbon triple bond present in their structure.
Aromatic hydrocarbons are classified into:
Organic chemistry is the study of carbon and it's compounds.
Carbon is the focus of organic chemistry because it has a wide chemical diversity in the sense that it can combine with other carbon atoms to form a long chain of carbon molecule. This ability and process whereby carbon can form a long chain of itself is called catenation.
A major challenge encountered when calculating molecular mass is that it becomes difficult or impossible to calculate especially when the relative molecular mass of large molecules, polymers and macromolecules are involved.
Examples of large molecules (with indefinite molecular masses) include carbohydrates, cellulose and complex sugars.
The large molecules (above) have no specific chemical formula throughout their volume.
Understand that Relative Molecular Mass prove to be useful only when we calculate substances with small and definite molecular sizes. This was proven through the modifications of Dalton's atomic theory.
Please read on Dalton's atomic theory and its modifications here.
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