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Chemistry XI > 1 Basic Concepts of Chemistry > Flashcards

1 Basic Concepts of Chemistry Flashcards

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1
Q

Chemistry was mainly developed in the form of _______________.

A

Alchemy and Iatrochemistry

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2
Q

In ancient India, chemistry was called ___________.

A

In ancient India, chemistry was called Rasayan Shastra or Rasvidya. It included metallurgy, medicine, manufacture of cosmetics, glass, dyes, etc

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3
Q

Who was the first Indian to formula the atomic theory?

A

Acharya Kanada was the first proponent of the ‘Atomic Theory’. He formulated that all substances are aggregated form of smaller units called atoms, which are spherical and indestructible in the original state

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4
Q

Which two drugs are effective in cancer therapy?

A

CISPLATIN and TAXOL

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5
Q

Which drug is used for treating AIDS patients?

A

AZT (Azidothymidine)

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6
Q

What is matter?

A

Anything which has mass and occupies space is called matter. Everything around us is composed of matter. Matter can exist in three states – solids, liquids and gases

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7
Q

Solids have ______ shape and volume.

A

• Solids have definite shape and volume. Particles are held very close to each other and there is not much freedom of movement

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8
Q

Liquids have _______ volume but _____ shape.

A

• Liquids have definite volume but do not have definite shape. They take up the shape of container. Particles are close to each other but they can move around

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9
Q

Gases have _____ shape and _______ volume.

A

• Gases have neither definite volume nor definite shape. They completely occupy the space in the container in which they are placed

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10
Q

What is a mixture?

A

A mixture contains many particles of two or more pure substances which may be present in any ratio. Their composition is variable. A mixture may be homogeneous or heterogeneous

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11
Q

What is a homogeneous mixture?

A

• In a homogeneous mixture, the particles of components are uniformly distributed throughout the bulk of the mixture. Eg – Sugar solution, air

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12
Q

What is a heterogeneous mixture?

A

• In a heterogeneous mixture, the composition is not uniform and sometimes different components are visible. Eg – Mixture of Salt and Sugar

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13
Q

What is a pure substance?

A

• When all constituent particles of a substance are same in chemical nature, it is said to be a pure substance. The constituent particles of pure substances have fixed composition. Eg – Glucose, Copper, Silver. Pure substances can be further divided into elements and compounds

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14
Q

What is a compound?

A

When two or more atoms of different elements combine together in a definite ratio, a compound is obtained. Eg – Water, Ammonia, CO2, etc

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15
Q

The Metric System originated in ______.

A

France

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16
Q

The International System of units was established by ______________

A

• The International System of Units was established by the 11th General Conference on Weights and Measurements. (Metre Convention Treaty – Paris)

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17
Q

What is the difference between mass and weight?

A

Mass of a substance is the amount of matter present in it while weight is the force exerted by gravity on an object

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18
Q

The mass of a substance can be determined accurately in the laboratory by using a ____________.

A

ANALYTICAL BALANCE

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19
Q

__________ is the amount of space occupied by a substance.

A

Volume

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20
Q

Temperature below 0 degree Celsius is possible in _________ scale but not in _________ scale.

A

Temperature below 0 degree Celsius is possible in Celsius scale but not in Kelvin scale

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21
Q

What is the formula for conversion Fahrenheit to Celsius?

A

F = 9/5 (C) + 32

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22
Q

The Fahrenheit scale is represented between _____ degree and ______ degree.

A

The Fahrenheit scale is represented between 32 and 212.

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23
Q

How to convert Celsius to Kelvin?

A

K = C + 273.15

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24
Q

What are significant figures?

A

• Significant figures are meaningful digits which are known with certainty plus one which is uncertain. The uncertainty is indicated by writing the certain digits and the last uncertain digit

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25
Q

What is the difference between precision and accuracy?

A

Precision – Closeness of various measurements for the same quantity

Accuracy – Agreement of a particular value to the true value of the result

26
Q

What are the rules for the following operations of figures?

a) Addition/Subtraction
b) Multiplication/Division

A

Addition/Subtraction of SF = Minimum number of digits after Decimal Point

Multiplication/Division of SF = Minimum number of significant digits after Decimal

27
Q

What are the other names for Dimensional Analysis?

A

FACTOR LABEL METHOD

UNIT FACTOR METHOD

DIMENSIONAL ANALYSIS

28
Q

What is the Law of Conservation of Mass?

A

Law Of Conservation Of Mass - It says that matter can neither be created nor destroyed.

29
Q

Who put forward the Law of Conservation of Mass?

A

This law was put forth by Antoine Lavoisier in 1789.

30
Q

What is the Law of Definite Proportions?

A

• Law Of Definite Proportions – Proust worked with two samples of cupric carbonate and concluded that a given compound always contains same elements combined together in the same proportion by mass.

31
Q

Who put forward the Law of Definite Proportions?

A

This law was given by French chemist Joseph Proust.

32
Q

What is the Law of Multiple Proportions?

A

Law Of Multiple Proportions – According to this law, if two elements can combine to form more than one compound, the masses of one element that combine with a fixed mass of the other element, are in the ratio of small whole numbers

33
Q

Who put forward the Law of Multiple Proportions?

A

This law was proposed by John Dalton in 1803.

34
Q

What is the Law of Gaseous Volumes?

A

• Law of Gaseous Volumes – It states that when gases combine in a reaction, they do so in a simple ratio by volume, provided all gases are at same temperature and pressure

35
Q

Who put forward the Law of Gaseous Volumes?

A

This law was given by Gay Lussac in 1808.

36
Q

What is the Avogadro’s Law?

A

In 1811, Avogadro proposed that equal volumes of all gases at the same temperature and pressure should contain equal number of molecules

37
Q

Avogadro’s proposal was published in the __________________.

A

French Journal de Physique

38
Q

What is the Dalton’s Atomic Theory?

A

1) Matter consists of indivisible atoms.
2) All atoms of a given element have identical properties, including identical mass. Atoms of different elements differ in mass.
3) Compounds are formed when atoms of different elements combine in a fixed ratio.
4) Chemical reactions involve reorganisation of atoms. These are neither created nor destroyed in a chemical reaction.

39
Q

Dalton published his publication ____________________.

A

‘A New System of Chemical Philosophy’

40
Q

What are the limitations of the Dalton’s Atomic Theory?

A

It could not explain the laws of gaseous volumes.

It could not provide the reason for combining of atoms.

41
Q

What is one atomic mass unit?

A

One atomic mass unit (amu) is defined as a mass exactly equal to one-twelfth the mass of one 12C atom.

42
Q

1 amu = ___________ g

A

1 amu = 1.66 x 10^-24 g

43
Q

What is the value of the Avogadro’s constant?

A

• The mole, symbol ‘mol’, is the SI unit of amount of substance. One mole contains exactly 6.022 x 1023 elementary entities. This number is called the ‘Avogadro Constant’ or the ‘Avogadro Number’

44
Q

What is used to determine the mass of an atom?

A

Mass Spectrometer

45
Q

What is molar mass?

A

• The mass of one mole of a substance in grams is called its molar mass (Molar Mass = Molecular Mass). The molar mass in grams is numerically equal to atomic/molecular/formula mass in ‘u

46
Q

An empirical formula represents the ____________ ratio of various atoms present in a compound, whereas, the molecular formula shows the ____________ of different types of atoms present in a molecule of a compound

A

Empirical Formula - Simplest Whole Number Ratio

Molecular Formula - Exact Number

47
Q

_____________ deals with the calculation of the reactants and products involved in a chemical reaction.

A

Stoichiometry deals with the calculation of masses of the reactants and products involved in a chemical reaction

48
Q

What is a limiting reagent?

A

The reactant which gets consumed first, limits the amount of product formed and is, therefore, called the limiting reagent

49
Q

What is the formula of mole fraction?

A

Mole Fraction = No. of Moles of A/Total No. of Moles

50
Q

What is molarity?

A

Molarity is the most widely used unit and is denoted by ‘M’. It is defined as the number of moles of solute in 1 litre of solution

Molarity (M) = No. of Moles of Solute/Volume of Solution in Litres

51
Q

The molarity of a solution __________ upon temperature because volume of a solution is dependent on temperature

A

The molarity of a solution depends upon temperature because volume of a solution is dependent on temperature

52
Q

What is molality?

A

Molality is denoted by ‘m’ and is defined as the number of moles of solute present in 1 kg of solvent

53
Q

The molality of a solution _________ change with temperature since mass remains unaffected with temperature

A

The molality of a solution does not change with temperature since mass remains unaffected with temperature

54
Q

What is a stock solution?

A

• Often in labs, a solution of desired concentration is prepared by diluting a solution of known higher concentration. The solution of higher concentration is known as stock solution

55
Q

What is 1 angstorm?

A

1 angstrom = 10^-10m = 10^-1 nm = 10^2 pm

56
Q

What is the Law of Reciprocal Proportions?

A

The law of reciprocal proportions was proposed by Jeremias Ritcher in 1792.

It states that, “If two different elements combine separately with the same weight of a third element, the ratio of the masses in which they do so are either the same or a simple multiple of the mass ratio in which they combine.”

57
Q

What are the formulae for calculating number of moles?

A

N = Given Mass/Atomic Mass

N = Given number of entities/6.022 * 10^23

N = Given Volume/22.4 L

58
Q

What is 1 gram atom?

A

1 gram atom = 6.022 * 10^23 atoms

1 gram molecule = 6.022 * 10^23 molecules

59
Q

What is the formula for calculating ‘n’ (Molecular and Empirical Mass)?

A

n = Molecular Mass/Empirical Formula Mass

60
Q

What is the difference between molarity and molality?

A

Molarity is the most widely used unit and is denoted by ‘M’. It is defined as the number of moles of solute in 1 litre of solution.

Molality is denoted by ‘m’ and is defined as the number of moles of solute present in 1 kg of solvent.

Chemistry XI (2 decks)

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