GRADE 7 TH : ELEMENTS, COMPOUNDS &...
Transcript of GRADE 7 TH : ELEMENTS, COMPOUNDS &...
GRADE 7 TH : ELEMENTS, COMPOUNDS & MIXTURES
Atoms:
• Everything in this world is made of billions of atoms.
• The smallest atom known as hydrogen.
• Each atom is represented as a sphere having a diameter of 7 X 10-8 mm.
• Different elements have different diameter and different masses.
• Chemists use shorthand symbols to label the elements and their atoms.
• The symbols consists of 1, 2 or 3 letters.
• For example 1. C - Carbon 2. Cl – Chlorine
• Some symbols seems to have no relations with the name of the element. For
example: 1. Na – Sodium 2. Pb - Lead
• These symbols come from their Latin names.
Atomicity: the number of atoms present in the molecule of an element. For example, each molecule of oxygen (O2) is composed of two oxygen atoms. So atomicity of oxygen is 2.
Molecules:
• The atoms of same elements join together to form a molecule.
• The small group of atoms are called molecules.
• For example: when the atoms of elements hydrogen, oxygen, nitrogen, fluorine,
chlorine, bromine and iodine are each joined in pairs and are known as diatomic
molecules.
• but in phosphorus and sulfur the atoms are joined in larger numbers, 4 and 8
respectively (P4, S8)
• The gaseous elements helium, neon, argon, krypton, xenon and radon are composed
of separate and individual atoms.
• When an element exists as separate atoms, then the molecules are said to be
monatomic.
Valency: The valency of an element is the number of electrons an atom of the
element uses to combine with atoms of other elements - it is the combining power of
an atom of the element. In an atom, the valence electrons are the electrons that can
be used in combining with other atoms - these are the electrons in the orbits of the
outermost shell (also called valence shell).
Elements :
An element is a pure substance that cannot be separated into simpler substances by
physical or chemical means.
A pure substance is a substance in which there is only one type of particle.
Elements are pure substances so each element only contains one type of particle.
Example: Every particle in a 5g nugget of the element gold is like every other particle
of gold
Every element has a unique set of properties:
Each element can be identified by its properties.
Each element has its own characteristic properties.
Characteristic properties: properties that don’t depend on the amount of material
present in a sample of the element
Characteristic Properties of Elements:
Physical Properties
Boiling Point
Melting Point
Density
Chemical Properties
Reactivity with different substances
Elements are grouped into categories based on the properties they share.
Example: Iron, nickel, and cobalt are all shiny and conduct heat and electrical
current. They’ve been placed into a large group called metals with similar
elements.
Elements are divided into:
o Metals
o Non-metals
o Metalloids
o Noble gas
Major Categories of Elements:
1. Metals: shiny, good conductors of thermal energy and electric current,
malleable (can be hammered into thing sheets) and ductile (can be drawn into thin
wires). Elements in this category :Iron, Tin, Lead, Copper
2. Non-metals: dull, poor conductors of thermal energy and electric current,
brittle and unmalleable. Elements in this category: Neon, Bromine, Sulfur
3. Metalloids: have properties of both metals and non metals, some are shiny
while others are dull, some are good conductors while others are not. Elements in this
category : Silicon, Antimony, Boron
4. Noble gas: are chemically inert and do not react with elements and compounds.
Eg: Neon,krypton.
Compounds:
Are pure substance composed of two or more elements that are chemically
combined.
In order for elements to combine, they must react, or undergo a chemical
change, with one another.
Some Familiar Compounds:
Table Salt: Sodium and Chlorine
Water: Hydrogen and Oxygen
Sugar: Carbon, Hydrogen, and Oxygen
Carbon Dioxide: Carbon and Oxygen
Baking Soda: Sodium, Hydrogen, Carbon, and Oxygen
Compounds Have Unique Sets of Properties
Compounds have different properties from the elements that form it.
Ex: Table salt is made of sodium (which reacts violently with water) and
chlorine (which is poisonous).
Compounds Can Be Broken Down into Simpler Substances by:
Either broken down into elements through chemical changes. Or undergo
chemical changes and form simpler compounds
Compounds Cannot Be Broken Down by Physical Changes
Only way to break down a compound is through a CHEMICAL change.
Chemical formulae: A compound is a substance made up of a definite proportion of two or more elements. A chemical formula tells us the number of atoms of each element in a compound. It contains the symbols of the atoms of the elements present in the compound as well as how many there are for each element in the form of subscripts.
Mixtures:
Mixture is a combination of two or more substances that are not chemically
combined
Two or more materials form a mixture if they do not react to form a compound
Substance in a mixture keep their identities.
Mixtures can be physically separated.
Homogeneous mixture:
These are the types of mixtures in which the components mixed are uniformly
distributed throughout the mixture or in other words “the same throughout”.
We can observe only one phase of matter in a homogeneous mixture. Key
points regarding this type of mixtures:
Particles are distributed uniformly
We can’t judge a homogeneous mixture by just seeing it
Homogeneous mixtures are also called as solutions
Uniform composition
Example: rainwater, vinegar, etc.
Heterogenous mixture:
This is a type of mixture in which all the components are completely mixed
and all the particles can be seen under a microscope. We can easily identify
the components and more than one phase can be seen by naked eyes.
Key points regarding this type of mixtures:
Particles are distributed non uniformly
We can judge a heterogeneous mixture by just seeing it
Non-uniform composition
Example: seawater, etc.
Practice questions:
1. Define the following:
a. Atomicity
b. Atom
c. Molecule
d. Valency
2. What are the molecular formulae of the following compounds?
Hydrochloric acid, sulphuric acid, sodium chloride, glucose, methane.
3. State 4 differences between compounds & mixtures?
4. Give one example of each:
a. Solid-solid mixture
b. Solid-liquid mixture
c. Liquid-gas mixture
5. What are the characteristic properties of a pure substance? Why do we need them?
Worksheet 1:
Video links for better understanding:
https://www.youtube.com/watch?v=aq7L84Ylx34
https://www.youtube.com/watch?v=fQ_kiFRETGI
https://www.youtube.com/watch?v=j7690jLbvZk
https://www.youtube.com/watch?v=msSclkLW4Lk
TEXTUAL SHORT QUESTION-ANSWERS FOR CH-1,2,3
FOR CH3: ELEMENTS,COMPOUNDS AND MIXTURES:
1) What are non metals? Are non metals good conductors of heat and
electricity?
It is a chemical element that does not have the properties of a metal.No
they are not good conductors of heat and electricity.
2) Which elements are required to make sugar ? Also give the chemical
formula of sugar.
Elements required for making sugar are C,H ,O.The chemical formula for
sugar is C22H11O11.
3) “The properties of a compound are the same as the properties of the
elements that make up the compound”.is this statement correct.If not correct
it.
No. The properties of a compound are not the same as the properties of
the elements that make up the compound.
4) Name a few elements whose names start with Latin names.
Sodium (Natrium) ,Iron (Ferrum) ,Gold (Aurum) and Potassium (Kalium).
5) What do you mean by chemical symbols for elements ?
The abbreviation of the name of the element to its initial letter or
second letters is called symbol of element.
6) Write down the symbols for each of these elements.
i. Potassium K
ii. Sodium Na
iii. Chlorine Cl
iv. Gold Au
v. Silver Ag
vi. Aluminium Al
vii. Calcium Ca
viii. Cobalt Co
7) Write down the names of the elements /compounds for each of these
symbols.
i. Ca Calcium
ii. MgO Magnesium Oxide
iii. CuS Copper Sulphide
iv. P Phosphorous
v. S Sulphur
vi. Sb Antimony
vii. He Helium
viii. Zn Zinc
ix. ZnO Zinc Oxide
8) Write molecular formula for each of the following:
i. Chlorine Cl2
ii. Oxygen O2
iii. Common Salt NaCl
iv. Water H2O
v. Nitrogen N2
vi. Lead Sulphide PbS
vii. Hydrogen H2
viii. Calcium Oxide CaO
9) What do you understand by the term atomicity? Give the atomicity of
sulphur.
Atomicity is defined as the number of atoms present in one molecule of
an element. The atomicity of sulphur is 8.
10) Differentiate between Homogeneous and Heterogeneous mixture
Homogeneous Mixture Heterogeneous Mixture
It is the one in which there is perfect mixing of the components of the mixture.
It is a mixture that contains physically distinct parts, each with different properties.
FOR CH2: PHYSICAL AND CHEMICAL CHANGES
1. State whether rusting of iron is a physical or chemical change? How can you
prevent rusting of iron?
Ans. Rusting of iron is a chemical change. We can prevent rusting of iron by
painting, greasing and galvanizing.
2. Is an earthquake a periodic or non-periodic change? Give reasons. Also
mention some of the losses that occur due to earthquakes.
Ans. Earthquake is a non-periodic change because it occurs at any time. Due to
earthquake there is loss of property, mankind, health etc.
3. What are periodic and non-periodic changes? Is cyclonic weather a periodic
or non-periodic change?
Ans. Periodic change- Changes which are repeated after a fixed interval of time
are known as periodic changes.
Non-periodic changes- Changes which are not repeated at regular intervals and
occur irregularly are called non-periodic changes.
Cyclonic weather is a non-periodic change.
4. Is falling of leaves from a tree an irreversible change? Give reasons.
Ans. Yes, falling of leaves from a tree is an irreversible change because we
cannot put leaves back to the tree.
5. Give three characteristics of a physical change.
Ans. a) A physical change is temporary and easily reversible.
b) No new substances are formed during a physical change.
c) Heat may be given out or absorbed in a physical change.
6. Give three characteristics of a chemical change.
Ans. a) New substances, entirely with new properties are formed during a
chemical change.
b) Chemical change cannot be reversed to get the original substance.
c) Chemical changes are accompanied with change in energy in the form of
heat, light or sound.
FOR CH1:MATTER AND ITS COMPOSITION:
1. Why can’t we see atoms with naked eyes ?
• Atoms are too small in size, so it cannot be seen with naked eyes.
2. Can we change solid iron into liquid? If yes how?
• Yes, we can change solid iron into liquid by heating it.
3. Why can’t we compress the solid block of steel?
• The particles of solids are closely packed, intermolecular space is less
and intermolecular force of attraction is strongest. So we can’t compress the
solid block of steel.
4. Why gases do not have definite volume?
• The molecules of gases lie far apart from each other, intermolecular
space are very large and intermolecular force of attraction is weak .As a result
gases do not have definite volume.
5. Why can liquids flow whereas solids can be heaped ?
• In liquid molecules , particles are at greater distance. Intermolecular
forces between molecules is less. However in solids the bonds are very strong
and prevent molecules from moving around.