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SUPER
Science
10th
grade
CBSE Board Class X Science Sample Paper - 1 Term 2_2
119 questions
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- 1. Multiple Choice
Which of the "Halogens" is found in liquid state at room temperature?
Flourine
Chlorine
Iodine
Bromine
- 2. Multiple Choice
Which of the "Halogens" is found in liquid state at room temperature?
Flourine
Chlorine
Iodine
Bromine
- 3. Multiple Choice
Which of the "Halogens" has yellowish green color?
Chlorine
Bromine
Flourine
Iodine
- 4. Multiple Choice
Which of these elements are Halogens?
Fluorine
Helium
Zinc
Bromine
- 5. Multiple Choice
What group are the Halogens?
6.9
7
8
3
- 6. Multiple Choice
You've seen the name many times, how do you spell it?
Halogens
Helogens
Hallogens
Halogans
- 7. Multiple ChoiceAt room temperature, chlorine is...a yellow-green gasa brown gasa yellow-green liquid
- 8. Multiple Choice
As you move down the group, halogens' reactivity...
increases
decreases
doesn't change
shows no trend.
- 9. Multiple ChoiceAt room temperature, iodine is a....GasLiquidSolid
- 10. Multiple Choice
How many electrons do the halogens all have in their outer shells?
1
2
7
8
- 11. Multiple Choice
The Halogens are found in which group number?
5
6
7
0
- 12. Multiple Choice
All halogens attract 1 electron to their outer shell to become stable.
true
false
- 13. Multiple Choice
All halogens lose 7 electrons from their outer shell to become stable.
true
false
- 14. Multiple Choice
Which one is the odd one out?
Bromine
Fluorine
Chlorine
- 15. Multiple Choice
Which halogens is a solid?
iodine
fluorine
bromine
chlorine
- 16. Multiple Choice
Which halogens are gases?
iodine
fluorine
bromine
chlorine
- 17. Multiple Choice
The nucleus of which halogen is best at attracting electrons?
fluorine
iodine
bromine
chlorine
- 18. Multiple Choice
Which halogen is the most reactive?
iodine
chlorine
bromine
fluorine
- 19. Multiple Choice
Which halogen is the least reactive?
iodine
chlorine
bromine
fluorine
- 20. Multiple Choice
Which halogen is a purple-black solid?
iodine
chlorine
bromine
fluorine
- 21. Multiple Choice
Which halogen has the biggest atoms?
iodine
chlorine
bromine
fluorine
- 22. Multiple Choice
What is the chemical formula of Magnesium chloride?
MgCl
MgCl2
MgC
MgC2
- 23. Multiple Choice
An element X belongs to Group 17 and the third period of the periodic table.
is it a metal or non metal
Metal
NON METAL
- 24. Multiple Choice
Valency of the elements in the halogen group is _______.
(A) one
(B) two
(C) three
(D) four
- 25. Multiple Choice
An element X belongs to Group 17 and the third period of the periodic table. Give the formula of the compound formed when it combines with an element Y having a valency three.
The formula of the compound formed when element X combines with an element Y is YX3.
The formula of the compound formed when element X combines with an element Y is YX2
The formula of the compound formed when element X combines with an element Y is YX
- 26. Fill in the Blank
An element X belongs to Group 17 and the third period of the periodic table. (a) Write the electronic configuration of the element
- Comprehension for next 20 questions
The video talks about different types of bonds between atoms. The speaker introduces the concept with an ionic bond, then explains covalent bond.
An ionic bond is formed between an atom that wants to give away an electron (like sodium) and an atom that wants to gain an electron (like chlorine). When they bond, they form ions (charged particles) because one loses an electron and becomes positively charged, while the other gains an electron and becomes negatively charged. They are attracted to each other because of the opposite charges.
Covalent bonds are different because they form between two atoms that each want to gain an electron. Instead of giving away or taking electrons from each other, they share electrons. The sharing allows each atom to feel like it has a complete outer shell, which makes the bond stable. Hydrogen is used as an example. A hydrogen atom has one electron, and it would need another electron to have a complete outer shell. When two hydrogen atoms come together, they can share their electrons. Each atom feels like it has two electrons, even though they are really sharing.
27. Multiple Choice30 seconds1 ptWhat does Ohm's Law explain the relationship between in an electric circuit?
Voltage and resistance
Current and resistance
Current and voltage
Power and resistance
28. Multiple Choice30 seconds1 ptWhat does the linear relationship between current and voltage confirm?
Newton's Law
Boyle's Law
Ohm's Law
Archimedes' Principle
29. Multiple Choice30 seconds1 ptHow is the relationship between current and voltage validated?
By solving complex equations
By conducting experiments
By reading textbooks
By guessing randomly
30. Multiple Choice30 seconds1 ptHow does increasing the number of batteries in series affect current and voltage readings?
Decreases current and voltage readings
Has no effect on current and voltage readings
Increases current readings but decreases voltage readings
Increases current and voltage readings
31. Multiple Choice30 seconds1 ptWho discovered Ohm's Law in 1827?
Isaac Newton
Georg Simon Ohm
Albert Einstein
Nikola Tesla
32. Multiple Choice30 seconds1 ptAccording to Ohm's Law, what is directly proportional to the current flowing through a metallic wire?
Resistance
Voltage
Power
Temperature
33. Multiple Choice30 seconds1 ptWhat components are used in the electric circuit to demonstrate Ohm's Law?
Resistor, capacitor, inductor
Bulb, battery, ammeter, voltmeter
Switch, wire, transformer
Motor, diode, fuse
34. Multiple Choice30 seconds1 ptWhat concept does the video aim to explain?
Ohm's Law
The history of the companyThe benefits of exerciseThe process of baking a cake35. Multiple Choice30 seconds1 ptWhat device measures the current in the circuit?
VoltmeterOscilloscopeThermometerAmmeter
36. Multiple Choice30 seconds1 ptHow is the voltmeter connected in the circuit?
In parallelAt the outputAt the inputIn series37. Multiple Choice45 seconds1 ptWhat happens when the switch is turned on in the circuit?
Current flows through the circuitThe temperature increasesThe circuit breaksThe lights turn on
38. Multiple Choice30 seconds1 ptWho discovered the relationship between current and voltage, known as Ohm's Law?
Isaac NewtonAlbert EinsteinNikola TeslaGeorg Simon Ohm39. Multiple Choice30 seconds1 ptAccording to Ohm's Law, what is the relationship between voltage and current?
ExponentialDirectly proportionalConstantInverse proportional40. Multiple Choice45 seconds1 ptWhat is the significance of the proportionality constant in Ohm's Law?
The significance of the proportionality constant in Ohm's Law is that it represents the resistance of the material through which the current is flowing.It determines the voltage drop across the circuitIt represents the power dissipated in the circuitIt indicates the current flowing through the circuitIt relates the voltage and current in the circuit
41. Multiple Choice30 seconds1 ptWhat material is the metallic wire typically made of in electrical circuits?
GoldAluminumSteelCopper42. Multiple Choice30 seconds1 ptHow is the potential difference across the ends of a metallic wire related to the current flowing through it?
Inversely proportionalNo relationDirectly proportionalExponentially related43. Multiple Choice30 seconds1 ptWhat remains constant for Ohm's Law to be applicable in a circuit?
PowerCurrentVoltageTemperature
44. Multiple Choice30 seconds1 ptIn the experiment described in the passage, what happened to the current when more batteries were connected in series?
The current increased.
The current decreased.The current fluctuated.The current remained the same.45. Multiple Choice30 seconds1 ptWhat is the unit of electrical potential difference?
amperesvoltswattsohms46. Multiple Choice30 seconds1 ptWho discovered Ohm's Law?
Isaac NewtonNikola TeslaGeorg Simon OhmAlbert Einstein - Comprehension for next 26 questions
The video talks about different types of bonds between atoms. The speaker introduces the concept with an ionic bond, then explains covalent bond.
An ionic bond is formed between an atom that wants to give away an electron (like sodium) and an atom that wants to gain an electron (like chlorine). When they bond, they form ions (charged particles) because one loses an electron and becomes positively charged, while the other gains an electron and becomes negatively charged. They are attracted to each other because of the opposite charges.
Covalent bonds are different because they form between two atoms that each want to gain an electron. Instead of giving away or taking electrons from each other, they share electrons. The sharing allows each atom to feel like it has a complete outer shell, which makes the bond stable. Hydrogen is used as an example. A hydrogen atom has one electron, and it would need another electron to have a complete outer shell. When two hydrogen atoms come together, they can share their electrons. Each atom feels like it has two electrons, even though they are really sharing.
47. Multiple Choice30 seconds1 ptWhat type of bonds are formed between atoms that want to give away or gain electrons?
Covalent bonds
Metallic bonds
Ionic bonds
Hydrogen bonds
48. Multiple Choice30 seconds1 ptWhat happens to the charge of atoms in an ionic bond?
Both atoms become positively charged
Both atoms become negatively charged
One atom becomes positively charged and the other becomes negatively charged
Both atoms remain neutral
49. Multiple Choice30 seconds1 ptHow do covalent bonds differ from ionic bonds?
They involve electron sharing rather than electron transfer.
They involve electron transfer rather than electron sharing.
They involve proton sharing rather than electron transfer.
They involve neutron sharing rather than electron transfer.
50. Multiple Choice30 seconds1 ptWhat type of bonds form between atoms that each want to gain an electron?
Ionic bonds
Covalent bonds
Metallic bonds
Hydrogen bonds
51. Multiple Choice30 seconds1 ptWhy is the concept of complete outer shells crucial for understanding the stability of different types of bonds?
It determines the color of the bond
It affects the length of the bond
It influences the strength of the bond
It determines the shape of the bond
52. Multiple Choice30 seconds1 ptWhat are the two types of bonds discussed in the video?
Ionic bonds and metallic bonds
Covalent bonds and hydrogen bonds
Ionic bonds and covalent bonds
Metallic bonds and hydrogen bonds
53. Multiple Choice30 seconds1 ptWhat is hydrogen used as an example of in covalent bonding?
Ionic bonding
Metallic bonding
Covalent bonding
Van der Waals forces
54. Multiple Choice30 seconds1 ptWhat type of bond is formed between atoms that want to give away and gain electrons?
Metallic bondHydrogen bondCovalent bondIonic bond55. Multiple Choice30 seconds1 ptWhat happens to the atoms when they form an ionic bond?
Atoms lose or gain electrons to form charged ions.Atoms gain or lose neutrons to form charged ionsAtoms lose protons to form charged ionsAtoms share electrons equally56. Multiple Choice30 seconds1 ptWhat charge do ions have in an ionic bond?
Opposite chargesSame chargesVariable chargesNeutral charges57. Multiple Choice30 seconds1 ptHow do atoms in a covalent bond achieve stability?
a) By gaining electrons
b) By losing electrons
c) By sharing electrons
d) By transferring protons
58. Multiple Choice30 seconds1 ptWhich example is used to illustrate a covalent bond?
The bond between two hydrogen atoms in a hydrogen molecule (H2)The bond between sodium and chlorine in sodium chloride (NaCl)The bond between two oxygen atoms in an oxygen molecule (O2)The bond between a metal and a non-metal in an ionic compound59. Multiple Choice30 seconds1 ptHow many electrons does a hydrogen atom have?
032160. Multiple Choice30 seconds1 ptWhat is the purpose of electron sharing in a covalent bond?
To create an unstable electron configurationTo form ionic bondsTo increase the reactivity of the atoms involvedTo achieve a stable electron configuration by filling valence shells.61. Multiple Choice30 seconds1 ptHow many electrons do hydrogen atoms feel like they have when they share electrons?
243162. Multiple Choice30 seconds1 ptWhat makes a covalent bond stable?
Presence of metallic ionsShared electrons creating a balanced and low-energy stateHigh-energy state due to unshared electronsOpposite charges attracting each other63. Multiple Choice30 seconds1 ptWhich type of bond involves atoms each wanting to gain an electron?
Metallic bondCovalent bondIonic bondHydrogen bond64. Multiple Choice30 seconds1 ptWhat is formed when two or more atoms form a chemical bond?
solutionelementmoleculecompound65. Multiple Choice30 seconds1 ptWhich type of elements typically form covalent compounds?
Alkali metalsNonmetal elementsMetal elementsNoble gases66. Multiple Choice30 seconds1 ptIn the compound water (H2O), how many electrons are shared between each hydrogen and oxygen atom?
431267. Multiple Choice30 seconds1 ptWhat is a characteristic of covalent compounds regarding melting and boiling points?
Higher melting and boiling pointsNo melting or boiling pointsInconsistent melting and boiling pointsLower melting and boiling points68. Multiple Choice30 seconds1 ptWhat are ionic compounds made up of?
Positively and negatively charged ionsOnly negatively charged ionsNeutral atomsOnly positively charged ions69. Multiple Choice30 seconds1 ptWhich compound is mentioned as an example of an ionic compound?
Calcium carbonate (CaCO3)Sodium chloride (NaCl)Hydrogen peroxide (H2O2)Sulfuric acid (H2SO4)70. Multiple Choice30 seconds1 ptWhat characteristic do ionic compounds typically have in terms of melting and boiling points?
VariableMediumLowHigh71. Multiple Choice30 seconds1 ptHow do ionic compounds behave when struck?
Ionic compounds explodeIonic compounds meltIonic compounds shatter/ They break apart
Ionic compounds bend72. Multiple Choice30 seconds1 ptWhen dissolved in a solution, ionic compounds are:
Merged into moleculesConverted into atomsTransformed into covalent bondsDissociated into ions - Comprehension for next 17 questions
Noble gases, comprising helium, neon, argon, krypton, xenon, and radon, possess unique properties and find various applications in real-life scenarios. Notably, these elements, located in Group 18 of the periodic table, boast full valence electron shells, rendering them highly stable. Historically labeled as inert or unreactive gases due to their stability, some noble gases can indeed form compounds, leading to their modern classification as noble gases.
Characterized by their colorlessness and monatomic nature, noble gases exhibit increasing atomic size and boiling points down the group, as the number of electron shells rises. Consequently, their intermolecular forces and density increase correspondingly. Despite their stability and limited reactivity, noble gases have diverse practical applications.
Helium, for instance, is widely used to fill party balloons and airships due to its buoyancy. In industry, krypton and xenon find use in lasers, flat panel displays, and automotive headlights, enhancing brightness and safety. Neon emits a distinctive orange light when subjected to electrical current, making it suitable for light bulbs. Argon, utilized in light bulb filling, offers non-reactivity with tungsten filaments.
Moreover, noble gases contribute to medical advancements. Xenon serves as a natural anesthetic, aiding in surgical procedures with minimal side effects. Conversely, radon's radioactivity is harnessed in cancer treatment through radiotherapy. Beyond conventional applications, krypton enhances insulation in double glazing, while xenon propels satellites, facilitating orbital maneuvers in space exploration.
In summary, noble gases' inherent stability underpins their myriad practical applications across industries, from lighting and insulation to medicine and space exploration.
73. Multiple Choice30 seconds1 ptWhat are some applications of krypton and xenon?
Filling party balloons
In lasers and automotive headlights
In cooking gas
In mobile phones
74. Multiple Choice30 seconds1 ptWhat is one application of xenon mentioned in the passage?
Enhancing insulation in double glazing
Propelling satellites in space exploration
Generating electricity in nuclear power plants
Producing light in neon signs
75. Multiple Choice30 seconds1 ptWhat properties of noble gases exhibit increasing trends down the group?
Atomic number and melting points
Atomic size and boiling points
Ionization energy and electronegativity
Density and reactivity
76. Multiple Choice30 seconds1 ptWhat enables diverse applications in lighting, medicine, and space technology?
High reactivity
Low stability
Noble gases' stability
Radioactive properties
77. Multiple Choice30 seconds1 ptWhat is xenon used for in medical procedures?
As a natural anesthetic
As a cancer treatment
As a painkiller
As a disinfectant
78. Multiple Choice30 seconds1 ptWhere are noble gases located in the periodic table?
Group 1
Group 18
Group 7
Group 12
79. Multiple Choice30 seconds1 ptWhat are some practical applications of noble gases in various industries?
Medical imaging
Lighting
Cryogenics
Agriculture
80. Multiple Choice30 seconds1 ptWhat group do noble gases belong to in the periodic table?
Group 18Group 15Group 12Group 781. Multiple Choice30 seconds1 ptHow many valence electrons do noble gases typically have?
6108482. Multiple Choice30 seconds1 ptWhat were noble gases historically referred to as due to their stability?
reactive gasesvolatile gasescombustible gasesinert gases83. Multiple Choice30 seconds1 ptWhich noble gas emits a bright orange light when an electrical current is passed through it?
NeonXenonKryptonArgon84. Multiple Choice30 seconds1 ptWhat is the increasing trend of boiling points observed down the noble gas group attributed to?
Increase in atomic size and London dispersion forcesDecrease in atomic size and ionic bondingIncrease in atomic size and covalent bondingDecrease in atomic size and hydrogen bonding85. Multiple Choice30 seconds1 ptWhat is one practical application of helium mentioned in the passage?
Purifying drinking waterHeating systems in residential homesCooling superconducting magnets in MRI machines and filling balons
Enhancing the flavor of food products86. Multiple Choice30 seconds1 ptWhat noble gas is used in radiotherapy for cancer treatment due to its radioactivity?
RadonArgonXenonKrypton87. Multiple Choice30 seconds1 ptWhat is the characteristic property of argon that makes it suitable for filling light bulbs?
Highly reactive and prone to corrosionIncompatible with electrical circuitsEmits toxic fumes when exposed to heatNon-reactive and does not corrode with tungsten filaments
88. Multiple Choice30 seconds1 ptWhich noble gas is used to enhance insulation in double glazing?
KryptonXenonNeonArgon89. Multiple Choice30 seconds1 ptIn what industry is xenon used as a propellant?
ChemicalAutomotiveAerospaceMedical - Comprehension for next 30 questions
In this lesson, we delve into the alkaline earth metals found in Group 2 of the periodic table, with a particular focus on magnesium and calcium. These metals, including beryllium, magnesium, calcium, strontium, barium, and radium, share commonalities such as having two electrons in their valence shell. With the exception of beryllium, they can lose these electrons to form ions with a +2 charge.
Similar to alkali metals, alkaline earth metals are typically stored in oil to prevent reactions with air. Moving down the group, their density and reactivity increase, while melting and boiling points decrease, and they become softer. Specifically, we explore the reactions of magnesium and calcium with oxygen and water.
Magnesium, typically shiny but often coated with an oxide layer, reacts with oxygen to form magnesium oxide, accompanied by a bright white flash. On the other hand, calcium, softer than magnesium, also reacts with oxygen to produce calcium oxide, burning with a red flame. When these oxides react with water, magnesium oxide yields magnesium hydroxide and hydrogen gas, while calcium oxide produces calcium hydroxide and hydrogen gas, with calcium demonstrating a more vigorous reaction with water compared to magnesium.
It's worth noting that magnesium reacts with steam to form magnesium oxide and hydrogen gas. Through these reactions, we gain insights into the properties and reactivity of alkaline earth metals, mirroring trends observed in the alkali metal group.
90. Multiple Choice30 seconds1 ptWhat insights do the reactions of magnesium and calcium with oxygen and water provide into the behavior of alkaline earth metals?
They provide insights into the reactivity of alkaline earth metals
They provide insights into the color of alkaline earth metals
They provide insights into the melting point of alkaline earth metals
They provide insights into the electrical conductivity of alkaline earth metals
91. Multiple Choice30 seconds1 ptWhat does magnesium react with to form magnesium oxide and hydrogen gas?
Water
Oxygen
Carbon dioxide
Nitrogen
92. Multiple Choice30 seconds1 ptWhat group of elements exhibit trends in properties and reactivity similar to those observed in the alkali metal group?
Transition metals
Noble gases
Alkaline earth metals
Halogens
93. Multiple Choice30 seconds1 ptWhat is a common characteristic of alkaline earth metals in Group 2 of the periodic table?
They have one electron in their valence shell
They have two electrons in their valence shell
They have three electrons in their valence shell
They have four electrons in their valence shell
94. Multiple Choice30 seconds1 ptWhat color flame does calcium produce when reacting with oxygen?
Bright white
Red
Blue
Green
95. Multiple Choice30 seconds1 ptWhy are alkaline earth metals typically stored in oil?
To prevent reactions with air
To increase their density
To decrease their reactivity
To enhance their color
96. Multiple Choice30 seconds1 ptWhat is the product of the reaction between magnesium oxide and water?
Magnesium hydroxide and hydrogen gas
Calcium hydroxide and hydrogen gas
Magnesium oxide and water
Calcium oxide and water
97. Multiple Choice30 seconds1 ptWhat group in the periodic table do alkaline earth metals belong to?
Group 3Period 2Family 1Group 298. Multiple Choice30 seconds1 ptHow many electrons do alkaline earth metals typically have in their valence shell?
826499. Multiple Choice30 seconds1 ptWhich of the following alkaline earth metals cannot form ions with a +2 charge?
BerylliumMagnesiumStrontiumCalcium100. Multiple Choice30 seconds1 ptWhat is the primary difference between the reactivity of magnesium and calcium?
Calcium is more reactive than magnesium.Both magnesium and calcium have the same reactivity.Magnesium is more reactive than calcium.Magnesium is less reactive than calcium.101. Multiple Choice30 seconds1 ptWhich gas is produced when magnesium reacts with steam?
Oxygen gasCarbon dioxideNitrogen gasHydrogen gas102. Multiple Choice30 seconds1 ptWhat is the product when calcium reacts with cold water?
Calcium oxide and oxygen gasCalcium carbonate and water vaporCalcium hydroxide and hydrogen gasCalcium chloride and hydrogen gas103. Multiple Choice30 seconds1 ptWhich alkaline earth metal sinks to the bottom when reacting with water?
CalciumStrontiumBariumMagnesium104. Multiple Choice30 seconds1 ptWhat characteristic color does the flame turn when calcium reacts with oxygen?
Brick redYellowBlueGreen105. Multiple Choice30 seconds1 ptWhat happens when magnesium reacts with oxygen?
Magnesium hydroxide is formed.Magnesium oxide is formed.Magnesium chloride is formed.Magnesium sulfate is formed.106. Multiple Choice30 seconds1 ptHow do the properties of alkaline earth metals compare to those of alkali metals?
Alkaline earth metals have lower melting points, densities, and boiling points compared to alkali metals.Alkaline earth metals have lower ionization energies and are more reactive than alkali metals.Alkaline earth metals are located in Group 1 of the periodic table, while alkali metals are in Group 2.Alkaline earth metals have higher melting points, densities, and boiling points compared to alkali metals. They also have higher ionization energies and are less reactive than alkali metals.107. Multiple Choice30 seconds1 ptAlkali metals are found in which group of the periodic table?
Noble gasesGroup 1Period 3Group 7108. Multiple Choice30 seconds1 ptWhich of the following earth metal is the most reactive in water?
MagnesiumBariumCalciumStrontium109. Multiple Choice30 seconds1 ptWhich of the following is NOT an alkali metal?
IronLeadGoldMercury110. Multiple Choice30 seconds1 ptWhich is the lightest alkali metal?
Sodium (Na)Potassium (K)Rubidium (Rb)Lithium (Li)111. Multiple Choice30 seconds1 ptWhat is the atomic number of lithium?
5739112. Multiple Choice30 seconds1 ptMendeleev organized the elements by atomic mass in each of the rows. How are they actually organized?
By atomic weightBy group numberBy melting pointBy atomic number113. Multiple Choice30 seconds1 ptWhich alkali earth metal is commonly used in fireworks to produce a red color?
PotassiumLithiumBariumStrontium114. Multiple Choice30 seconds1 ptWhich alkali earth metal is known for its high reactivity with water?
Barium (Ba)Magnesium (Mg)Sodium (Na)Calcium (Ca)115. Multiple Choice30 seconds1 ptWhat is the most abundant alkali earth metal in the Earth's crust?
SodiumPotassiumBariumCalcium116. Multiple Choice30 seconds1 ptWhich alkali earth metal is used in the production of magnesium alloys?
StrontiumBariumSodiumCalcium117. Multiple Choice30 seconds1 ptWhat is the atomic number of strontium?
36384240118. Multiple Choice30 seconds1 ptWhich alkali earth metal is used in the manufacture of batteries?
potassiumsodiumlithiumcalcium119. Multiple Choice30 seconds1 ptWhich alkali earth metal is used in the treatment of osteoporosis?
LithiumBerylliumMagnesiumStrontium - Answer choicesTagsAnswer choicesTags