MUET Entry Test 2016 Past Paper

Magnetic Q.No. specifies:

A. Size of orbital
B. Shape of orbital
C. Orientation of orbital
D. Nuclear stability

C. Orientation of orbital

The magnetic quantum number (m_l) specifies:

C. Orientation of orbital

Here’s a breakdown of the quantum numbers and their specifications:

  • Principal quantum number (n): This specifies the energy level or shell of the electron.
  • Azimuthal quantum number (l): This specifies the subshell of the electron (s, p, d, f). It’s related to the shape of the orbital.
  • Magnetic quantum number (m_l): This specifies the orientation of the orbital within a subshell. Since orbitals of the same subshell have the same shape but may have different orientations in space, m_l helps distinguish them.
  • Spin quantum number (m_s): This specifies the spin of the electron along a chosen axis (usually +1/2 or -1/2).

So, the magnetic quantum number focuses on how an orbital is oriented in space, not its size or nuclear stability.

Magnetic Q.No. specifies: Read More »

The elements required to the soil in small amounts are called:

A. Micronutrients
B. Macronutrients
C. Meganutrients
D. Microscopic

A. Micronutrients

Micronutrients are essential for plant growth, even though they are needed in much smaller quantities compared to macronutrients. They play various roles in plant physiology, but only a tiny amount is sufficient. Examples of micronutrients include boron, copper, iron, and zinc.

Here’s a breakdown of the other options:

  • B. Macronutrients: These are elements required by plants in relatively large amounts. Examples include nitrogen, phosphorus, and potassium.
  • C. Meganutrients: This term is not a standard scientific term used in soil science.
  • D. Microscopic: Microscopic refers to the size of something being very small and needing a microscope to see. While some micronutrients may have microscopic particles, it doesn’t describe their function in the soil.

The elements required to the soil in small amounts are called: Read More »

The maximum concentration of substrate above which increase of substrate concentration does not increase the rate of reaction is called _______ of enzymes with substrate.

A. Termination
B. Saturation
C. Fluctuation
D. Maximum Optimation

B. Saturation

Enzymes are biological catalysts that accelerate the rate of chemical reactions. As the concentration of substrate increases, the rate of the reaction also increases due to more frequent collisions between enzyme and substrate molecules. However, there’s a limit:

  • Saturation: At a certain point, all the active sites of the enzyme molecules become occupied by substrate molecules. Increasing the substrate concentration further won’t affect the reaction rate because there are no free enzyme molecules available to bind with the additional substrate. This maximum concentration of substrate is called the saturation concentration.

The other options don’t accurately describe this concept:

  • Termination: Termination refers to the final step in a reaction pathway, not the limitation of substrate binding.
  • Fluctuation: Fluctuation implies random variations, not the specific point of maximum binding.
  • Maximum Optimation: This term isn’t commonly used in enzyme kinetics.

The maximum concentration of substrate above which increase of substrate concentration does not increase the rate of reaction is called _______ of enzymes with substrate. Read More »

An alkyl halide reacts with aqueous KOH solution to give an:

A. Aldehyde
B. Alkane
C. Alcohol
D. Acid

C. Alcohol

The reaction of an alkyl halide with aqueous KOH solution typically results in the formation of an alcohol.

Here’s why:

  • Alkyl halide: This represents a molecule where a halogen atom (Cl, Br, I, or F) is bonded to an alkyl group (a hydrocarbon chain).
  • Aqueous KOH solution: This refers to potassium hydroxide (KOH) dissolved in water. KOH acts as a strong base, with the OH⁻ ion being the nucleophile (electron-rich species) that attacks the alkyl halide.

In the reaction, the nucleophilic OH⁻ ion attacks the carbon atom bonded to the halogen in the alkyl halide. The halogen atom leaves as a halide ion (Cl⁻, Br⁻, I⁻, or F⁻), and a new C-O bond is formed, creating an alcohol.

Therefore, the answer is:

C. Alcohol

An alkyl halide reacts with aqueous KOH solution to give an: Read More »

The elements in which ‘d’ or ‘f’ orbitals are incomplete either in the atomic state or in their common ions are called:

A. Trans uranium elements
B. Transition elements
C. Lanthanides
D. Actinides

B. Transition elements

  • Transition elements: These elements (groups 3-12 in the periodic table) have incompletely filled d-orbitals in either their atomic state or in their common ions. This incomplete filling of d-orbitals contributes to their characteristic properties, including variable oxidation states, ability to form colored compounds, and involvement in coordination complexes.

The elements in which ‘d’ or ‘f’ orbitals are incomplete either in the atomic state or in their common ions are called: Read More »

Aluminum reacts slowly with dil. H2SO4 to produce:

A. Nitrogen gas
B. Oxygen gas
C. Hydrogen gas
D. Sulphur dioxide gas

C. Hydrogen gas

When aluminum reacts with dilute sulfuric acid (H₂SO₄), it undergoes a single displacement reaction. Here’s the balanced chemical equation for this reaction:

2Al(s) + 3H₂SO₄(aq) → 3H₂(g) + Al₂(SO₄)₃(aq)

As you can see, the reaction produces hydrogen gas (H₂) and aluminum sulfate (Al₂(SO₄)₃).

Aluminum reacts slowly with dil. H2SO4 to produce: Read More »

Electrical conductivity of alkaline earth metals _____ from Be to Ra.

A. Remains disturbed
B. Remains same
C. Increases
D. Decreases

C. Increases

The electrical conductivity of alkaline earth metals increases from Be to Ra.

Here’s why:

As we move down the group (Be to Ra) in the periodic table for alkaline earth metals:

  • Atomic size increases: The outer electrons are further away from the nucleus, experiencing a weaker attractive force. This makes them more readily available for conduction.
  • Number of valence electrons remains the same (2): All alkaline earth metals have two valence electrons in their outermost shell, which they can contribute to conduction.

The combined effect of increasing atomic size and readily available valence electrons leads to improved electrical conductivity down the group from Be to Ra.

Electrical conductivity of alkaline earth metals _____ from Be to Ra. Read More »

Hydrogen, an ordinary temperature and pressure exist in nature in the:

A. Solid state
B. Liquid state
C. Gaseous state
D. Plasma state

C. Gaseous state

At ordinary temperature (around room temperature) and pressure, hydrogen exists as a gas. It’s the lightest element and due to its weak intermolecular forces, it readily fills the available volume as a gas.

  • Solid hydrogen: Requires extremely low temperatures (below -259°C) to solidify.
  • Liquid hydrogen: Achieved at very low temperatures (around -253°C) and remains a liquid even at room temperature if kept in a well-insulated container.
  • Plasma state: Requires very high temperatures and is not the typical state for hydrogen under normal conditions.

Hydrogen, an ordinary temperature and pressure exist in nature in the: Read More »

Coinage metals are elements of sub-group I-B and these includes:

A. Cu, Ag, Au
B. Zn, Cd, Hg
C. Fe, Co, Ni
D. Cu, Zn, Ni

A. Cu, Ag, Au

Coinage metals are elements of subgroup I-B and these include:

  • Copper (Cu)
  • Silver (Ag)
  • Gold (Au)
     

Subgroup I-B, also known as group 11, is located on the left side of the p-block in the periodic table. These elements are known for their excellent electrical conductivity, malleability, and ductility. Their unique properties make them ideal for use in various applications, including:

  • Electrical wiring: Copper is widely used in electrical wires due to its high conductivity.
  • Jewelry: Silver and gold are popular choices for jewelry because of their lustrous appearance and ability to be shaped into intricate designs.
  • Electronics: Gold is used in electronic components due to its resistance to corrosion.
  • Coins: Historically, copper, silver, and gold were the primary metals used to mint coins. Although less common today, some collector’s coins and high-value currencies may still incorporate these metals.

Coinage metals are elements of sub-group I-B and these includes: Read More »

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