Answer:
An ice cube melts when a person holds it in his hand.
Explanation:
B.they increase the concentration of reactants
C.they decrease the concentration of products
D. They act as reactants
Answer:
D) They act as reactants
Explanation:
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FALSE
lithium atom
potassium atom
sodium atom
The atoms having partially filled shells have orbitals with electrons half or less than the number of electrons that can be accomodated in it. The atom which has a partially filled second electron shell in the ground state is lithium.
Lithium is 3rd element in periodic table and thus having 3 electrons in it. The main shell electronic configuration of lithium is written as K=2, L=1. Thus the second shell L has only one electron and it is said to be partially filled.
The element hydrogen is having only one electron located in the K shell and it have o more shells which are filled.
The elements sodium and potassium are first group elements sodium with 11 electrons and potassium atom with 19 electrons. Both are having 3 main shells and one electron in the last shell. Thus their second shell is completely filled.
Hence, the atom which have partially filled second electron shell in the ground state among the following is lithium. Thus, option B is correct.
To find more about lithium, refer the link below;
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True
As the shorter the bond, the stronger it is hence more energy will be required to overcome this bond
The statement 'The longer the bond, the smaller the bond enthalpy' is true as bond length and bond enthalpy have an inverse relationship. As bond strength increases (with an increase in electron pairs in the bond), bond length decreases. So longer bonds, indicating weaker bonding, have smaller bond enthalpies.
The statement 'The longer the bond, the smaller the bond enthalpy' is true. The bond length and bond enthalpy have an inverse relationship. As the strength of a bond increases with the increase in the number of electron pairs, the bond length decreases. Thus, triple bonds are generally stronger and shorter than double bonds between the same two atoms, and by the same logic, double bonds are stronger and shorter than single bonds.
For example, if we consider the bonds between carbon and various atoms in a group, we find the bond strength typically decreases as we move down the group - C-F has a bond enthalpy of 439 kJ/mol, C-Cl has 330 kJ/mol, and C-Br is at 275 kJ/mol.
The bond energy, essentially the enthalpy required to break the bond, is a representation of its strength. Thus, a longer bond, indicating weaker bonding, will have a smaller bond enthalpy.
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