Explanation

A dipole moment is a measure of the net polarity or charge separation within a molecule or bond,

Indicating the extent to which a distance separates positive and negative charges.

It is a vector quantity, meaning it has both a magnitude (the amount of charge separation)

And a direction (from the negative to the positive charge). 

Explanation

 Metallic bonding is best described as the electrostatic attraction between a sea of delocalized electrons

And a lattice of positively charged metal ions.

In this type of chemical bond, outer electrons are shared among all the atoms in a metal,

Creating a common pool of electrons that are free to move throughout the entire structure.

This unique electron arrangement is responsible for the characteristic physical properties of metals,

Such as high electrical and thermal conductivity, ductility, and strength. 

Explanation

VSEPR theory is used to predict the 3-D molecular geometry or shape of molecules by considering the repulsion

Between electron pairs in the valence shell of an atom,

Which arrange themselves to minimize this repulsion. 

Explanation

The bond angle in a water molecule is approximately 104.5 degrees.

This angle is smaller than the ideal tetrahedral angle of 109.5 degrees

Because the two lone pairs of electrons on the oxygen atom exert more repulsion

Than the bonded hydrogen atoms, pushing the O-H bonds closer together. 

Explanation

Explanation

• Atomic radius decreases along a period as you move from left to right.
• This is because the number of protons in the nucleus increases, which pulls the electrons closer to the nucleus, resulting in a smaller atomic radius.

Explanation

Explanation

One mole of any substance contains Avogadro's number of particles.  

So, 1 mole of NaCl contains 6.022 × 10²³ formula units.

Explanation

• An atom typically has an equal number of electrons and protons.
• They are equal in number to the atomic number (Z) of the element.
• This number is unique to each element and determines the properties of the element.

Explanation

• Across a period: Ionization energy increases (stronger nuclear charge).
• Down a group: Ionization energy decreases (electron shielding + distance).
• Exceptions within a period:
  • Group 13: slight dip (new p subshell).
  • Group 16: slight dip (electron pairing repulsion).