Periodic Table and Electron Configuration

Mrs. Jeevan discusses atomic identity and reactivity, focusing on how protons determine an element's identity and valence electrons influence chemical properties. The video covers the structure of the periodic table, explaining periods and groups, and how they relate to atomic identity. It introduces Bohr models and Lewis dot structures to visualize atomic structure and electron placement. The video also explores atomic reactivity, highlighting the role of valence electrons in predicting reactivity and stability, with examples of reactive and stable elements.

What determines the identity of an element?

• Number of valence electrons

• Number of electrons

• Number of protons

• Number of neutrons

Which element has an atomic number of 7?

• Carbon

• Nitrogen

• Helium

• Oxygen

In a Bohr model, how many electrons can the first ring hold?

• Eight

• Six

• Four

• Two

How many valence electrons does carbon have?

• Eight

• Two

• Four

• Six

What is the maximum number of valence electrons a Lewis dot structure can show?

• Four

• Six

• Ten

• Eight

Which group in the periodic table is known for being stable and non-reactive?

• Group 3

• Group 18

• Group 7

• Group 1

What happens to metals in terms of electron transfer to become stable?

• They share electrons

• They lose electrons

• They do not change

• They gain electrons

Which element is an exception in Group 18 for having only two valence electrons but still being stable?

• Neon

• Argon

• Helium

• Krypton

How does chlorine achieve stability?

• By losing one electron

• By gaining one electron

• By not reacting

• By sharing electrons

What is the trend in reactivity as you move from Group 1 to Group 7 in the periodic table?

• Reactivity increases

• Reactivity fluctuates

• Reactivity decreases

• Reactivity remains constant