Inv6.Exp1 Text B

1. According to Rutherford's discovery, what percentage of an atom's mass is concentrated in its nucleus?

• More than 90%
• Less than 90%
• More than 99%
• Less than 50%

2. What was the main issue that Bohr's model addressed regarding Rutherford's atomic model?

• The size of the nucleus
• The mass of protons
• Why electrons don't fall into the nucleus
• The location of neutrons

3. In modern atomic theory, electrons are viewed as:

• Stationary particles
• Waves of probable positions
• Fixed orbital particles
• Nucleus components

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4. What determines the atomic radius of an element?

• Only the number of protons
• Only the number of electrons
• The distance from nucleus to outermost electrons
• The total mass of the atom

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NGSS.HS-PS1-1

5. How does nuclear charge affect atomic radius?

• Stronger charge increases radius
• Stronger charge decreases radius
• Nuclear charge has no effect on radius
• Nuclear charge only affects electron count

6. What happens to atomic radius as you move down the periodic table?

• It increases due to new electron shells
• It decreases due to nuclear charge
• It remains constant
• It fluctuates randomly

7. Electronegativity is primarily determined by:

• Number of neutrons
• Atomic mass
• Nuclear attractive force on electrons
• Number of electron shells

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NGSS.HS-PS1-1

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8. What causes atomic volume to decrease across a period?

• Decreasing nuclear charge
• Fewer electrons
• Stronger nuclear attraction
• Weaker electron bonds

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NGSS.HS-PS1-1

9. The modern view of electron behavior differs from early models by describing electrons as:

• Fixed particles in specific locations
• Randomly moving particles
• Probability waves in orbitals
• Static charges around the nucleus

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NGSS.HS-PS4-1

10. What property of atoms remains identical across all elements?

• Nuclear size
• Electron characteristics
• Atomic mass
• Number of neutrons