Emission of light from an atom occurs when an electron

drops from a higher to a lower energy level.

jumps from a lower to a higher energy level.

moves within its atomic orbital.

The graph above shows the ionization energy values as the elements are arranged on the periodic table. Which conclusion cannot be drawn from the graph?

The ionization energy increases gradually as you move right across a period because the valence electrons are in a shell further from the nucleus.

The ionization energy drops significantly as you move down a group because the valence electrons are in a shell further from the nucleus.

The ionization energy increases gradually as you move right across a period because you are adding more protons.

The ionization energy increases when the valence electrons are more attracted to the nucleus.

As you move down the periodic table atoms get bigger. This is because ____________.

The atoms have more energy levels

Electronegativity is...

how good an atom is at attracting electrons

the ability of an atom to lose electrons

the energy required to remove an electron from a specific atom

how easy it is to make friends.

Atomic radius generally increases as we move __________.

down a group and from right to left across a period

up a group and from left to right across a period

down a group and from left to right across a period

up a group and from right to left across a period

Ionization energy is...

how much energy it takes to remove an electron from an atom

the energy required to add an electron to a specific atom

the energy required to shield the outer electrons from the nucleus

a measure of the ability of an atom to attract electrons

Which is larger... P or P 3- ?

P 3- due to extra electron repulsion

P 3- because it gains an energy level

P because it loses an energy level

P because of extra electron repulsion

Which is smaller... Mg or Mg 2+ ?

Mg 2+ because it loses an energy level

Mg because it gains an energy level

Mg due to extra electron repulsion

Mg 2+ because of extra electron repulsion

What can you infer about elements that are in the same group?

They will have the similar chemical properties.

They will contain the same number of protons.

They will display similar atomic masses.

They will emit X rays of similar frequency.

IB CHEMISTRY atomic structure

Authored by Matthew Neason

Chemistry

11th Grade

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MULTIPLE CHOICE QUESTION

2 mins • 1 pt

Subatomic particles with a negative charge

Electrons

Neutrons

Protons

Quarks

Tags

NGSS.HS-PS2-4

MULTIPLE CHOICE QUESTION

2 mins • 1 pt

subatomic particles found on the outermost shell & responsible for the atom's reactivity

neutrons

valence electrons

isotopes

ions

Tags

NGSS.HS-PS1-1

NGSS.HS-PS1-2

MULTIPLE CHOICE QUESTION

2 mins • 1 pt

Measure mainly of the nuclear particles: protons + neutrons

Subatomic Particles

Atomic Number

Atomic Mass

Gluons

Tags

NGSS.HS-PS1-8

MULTIPLE CHOICE QUESTION

2 mins • 1 pt

Value representing the number of protons in an element

Atomic Mass

Mass Number

Valence Electrons

Atomic Number

MULTIPLE CHOICE QUESTION

2 mins • 1 pt

Atoms of the same element with a different number of neutrons

Ion

Gluons

Isotope

Quarks

Tags

NGSS.HS-PS1-8

MULTIPLE CHOICE QUESTION

2 mins • 1 pt

A charged atom

Ion

Isotope

Electron Cloud

Quark

Tags

NGSS.HS-PS2-4

NGSS.HS-PS1-3

MULTIPLE CHOICE QUESTION

2 mins • 1 pt

Where electrons are likely to be found as they travel around the nucleus

Nucleus

Electron Cloud

Within a Proton

Within a Neutron

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IB CHEMISTRY atomic structure

Subatomic particles with a negative charge

subatomic particles found on the outermost shell & responsible for the atom's reactivity

Measure mainly of the nuclear particles: protons + neutrons

Value representing the number of protons in an element

Atoms of the same element with a different number of neutrons

A charged atom

Where electrons are likely to be found as they travel around the nucleus

Arrangement of elements organized by atomic number

Discovered the nucleus of the atom through the Gold Foil Experiment

Believed that atoms of the same element are identical to each other

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