Chemistry Exam Type Terms Flashcards
What are the three subatomic particles in an atom?
Protons, Neutrons, and Electrons.
Where are protons, neutrons, and electrons located?
Protons and neutrons are in the nucleus; electrons orbit in energy levels.
What is the charge of each subatomic particle?
Proton (+1), Neutron (0), Electron (-1).
What is an ion?
An atom or molecule that has gained or lost electrons, giving it a charge.
What is a cation?
A positively charged ion that has lost electrons (e.g., Na⁺).
What is an anion?
A negatively charged ion that has gained electrons (e.g., Cl⁻).
How do you determine the charge of an ion?
By comparing the number of protons and electrons. More protons = positive charge, more electrons = negative charge.
What do absorption and emission spectra tell us about elements?
They show the specific wavelengths of light absorbed or emitted when electrons transition between energy levels. Used to identify elements.
What happens when an electron moves from a higher energy level to a lower one?
Energy is released as a photon, producing an emission spectrum.
What happens when an electron absorbs energy?
It moves to a higher energy level, creating an absorption spectrum.
How is effective nuclear charge (Zeff) calculated?
Zeff = Protons - Core Electrons (Shielding Effect)
Why does Zeff increase across a period?
More protons increase nuclear attraction, while shielding remains constant.
What happens to atomic radius across a period?
Decreases due to increased nuclear charge pulling electrons closer.
What happens to ionization energy across a period?
Increases because more energy is required to remove an electron.
What happens to electronegativity across a period?
Increases as atoms attract electrons more strongly.
Why is Na+ smaller than Na?
Losing an electron removes an energy level, reducing size.
Why is Cl- larger than Cl?
Gaining an electron increases electron repulsion, expanding the electron cloud.
Which element has the highest electronegativity?
Fluorine (F), due to its small size and high Zeff.
What happens to electronegativity down a group?
Decreases as atomic size increases and nuclear attraction weakens.
Define first ionization energy.
The energy required to remove one electron from a neutral atom.
Why does ionization energy decrease down a group?
Outer electrons are further from the nucleus, experiencing less attraction.
What is ionic bonding?
Transfer of electrons from a metal to a non-metal, forming oppositely charged ions.
