Elements and Atoms - AP Chemistry

The metals are found on the left side and the middle of the periodic table, and include the active metals, transition metals, and lanthanide and actinide series of elements. They easily give up electrons to form cations, since they have LOW ionization energies.

The number of neutorns is the only thing out of the answer choices that does not impact an element's atomic radius. Since neutrons have no charge, they do not impact the attractive forces between electrons and protons.

Selenium is on the right side of the periodic table, so it is not a metal or metalloid. It is not in column 7 or 8, so it is not a halogen or noble gas. Thus, it must be a nonmetal.

Electricity is produced and conducted by the movement of electrons, and thus the most important property that allows them to be used for wiring is their valence electrons that can move freely.

Hydrogen does not have enough space for 8 electrons, since it has only one s-subshell, which holds a maximum of 2 electrons.

This is the correct definition of ionization energy. By removing an electron from an atom, a cation is produced.

Rust forms when a substance is oxidized; thus iron cannot be a better oxidizing agent, because that would mean it would be more easily reduced. Aluminum and zinc are reactive, so that answer choice can be ruled out. Aluminum and zinc can form protective oxides by complexing the atom with oxygen.

Ionic bonds occur between metals and non-metals. The non-metal species are often halogens, very electronegative atoms which will completely take one of the non-metal's electrons. An ionic bond is not as much a bond as it is an association between positive and negatively charged atoms (ions). This association leads to the formation of rigid lattice structures of ionic compounds. Which makes them very stable, as seen by their high boiling points. When looking for ionic bonding, look for bonding between non-metals and metals, and atoms that are from opposite ends of the periodic table.

Atoms in the third period and above have d-orbitals that can hold up to 10 elecrons. This is what allows for atoms to exceed the octet rule.

This is the definition of gamma radiation.

In alpha decay, an element loses the equivalent of a helium nucleus, or 2 protons and 2 neutrons. Uranium-238 has an atomic number of 92 and a mass of 238 units, so the product of alpha decay will have an atomic number of 90 and a mass of 234 units. This corresponds to thorium-234.

de Broglie suggested that all matter has both wave-like and particle-like properties. His
equation states that λ= h/mv , where λ is the wavelength, m is mass, h is Planck’s constant,
and v is velocity. 4 mph is 1.8 m s−1 and Planck’s constant is 6.626e-34 kg m2 s−1 , giving
us a wavelength (λ) 4.6e-36 m ! A very small wavelength, indeed.

Rutherfords experiment focused a beam of alpha particles on a piece of gold foil. The result showed that most of the alpha particles passed through the foil, while a small fraction of particles were significantly deflected. This suggested the presence of a small, dense, positively charged nucleus. Most of the alpha particles passed through the electron clouds of the gold atoms, without impacting the nuclei, while those that did impact the nuclei were deflected by the positive charge of the nucleus.

Rutherford's experiment does not give us any concrete information about neutrons, nor does it allow us to assume that the number of protons and neutrons in the nucleus are equal.

In the Rutherford experiment, a beam of alpha particles was shot through a gold foil, with most of the particles flying straight through and a few scattering at angles greater than . These results suggest that most of the volume of foil was "empty" space, with small concentrations of positive charge, which we now know is the nucleus.

Ernest Rutherford made great advances in current understanding of atomic structure through his gold foil experiment. When firing positively-charged alpha particles at a thin film of gold atoms, most particles were found to pass straight through the film with little to no deflection, indicating that atoms were mostly composed of empty space. A few particles were deflected at large angles, indicating direct collisions with the positively charged nuclei of the atoms.

Recall that J.J. Thomson conducted the cathode ray tube experiment that proved the existence of a small negatively charged particle. Thomson was also able to determine the charge-to-mass ratio of an electron. Robert Millikan is the scientist who conducted the oil drop experiment, from which he was able to find the charge of the electron and deduce its mass using the electron's charge-to-mass ratio. Dalton was not involved in the discovery of the electron.

All the oil drops must have a charge that is a multiple of . If an oil drop is observed to have a charge of , that means the oil drop has three electrons. If an oil drop is observed to have a charge of , that means the oil drop has twelve electrons. If an oil drop is observed to have a charge of , that means the oil drop has two electrons.

B (boron) is one of the atoms known for making fewer than 4 covalent bonds, and therefore not filling its octet. C (carbon) always makes 4 bonds, while O (oxygen) and Cl (chloride) are also known for having full octets.

To find the number of electrons this oil drop contains, divide the observed charge by the charge of a single electron.

This oil drop contains electrons.

Recall that J.J. Thomson conducted the cathode ray tube experiment that proved the existence of a small negatively charged particle. Thomson was also able to determine the charge-to-mass ratio of an electron. Robert Millikan is the scientist who conducted the oil drop experiment, from which he was able to find the charge of the electron and deduce its mass using the electron's charge-to-mass ratio.