Unit 3 Target 1 & 5: Atoms, Ions, And Isotopes Quiz

When an atom gains electrons, it becomes negatively charged, forming a negative ion. This is because electrons have a negative charge, and when they are added to an atom, the overall charge of the atom becomes negative. Therefore, the correct answer is negative.

When an atom loses electrons, it becomes positively charged. This is because electrons have a negative charge, so when they are removed from an atom, the overall charge of the atom becomes positive. Therefore, the correct answer is positive.

Isotopes are atoms of the same element that have the same number of protons, but a different number of neutrons. Neutrons are subatomic particles that have no charge, and they are found in the nucleus of an atom along with protons. The number of neutrons in an atom can vary, resulting in different isotopes of the same element. This difference in the number of neutrons gives each isotope a different atomic mass. Therefore, the correct answer is that isotopes have a different number of neutrons.

The atomic mass of an atom is determined by the sum of its protons and neutrons. In this case, the atom has six protons and eight neutrons, resulting in a total of fourteen particles. Therefore, the atomic mass of the atom is fourteen atomic mass units.

Covalent bonds are formed when two atoms share electrons, resulting in a strong bond. Breaking covalent bonds requires a significant amount of energy because it involves breaking the shared electron pairs. Electrostatic bonds are formed between oppositely charged ions and are generally weaker than covalent bonds. Hydrogen bonds are relatively weak bonds that occur between a hydrogen atom and an electronegative atom. Intermolecular bonds are even weaker than hydrogen bonds and occur between molecules. Therefore, breaking covalent bonds would require the most energy compared to the other types of bonds listed.

The bond between the oxygen atom of a hydroxyl group (-OH) and a carbon atom in glycerol is best classified as a covalent bond. Covalent bonds are formed when atoms share electrons, and in this case, the oxygen atom and the carbon atom share electrons to form the bond. This type of bond is common in organic compounds like glycerol, where carbon atoms often form covalent bonds with other atoms, such as oxygen.

The particular type of element is determined by the number of protons. This is because the number of protons in an atom's nucleus defines its atomic number, which is unique to each element. The atomic number determines the element's properties and its position in the periodic table. Electrons, neutrons, valence electrons, and energy levels are all important factors in understanding an atom's behavior and reactivity, but they do not determine the element itself.

When an atom loses one or more electrons, it becomes positively charged and forms a cation. This occurs because the loss of electrons reduces the negative charge of the atom, leaving it with more protons than electrons. As a result, the atom becomes unstable and seeks to gain stability by losing electrons and forming a cation.

An ion is formed when an atom gains or loses electrons. In the process, the number of protons and electrons in the ion becomes unequal, resulting in a net positive or negative charge. On the other hand, an electrically neutral atom has an equal number of protons and electrons, meaning the charges balance out and there is no net charge. Therefore, the difference between an electrically neutral atom and an ion is that an ion has an unequal number of protons and electrons, while an atom has an equal number.

The number of neutrons varies among these carbon isotopes. Carbon-12 has 6 neutrons, carbon-13 has 7 neutrons, and carbon-14 has 8 neutrons. The number of protons and electrons remains the same in all carbon isotopes, which is 6. Photons are not subatomic particles, but rather particles of light, so they do not vary among carbon isotopes.

Isotopes are atoms of the same element that have the same number of protons but different numbers of neutrons. Since the question asks how isotopes differ from each other, the correct answer is "neutrons only" as the number of neutrons is the only characteristic that varies between isotopes.

The atomic number of an element represents the number of protons in its nucleus. Since the atomic number of lead (Pb) is 82, it means that Pb-208 has 82 protons. The atomic mass of an element is the sum of its protons and neutrons. Therefore, to find the number of neutrons in Pb-208, we subtract the atomic number from the atomic mass. Pb-208 has an atomic mass of 208, so subtracting 82 from 208 gives us 126 neutrons.

A single carbon atom can form a maximum of four covalent bonds with 1 or more hydrogen atoms. This is because carbon has four valence electrons and each hydrogen atom has one valence electron. By sharing electrons, carbon can form four bonds, one with each hydrogen atom, resulting in a stable molecule.

When a small neutral molecule becomes an ion, it is better able to function by dissolving in blood plasma. Blood plasma is a liquid component of blood that contains various ions and molecules. When a small neutral molecule becomes an ion and dissolves in blood plasma, it can easily interact with other ions and molecules present in the plasma, allowing it to participate in various biochemical reactions and physiological processes within the body. This dissolution in blood plasma enhances its ability to function effectively.