Period 4 Elements & Atomic Structure Quiz

A proton is a subatomic particle found in the nucleus of an atom. It carries a positive charge, which is equal in magnitude but opposite in sign to the negative charge carried by an electron. This positive charge is what allows protons to attract and hold the negatively charged electrons in an atom, creating a stable structure.

Electrons are particles that have a negative charge. They are found outside the nucleus of an atom and are involved in chemical reactions and electricity. Protons, on the other hand, have a positive charge, while neutrons have no charge. Therefore, the correct answer is electron.

Neutrons are subatomic particles found in the nucleus of an atom. They do not have a charge, meaning they are electrically neutral. Unlike protons, which have a positive charge, and electrons, which have a negative charge, neutrons have no charge at all. This neutrality allows them to interact with other particles in unique ways, contributing to the stability of atomic nuclei.

The atomic number of an element represents the number of protons in the nucleus of an atom. It is a unique identifier for each element and determines its position on the periodic table. The number of protons also determines the element's chemical properties and its place in the periodic table. Therefore, the atomic number provides essential information about an atom's identity and characteristics.

Dalton's atomic theory was accepted more than Democritus's theory because Dalton's model had evidence to support it. This means that Dalton's theory was based on experimental observations and scientific evidence, which made it more credible and convincing to the scientific community. In contrast, Democritus's theory lacked the same level of experimental evidence and was more based on philosophical reasoning. Therefore, Dalton's theory was more widely accepted due to its empirical foundation.

When an atom loses or gains an electron, it undergoes ionization. Ionization refers to the process of forming an ion by adding or removing electrons from an atom. This process can result in the formation of a positively charged ion (cation) when an atom loses an electron or a negatively charged ion (anion) when an atom gains an electron. Ionization plays a crucial role in various chemical reactions and is essential for the formation of compounds.

Alkaline Earth Metals are a family of elements found in the earth's crust that have a charge of +2 when they undergo ionization. These elements include beryllium, magnesium, calcium, strontium, barium, and radium. They are called alkaline earth metals because they are less reactive than alkali metals but still have similar properties. Alkaline earth metals have two valence electrons and readily lose these electrons to form a +2 charge.

Neutrons and protons are located in the nucleus of an atom. Neutrons have no charge and are responsible for adding mass to the nucleus, while protons have a positive charge and determine the atomic number of an element. Electrons, on the other hand, are located in the electron cloud surrounding the nucleus. Megatrons, on the other hand, are not subatomic particles and do not exist in the context of atomic structure.

The electron is by far the smallest particle among the given options. Protons and neutrons are both subatomic particles found in the nucleus of an atom, while electrons orbit around the nucleus. Electrons have a much smaller mass compared to protons and neutrons, making them significantly smaller in size.

True, the Periodic Law is a fundamental principle in chemistry that states that the properties of elements are periodic functions of their atomic numbers. This means that as the number of protons in an atom increases, there is a regular repetition of chemical and physical properties. This pattern is observed in the periodic table, where elements are arranged in order of increasing atomic number. Therefore, the statement that the Periodic Law states that when atoms are arranged by the number of protons they show a pattern of chemical and physical properties is true.

Atoms go through ionization to get a full outer shell of electrons. Ionization occurs when an atom gains or loses electrons, resulting in the formation of ions. This process helps atoms achieve a stable electron configuration similar to that of noble gasses, which have a full outer shell. Therefore, the statement is true.

When an atom gains an electron, it has an overall negative charge because the number of electrons is now greater than the number of protons. This type of atom is called an anion.

Alkali metals are highly reactive with water because they have only 1 valence electron. This electron is easily lost, resulting in the formation of a positive ion. The reactivity of alkali metals increases as you move down the periodic table because the outermost electron is further away from the positively charged nucleus, making it easier to remove. This reactivity with water is evident in their vigorous reaction, often producing hydrogen gas and forming alkaline solutions.

The S orbitals can hold a maximum of 2 electrons. This is because the S orbital is the first energy level and has only one subshell, which can accommodate a maximum of 2 electrons according to the Pauli exclusion principle.

An atom of helium has a full outer shell of only 2 electrons, not 8. Helium is in the first period of the periodic table and its electron configuration is 1s2, meaning it has 2 electrons in its outermost shell.

Radon is a chemical element with the atomic number 86, which indicates the number of protons in its nucleus. In a neutral atom, the number of electrons is equal to the number of protons, so there are 86 electrons in one neutral atom of Radon.

Noble gasses have a full outer shell of electrons, meaning they have achieved a stable electron configuration. This makes them highly stable and unreactive with other elements. Due to their full outer shells, noble gasses do not readily gain, lose, or share electrons with other elements, making them chemically inert. This characteristic of noble gasses explains why they do not react with any other element.

As you move from left to right across a period in the periodic table, metallic character decreases due to increasing electronegativity and ionization energy. Non-metals are found to the right of the periodic table, while metals are found to the left.

Dalton's atomic model, proposed in the early 19th century, described atoms as indivisible and indestructible particles. According to his model, atoms were the basic building blocks of matter and did not contain any subatomic particles such as protons, neutrons, or electrons. Therefore, the given image cannot be an accurate depiction of Dalton's atomic model as it shows subatomic particles, which were not included in his model.

When an atom loses an electron, it has an overall positive charge because it now has more protons than electrons. This positively charged atom is called a cation.

Radon has a lower ionization energy compared to Neon. Ionization energy is the energy required to remove an electron from an atom. Radon, being a larger atom with more electron shells, has a higher shielding effect and weaker attraction between the protons and the outermost electrons. This makes it easier to remove an electron from Radon, resulting in a lower ionization energy compared to Neon.

Radon is a chemical element with atomic number 86. The atomic number represents the number of protons in the nucleus of an atom. Since the element is neutral, the number of protons is equal to the number of electrons. The atomic mass of Radon is 222, which represents the sum of protons and neutrons in the nucleus. To find the number of neutrons, we subtract the atomic number from the atomic mass: 222 - 86 = 136. Therefore, there are 136 neutrons in one neutral atom of Radon.

Halogens are a family of elements that often form anions and are highly reactive with alkali metals to achieve a full outer shell. This is because halogens only need one more electron to complete their outer shell, and they can easily gain this electron by accepting it from alkali metals. This reaction allows both the halogens and alkali metals to achieve a more stable electron configuration, making halogens highly reactive with alkali metals.

An isotope is when an atom has the same number of protons but a different number of neutrons, not electrons. Isotopes have the same atomic number (number of protons) but different mass numbers (number of protons + neutrons). Therefore, the statement that an isotope is when an atom has the same number of protons but a different number of electrons is false.

According to Bohr's model of the atom, the 3rd energy level can hold a maximum of 18 electrons, not 8. This is because the 3rd energy level has 3 sublevels (s, p, and d), each with different orbital shapes and capacities. The s sublevel can hold a maximum of 2 electrons, the p sublevel can hold a maximum of 6 electrons, and the d sublevel can hold a maximum of 10 electrons. Therefore, the total capacity of the 3rd energy level is 2 + 6 + 10 = 18 electrons.

The bottom left corner of the periodic table corresponds to the elements in the alkali metals and alkaline earth metals groups. These elements have the highest atomic radius because they have the highest number of energy levels and the fewest protons in the nucleus. As you move down a group in the periodic table, the atomic radius increases because there are more energy levels, which leads to a larger atomic size.

Bohr's Model is the correct answer because it is based on the concept of electrons orbiting the nucleus in specific energy levels, much like planets orbiting the sun. This model was proposed by Niels Bohr in 1913 and it played a significant role in understanding the behavior of electrons in atoms. According to Bohr's Model, electrons occupy discrete energy levels and can jump between them by absorbing or emitting energy. This model successfully explained the stability of atoms and the emission and absorption spectra observed in experiments.

The average atomic mass of an element is calculated by taking the weighted average of the masses of its isotopes, where the weights are the relative abundance of each isotope. In this case, the given answer 20.187 is likely the result of calculating the average atomic mass of Neon using the masses of its three isotopes (20.085, 21.01, and 22.00) and their respective abundances. However, without the specific abundances of each isotope, it is not possible to provide a more detailed explanation.