The isotope of an unknown element, X, has a mass number of 79 . The most stable ion of the isoto

step 1 So we're looking at the isotope of unknown element X, which has a mass of 79. And the most stabl

The isotope of an unknown element, X, has a mass number of...

The isotope of an unknown element, $\mathrm{X}$, has a mass number of $79 .$ The most stable ion of the isotope has 36 electrons and forms a binary compound with sodium having a formula of $\mathrm{Na}_{2} \mathrm{X}$. Which of the following statements is(are) true? For the false statements, correct them. a. The binary compound formed between $\mathrm{X}$ and fluorine will be a covalent compound. b. The isotope of $\mathrm{X}$ contains 38 protons. c. The isotope of $\mathrm{X}$ contains 41 neutrons. d. The identity of $X$ is strontium, Sr.

The isotope of an unknown element, $\mathrm{X}$, has a mass number of $79 .$ The most stable ion of the isotope has 36 electrons and forms a binary compound with sodium having a formula of $\mathrm{Na}_{2} \mathrm{X}$. Which of the following statements is(are) true? For the false statements, correct them.
a. The binary compound formed between $\mathrm{X}$ and fluorine will be a covalent compound.
b. The isotope of $\mathrm{X}$ contains 38 protons.
c. The isotope of $\mathrm{X}$ contains 41 neutrons.
d. The identity of $X$ is strontium, Sr.

Key Concepts

Ionic versus Covalent Bonding

This key concept distinguishes between ionic and covalent bonds. Ionic compounds form when there is a significant electronegativity difference between elements, typically between metals and nonmetals, resulting in the complete transfer of electrons. In contrast, covalent compounds form between nonmetals with similar electronegativities, where electrons are shared rather than transferred. Understanding these bonding types helps in predicting the nature of the compound formed between two elements.

Periodic Trends and Group Characteristics

Periodic trends refer to the recurring properties of elements when arranged in the periodic table. Elements in the same group often exhibit similar chemical behaviors and common oxidation states. Recognizing these group characteristics aids in predicting the types of ions they form and their bonding behavior in compounds. This understanding can be crucial when identifying an element based on its chemical and ionic characteristics as deduced from compound formulas.

Atomic Structure and Isotopes

This concept involves understanding that every atom is defined by its number of protons (the atomic number) and that the mass number is the sum of protons and neutrons. Isotopes are variants of the same element that have the same number of protons but differ in the number of neutrons, which leads to different mass numbers. This understanding is essential when deducing information about an unknown isotope from its mass number and electron balance.

Ion Formation and Electron Count

Ion formation involves either the loss or gain of electrons relative to the neutral atom in order to achieve a more stable electron configuration. When an atom forms an ion, the difference between the number of electrons in the ion and the neutral atom indicates its charge. For example, if the most stable ion has more electrons than the neutral atom, it is an anion, and the electron count can be used to determine the original atomic number.

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