Problem 2
Question
Predict the formula of the compound that forms between phosphorus ( \(\mathrm{P}\) ) and hydrogen.
Step-by-Step Solution
Verified Answer
The formula of the compound that forms between phosphorus and hydrogen is \(\mathrm{PH}_{3}\).
1Step 1: Determine the valence of phosphorus
From the periodic table, we know that phosphorus (P) is in group 15. This means that it has 5 valence electrons. As a result, phosphorus needs to gain or lose 3 electrons to reach a stable electron configuration.
2Step 2: Determine the valence of hydrogen
Hydrogen (H) is in group 1 of the periodic table, which means it has 1 valence electron. Hydrogen typically needs to lose or gain 1 electron to reach a stable configuration.
3Step 3: Combine phosphorus and hydrogen to form a neutral compound
Because phosphorus needs to gain or lose 3 electrons and hydrogen needs to lose or gain 1 electron, we can predict that the compound will be a combination of one phosphorus atom and three hydrogen atoms. This means that the formula for the compound that forms between phosphorus and hydrogen is \(\mathrm{PH}_{3}\).
Key Concepts
Understanding Valence ElectronsDeciphering the Periodic TableElectron Configuration and StabilityPhosphorus and Hydrogen Compound
Understanding Valence Electrons
To comprehend how chemicals bond, it's essential to grasp the concept of valence electrons. These are the electrons located in the outermost shell of an atom and are critical in forming chemical bonds. Hydrogen, with its sole electron, and phosphorus, with five in its outer shell, must adhere to the octet rule, striving for a full set of eight valence electrons, akin to the noble gases.
For phosphorus, this means it can either gain three electrons or share three to achieve stability. Meanwhile, hydrogen, with just one valence electron, can either lose it or share it to reach a stable configuration. In sharing electrons, these elements can form compounds, fulfilling the octet rule through covalent bonding. This concept is fundamental to predicting the formula for compounds formed between elements like phosphorus and hydrogen.
For phosphorus, this means it can either gain three electrons or share three to achieve stability. Meanwhile, hydrogen, with just one valence electron, can either lose it or share it to reach a stable configuration. In sharing electrons, these elements can form compounds, fulfilling the octet rule through covalent bonding. This concept is fundamental to predicting the formula for compounds formed between elements like phosphorus and hydrogen.
Deciphering the Periodic Table
The periodic table is akin to a map, guiding us through the landscape of elements. Each element is placed in a specific group and period, which indicates its physical and chemical properties. For instance, phosphorus is situated in group 15, reflecting its five valence electrons. Group numbers can hint at the number of valence electrons for main-group elements—those in groups 1 through 2 and 13 through 18.
Understanding an element's location on the periodic table is vital for predicting how it might interact with others. Hydrogen, though a non-metal, is listed in group 1, which usually contains metals. This placement signifies that hydrogen, like its group mates, has one valence electron and is ready to bond with other elements. By mastering the layout and logic of the periodic table, you can deduce much about an element's reactive nature.
Understanding an element's location on the periodic table is vital for predicting how it might interact with others. Hydrogen, though a non-metal, is listed in group 1, which usually contains metals. This placement signifies that hydrogen, like its group mates, has one valence electron and is ready to bond with other elements. By mastering the layout and logic of the periodic table, you can deduce much about an element's reactive nature.
Electron Configuration and Stability
Electron configuration is the arrangement of electrons around the nucleus of an atom. Valence electrons play a starring role in bonding, and their configuration is crucial in determining how an element will bond with others. Each electron shell holds a maximum number of electrons: the first shell holds 2, the second holds 8, and so on.
Elements aim for the most stable electron configuration, often seeking to mirror the electron configuration of the nearest noble gas—the epitome of stability. Phosphorus, for instance, seeks to complete its third shell with eight electrons. It can either do so by gaining three electrons or by sharing them with other elements, like hydrogen, which itself seeks to either lose its single electron or share it. Through understanding electron configuration, the rationale behind the bonding in compounds such as phosphorus and hydrogen becomes quite lucid.
Elements aim for the most stable electron configuration, often seeking to mirror the electron configuration of the nearest noble gas—the epitome of stability. Phosphorus, for instance, seeks to complete its third shell with eight electrons. It can either do so by gaining three electrons or by sharing them with other elements, like hydrogen, which itself seeks to either lose its single electron or share it. Through understanding electron configuration, the rationale behind the bonding in compounds such as phosphorus and hydrogen becomes quite lucid.
Phosphorus and Hydrogen Compound
The compound that phosphorus (P) forms with hydrogen (H) is underpinned by the principles previously mentioned. Phosphorus has five valence electrons and needs three more for stabilization, while each hydrogen possesses one valence electron and requires another for its full duet. Therefore, three hydrogen atoms can share their electrons with one phosphorus atom, leading to a mutually beneficial arrangement.
The resultant compound is phosphine, with the chemical formula \(\mathrm{PH}_{3}\). In this covalent molecule, three hydrogen atoms are bonded to a phosphorus atom, completing the phosphorus shell and satisfying hydrogen's need for two electrons. This example showcases how elements use their valence electrons and principles of stability to form compounds, a fundamental concept that is utilized to predict and understand the myriad substances that make up our world.
The resultant compound is phosphine, with the chemical formula \(\mathrm{PH}_{3}\). In this covalent molecule, three hydrogen atoms are bonded to a phosphorus atom, completing the phosphorus shell and satisfying hydrogen's need for two electrons. This example showcases how elements use their valence electrons and principles of stability to form compounds, a fundamental concept that is utilized to predict and understand the myriad substances that make up our world.
Other exercises in this chapter
Problem 1
Predict the formula of the compound that forms between carbon and chlorine.
View solution Problem 3
Predict the formula of the compound that forms between silicon (Si) and bromine (Br).
View solution Problem 4
In forming molecules, atoms can share unpaired electrons in order to achieve an octet in their valence shell. Hydrogen is an exception. What number of electrons
View solution Problem 5
What is the molecular formula of the compound that forms between \(\mathrm{H}\) atoms and \(\mathrm{F}\) atoms? Justify your answer with dot diagrams.
View solution