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Chapter 13: Problem 2

State the number of valence electrons for a hydrogen atom and a bromine atom.

Short Answer

Expert verified
Hydrogen has 1 valence electron; bromine has 7 valence electrons.

Step by step solution

01

Understanding Valence Electrons

The valence electrons are the electrons in the outermost energy level of an atom. These electrons are important for chemical bonding as they participate in forming chemical bonds.
02

Determine Valence Electrons for Hydrogen

Hydrogen has an atomic number of 1, which means it has 1 electron in total. Since it only has one energy level (the first energy shell), this 1 electron is its valence electron.
03

Determine Valence Electrons for Bromine

Bromine has an atomic number of 35, meaning it possesses 35 electrons. Its electron configuration is \([Ar]\, 3d^{10}\, 4s^2\, 4p^5\). The electrons in the highest energy level are 4s^2 and 4p^5, totaling 7 valence electrons.

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Key Concepts

These are the key concepts you need to understand to accurately answer the question.

Chemical Bonding
Chemical bonding is a fundamental concept where atoms combine to form molecules. At the heart of chemical bonding are the valence electrons. These are the electrons located in the outermost shell of an atom. When atoms interact, they seek stability, often achieved by having a full valence shell. This shell is usually filled with either 2 or 8 electrons.
  • Covalent bonds form when atoms share pairs of valence electrons to achieve a filled outer shell.
  • Ionic bonds arise when one atom donates an electron to another, creating a positive and a negative ion which attract each other.
These interactions allow atoms to achieve more stable electron configurations, generally resembling those of noble gases, which are naturally stable and inert. Understanding chemical bonding is crucial as it explains how different substances form and determine the properties of the resulting compounds.
Electron Configuration
Electron configuration describes the arrangement of electrons around the nucleus of an atom. It provides a map of how electrons fill the different energy levels or orbitals. These configurations obey the principles like Pauli Exclusion Principle and Hund's Rule which dictate how orbitals are filled.
  • Electrons occupy orbitals in a specific order, filling the lowest energy levels first (known as Aufbau principle).
  • This order is typically: 1s, 2s, 2p, 3s, 3p, 4s, 3d, 4p, etc., following specific pattern of increasing energy.
For example, hydrogen, with an atomic number of 1, has the simplest electron configuration: 1s1. The more complex an atom, like bromine, has a detailed configuration such as \([Ar] \, 3d^{10} \, 4s^2 \, 4p^5 \), showing how its 35 electrons are distributed.
Atomic Number
The atomic number of an element is a critical property in determining its identity and position in the periodic table. This number corresponds to the number of protons in an atom's nucleus and, in a neutral atom, also equals the number of electrons surrounding the nucleus.
  • Atomic number is denoted with the symbol 'Z'.
  • It is a fundamental characteristic that defines the type of element. For example, hydrogen has an atomic number of 1, making it the simplest element.
  • Bromine, on the other hand, has an atomic number of 35, placing it much further down the periodic table.
Knowing the atomic number allows scientists to determine the electron configuration and predict an element's chemical behavior. This highlights the atomic number's significant role in both periodic trends and chemical reactivity.

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