Question

Consider the stable elements through lead (Z = 82). In how many instances are the atomic weights of the elements out of order relative to the atomic numbers of the elements?

Short answer

There are $3$ instances where the atomic weights are out of order relative to the atomic numbers of the elements up to lead (Z = 82), namely: 1. Argon (Z = 18, A = 39.95) and Potassium (Z = 19, A = 39.10) 2. Cobalt (Z = 27, A = 58.93) and Nickel (Z = 28, A = 58.69) 3. Tellurium (Z = 52, A = 127.60) and Iodine (Z = 53, A = 126.90)

Step-by-step solution

Identify the elements to consider

We need to consider the elements up to lead (Z = 82). This means we will consider all the elements from hydrogen (Z = 1) to lead (Z = 82).

List the atomic weights and atomic numbers

Obtain a list of atomic weights and atomic numbers for these elements. This information can be found on a periodic table or other reliable sources.

Compare the atomic weights and atomic numbers

Go through the list and compare each element's atomic weight to the atomic weights of elements with lower atomic numbers. If the atomic weight is less than that of an element with a lower atomic number, it's considered out of order.

Count the instances

Keep track of the number of instances where the atomic weights are out of order relative to the atomic numbers. After carefully analyzing the elements up to lead (Z = 82) and comparing their atomic weights and atomic numbers, it turns out that there are $3$ instances in which the atomic weights are out of order relative to the atomic numbers of the elements: 1. Argon (Z = 18, A = 39.95) and Potassium (Z = 19, A = 39.10) 2. Cobalt (Z = 27, A = 58.93) and Nickel (Z = 28, A = 58.69) 3. Tellurium (Z = 52, A = 127.60) and Iodine (Z = 53, A = 126.90) Thus, there are $3$ instances in which the atomic weights are out of order relative to the atomic numbers.

Key concepts

The Periodic Table

The periodic table is an organized chart displaying all known chemical elements. These elements are arranged in order of increasing atomic number. This order reflects their position based on the number of protons found in an atom's nucleus. The modern periodic table helps scientists and students easily find important chemical information, such as atomic number, atomic weight, electron configuration, and common oxidation states. The layout follows a specific pattern, grouping elements with similar properties vertically in columns, known as groups or families. The horizontal rows are called periods. Each element in the same group has similar chemical and physical properties, which helps us predict their behavior in chemical reactions. The periodic table serves as a fundamental tool in chemistry, aiding in the understanding of chemical behavior and properties of elements.

Understanding Atomic Number

The atomic number of an element is a unique identifier, denoting the number of protons in an atom's nucleus. This number determines the place of an element in the periodic table and defines the element itself. For example, hydrogen has an atomic number of 1, signifying it has one proton, while helium has an atomic number of 2, meaning it has two protons.
Protons are positively charged particles, so the atomic number also indicates the positive charge of the nucleus. Since atoms are electrically neutral, the atomic number also reveals the number of electrons orbiting the nucleus. This understanding is crucial for determining an element's chemical properties and reactivity.

• Elements are ordered sequentially by atomic number on the periodic table.
• An increase in atomic number typically results in a gradual change in properties.
• Atomic number is fundamental to the element's identity and cannot change without altering the element itself.

Grasping the concept of atomic number is essential for exploring and understanding the vast array of chemical elements and their interactions.

Element Comparison and Atomic Weight

When comparing elements, one important aspect to consider is their atomic weight, sometimes called atomic mass. Atomic weight is the average mass of an atom, usually measured in atomic mass units (amu). It's calculated based on the average of isotopes for an element, taking into account their relative abundance.
Diving into element comparison involves analyzing both atomic numbers and atomic weights. Typically, elements with lower atomic numbers have lower atomic weights, but that's not always the case. As seen in the example with elements up to lead (Z = 82), there can be instances where atomic weight ordering becomes inconsistent with atomic number ordering:

• Argon and Potassium
• Cobalt and Nickel
• Tellurium and Iodine

When such anomalies occur, it is usually because of the specific isotopes that influence the average atomic weight, proving that atomic weight can sometimes appear to be out of order. Being aware of these exceptions helps in accurate recognition of element behavior and properties. Understanding element comparison ensures a deeper comprehension of the periodic table and the subtle intricacies of atomic weights.