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Properties and trends across periods and down groups in the periodic table.
The periodic table is a tabular display of the known chemical elements, organized by their atomic number (number of protons in an atom), electron configuration, and recurring chemical properties.
The atomic number of an element is the number of protons in its atomic nucleus, which determines the identity of the element. The electron configuration of an atom is the arrangement of electrons in its energy levels. As you move across a period, the number of electrons increases by one for each successive element, resulting in an increase in the number of valence electrons. This leads to changes in chemical reactivity and physical properties.
As you move across a period, the atomic radius decreases due to the increasing positive charge on the nucleus. The ionization energy also increases as the number of protons in the nucleus increases. Additionally, the electronegativity of elements generally increases as you move from left to right across a period.
Elements in the same group have similar chemical properties due to the same number of valence electrons. As you move down a group, the atomic radius increases and the ionization energy decreases. This leads to changes in reactivity, with elements at the bottom of a group being more reactive than those at the top.
Metals are typically shiny, malleable, and good conductors of electricity. They tend to lose electrons to form ions. Nonmetals are dull, brittle, and poor conductors of electricity. They tend to gain electrons to form ions. Metalloids exhibit intermediate properties.
The periodic table is divided into four blocks: s-block, p-block, d-block, and f-block. The s-block contains the first two columns (alkali metals and alkaline earth metals), while the p-block includes the remaining elements in groups 13-18.
The periodic table is also organized into families based on chemical properties, such as alkali metals, alkaline earth metals, halogens, and noble gases. These families exhibit similar chemical reactivity due to their shared electron configurations.
The periodic table provides a framework for understanding the relationships between elements and their chemical properties. By examining the positions of elements in the periodic table, chemists can predict the types of bonds that will form between atoms and the physical and chemical properties of compounds.
What is the primary way elements are organized in the periodic table?
Which of the following statements about groups in the periodic table is true?
What is the term for a vertical column of elements in the periodic table that exhibit similar chemical properties?
As you move across a period, what happens to the atomic radius?
Which of the following is NOT a characteristic of metals in the periodic table?
What is the term for a horizontal row of elements in the periodic table that exhibit similar chemical properties?
Which of the following statements about the periodic table is true?
What is the term for a tabular display of the known chemical elements, organized by their atomic number, electron configuration, and recurring chemical properties?
As you move down a group, what happens to the atomic radius?
Describe the relationship between elements in the same group. (2 marks)
Explain how the periodic table can be used to predict the chemical reactivity of an element. (3 marks)
Compare and contrast metals and nonmetals. (3 marks)
Describe the relationship between elements in the same period. (2 marks)
Explain how the periodic table is organized into blocks and families. (3 marks)
Discuss the importance of understanding the periodic table in chemistry. (20 marks)
Describe how the periodic table can be used to predict the chemical reactivity of an element and explain why this is important in chemistry. (20 marks)