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PERIODIC TABLE 15.1

PERIODIC TABLE 15.1. Chapter Fifteen: Elements and the Periodic Table. 15.1 The Periodic Table of the Elements 15.2 Properties of the Elements. Chapter 15.1 Learning Goals. Differentiate physical and chemical properties of elements. Explain how the periodic table is organized.

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PERIODIC TABLE 15.1

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  1. PERIODIC TABLE 15.1

  2. Chapter Fifteen: Elements andthe Periodic Table • 15.1 The Periodic Table of the Elements • 15.2 Properties of the Elements

  3. Chapter 15.1 Learning Goals • Differentiate physical and chemical properties of elements. • Explain how the periodic table is organized. • Identify metals, semimetals, and nonmetals on the periodic table.

  4. Key Question: How is the periodic table organized? Investigation 15A The Periodic Table

  5. 15.1 Physical properties • Characteristics that you can see through direct observation are called physical properties. • Physical properties include color, texture, density, brittleness, and state (solid, liquid, or gas). • Melting point, boiling point, and specific heat are also physical properties.

  6. 15.1 Physical properties • A physical change does not result in a new substance being formed.

  7. 15.1 Chemical properties • Properties that can only be observed when one substance changes into a different substance are called chemical properties. • Any change that transforms one substance into a different substance is called a chemical change.

  8. 15.1 The Periodic Table • The periodic table organizes the elements according to how they combine with other elements (chemical properties). • The periodic table is organized in order of increasing atomic number.

  9. 15.1 The Periodic Table • The periodic table is further divided into periods and groups. • Each horizontal row is called a period. • Each vertical column is called a group.

  10. 15.1 The Periodic Table • All the elements in Group 1 of the periodic table form similar compounds. • The metals lithium, sodium, and potassium all form compounds with a ratio of 2 atoms of the metal to 1 atom of oxygen.

  11. 15.1 Atomic Mass • The mass of individual atoms is so small that the numbers are difficult to work with. • To make calculations easier, scientists use the atomic mass unit (amu). • The atomic mass of any element is the average mass (in amu) of an atom of each element.

  12. 15.1 Atomic Mass • Atomic masses differ from mass numbers because most elements in nature contain more than one isotope.

  13. 15.1 Atomic Number • Remember, the atomic number is the number of protons all atoms of that element have in their nuclei. • If the atom is neutral, it will have the same number of electrons as protons.

  14. 15.1 Groups of the periodic table • The first group is known as the alkali metals. • The alkali metals are soft and silvery in their pure form and are highly reactive. • This group includes the elements lithium (Li), sodium (Na), and potassium (K).

  15. 15.1 Groups of the periodic table • The group two metals include beryllium (Be), magnesium (Mg), and calcium (Ca). • They also bond easily with oxygen.

  16. 15.1 Halogens • The halogens tend to be toxic gases or liquids in their pure form. • Fluorine (F), chlorine (Cl), and bromine (Br) form salts when the bond with alkali metals.

  17. 15.1 Noble Gases • The noble gases, including the elements helium (He), neon (Ne), and argon (Ar). • These elements do not naturally form chemical bonds with other atoms and are almost always found in their pure state.

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