Elements, Atoms & Ions Chapter 4 (except 4.3, 4.5)

1. Elements, Atoms & IonsChapter 4(except 4.3, 4.5)

2. 4.1 Elements Substances that cannot be decomposed into simpler substances by chemical or physical means. Each element consists of atoms having the same atomic number. Over 112 known: 88 are found in nature, rest are man-made (per your text). Abundance is the percentage found in nature Oxygen is most abundant element (by mass) in the crust of the earth and in the human body (Tables 4.1, 4.2). However, iron is the most abundant element (by mass) throughout the entire earth.

3. 4.4 Formulas Describe Compounds A compound is a distinct substance composed of atoms of two or more elements. Compounds always contain the same relative numbers of atoms of each element Compounds always contain the same relative masses of each element • 4.2 Symbols for Elements • Each element has a unique symbol • The symbol of an element may be one letter or two • If two letters, the second is lower case

4. A formula describes a compound by indicating the number and type of each atom present in the simplest unit of the compound • Examples: • Rules for writing formulas (pg 90) • each element is represented by its letter symbol • the number of atoms of each element is written to the right of the element as a subscript • When only one atom of a type is given, the subscript 1 is not written • polyatomic groups are placed in parentheses (if more than one) • Examples:

5. 4.6 The Modern Concept of Atomic Structure Atoms are the fundamental units of which elements are composed. The smallest unit of matter that retains all properties of an element. Atoms are composed of three main parts: protons, neutrons and electrons. The nucleus contains protons (+) and neutrons (0). The electrons (-) are arranged in energy levels (orbitals) outside the nucleus. In a neutral atom, # protons = # electrons

6. The number of protons in the nucleus is the atomic number (Z). • The number of protons plus neutrons in the nucleus is the mass number (A). • Electrons of different atoms interact to form bonds. Therefore, the number of electrons an atom possesses determines its chemical behavior. • Size of atom (see fig 4.9) • Diameter of nucleus ~ 10-13 cm • Diameter of overall atom ~ 10-8 cm • Diameter of an atom is about 100,000 times the diameter of the nucleus! • Atoms are mostly empty space!

7. Masses of parts of an atom Electron = 1 (relative mass) Proton = 1836 Neutron = 1839 -- most of the mass of an atom is located in the nucleus; the mass of the electrons is insignificant • In summary: • Atoms are very small, although the overall diameter of an atom is very large compared to the diameter of the atom’s nucleus. • Almost all the mass is located in the very tiny nucleus, making it very dense.

8. 4.7 Isotopes All atoms of an element have the same number of protons Atoms of an element with different numbers of neutrons are called isotopes All isotopes of an element are chemically identical and behave the same in chemical reactions Isotopes of an element have different masses Isotopes are identified by their mass numbers mass number = protons + neutrons See examples on page 96

9. 4.8 Introduction to the Periodic Table See class handout for this section. 9

10. 4.9 Natural States of the Elements • Elements are usually not found in pure form in nature (on earth). • Matter around us consists mostly of compounds and mixtures. • Most elements are reactive and form compounds with other elements. • Ex: Na + Cl  NaCl • Exceptions: the noble gases (Group 8A) and the noble metals (gold, silver, platinum). • Noble gases exist as single atoms.

11. Some gases exist as diatomic molecules at normal temperatures: (around 25o C) H2 O2 and N2 are components of air The halogens -- F2, Cl2, Br2, I2 However, hydrogen and the halogens are rarely present on earth in elemental form because they easily form compounds with other elements. Ex: Na + Cl  NaCl Mg + 2Br  MgBr2 2H2 + O2 2H2O

12. Only two elements are liquids at normal temperatures: bromine (Br2) and mercury (Hg) metal. • All other elements are solids at normal temperatures (around 25o C). (cesium and gallium melt at about 30o C)

13. Allotropes Forms of a solid nonmetallic element with different physical properties. The different physical properties arise from the different arrangements of the atoms in the solid. Allotropes of carbon include: diamond (hard) graphite (slippery) buckminsterfullerene large, soccer-ball-shaped molecules See fig 4.18 13

14. 4.10 Ions • A neutral atom has zero net charge because the number of its protons (+) equals the number of its electrons (-). • Adding or removing electrons from an atom creates an ion – an atom with a net positive or negative charge. • When one or more electrons are lost by a neutral atom, an ion with a positive charge is formed, called an cation. • Examples:

15. A cation is named using the parent name of the atom: Na+ is the sodium ion (or sodium cation) Mg2+ is the magnesium ion (or magnesium cation) • When one or more electrons are gained by a neutral atom, an ion with a negative charge is formed, called an anion. • Examples:

16. An anion is named by taking the root name of the atom and adding the suffix –ide. Cl- is the chloride ion F- is the fluoride ion O2- is the oxide ion • Ions are never formed by adding or removing protons to a nucleus. • Isolated atoms do not form ions on their own.

17. Ions form when metallic elements react with nonmetallic elements. The metal atoms lose one or more electrons, which are in turn gained by the atoms of the nonmetal.

18. Ion Charges and the Periodic Table (See fig 4.19) • Group 1A metals form 1+ ions. • Group 2A metals form 2+ ions. • Group 3A metals form 3+ ions. • Transition metals form cations with various charges. Examples: Fe2+ and Fe3+ Cu+ and Cu2+ • Group 4A metals form cations with various charges: Pb2+ and Pb4+ Sn2+ and Sn4+ • Group 5A nonmetals form 3- ions. • Group 6A nonmetals form 2- ions. • Group 7A nonmetals form 1- ions