Transcript Chapter 4

Elements, Atoms & Ions

Chapter 4


• • • •


Over 112 known, of which 88 are found in nature – others are man-made Abundance is the percentage found in nature – oxygen most abundant element (by mass) on earth and in the human body – the abundance and form of an element varies in different parts of the environment 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 2

Table 4.1: Distribution (Mass Percent) of the 18 Most Abundant Elements in the Earth's Crust, Oceans, and Atmosphere 3

Table 4.2: Abundance of elements in the human body


Dalton’s Atomic Theory

   Elements are composed of atoms – tiny, hard, unbreakable, spheres All atoms of a given element are identical – all carbon atoms have the same chemical and physical properties Atoms of a given element are different from those of any other element – carbon atoms have different chemical and physical properties than sulfur atoms 5

Dalton’s Atomic Theory

 Atoms of one element combine with atoms of other elements to form compounds. – Law of Constant Composition • all samples of a compound contain the same proportions (by mass) of the elements – Chemical Formulas 6

Dalton’s Atomic Theory

 Atoms are indivisible in a chemical process.

– all atoms present at beginning are present at the end – atoms are not created or destroyed, just rearranged – atoms of one element cannot change into atoms of another element • cannot turn Lead into Gold by a chemical reaction 7

Formulas Describe Compounds

• • • • • a compound is a distinct substance that is composed of atoms of two or more elements describe the compound by describing the number and type of each atom in the simplest unit of the compound – molecules or ions each element represented by its letter symbol the number of atoms of each element is written to the right of the element as a subscript – if there is only one atom, the 1 subscript is not written polyatomic groups are placed in parentheses – if more than one 8

Figure 4.2: Dalton pictured compounds as collections of atmosphere NO, NO 2 , and N 2 O are represented 9

Are Atoms Really Unbreakable?

• • • • • • J.J. Thomson investigated a beam called a

cathode ray

he determined that the ray was made of tiny negatively charged particles we call


his measurements led him to conclude that these electrons were smaller than a hydrogen atom if electrons are smaller than atoms, they must be pieces of atoms if atoms have pieces, they must be breakable Thomson also found that atoms of different elements all produced these same electrons 10

The Electron • •

Tiny, negatively charged particle Very light compared to mass of atom – 1/1836 th the mass of a H atom

Move very rapidly within the atom 11

Rutherford’s Results • • •

Over 98% of the  About 2% of the  particles went straight through particles went through but were deflected by large angles About 0.01% of the  particles bounced off the gold foil 12

Figure 4.6: (a) The results that the metal foil experiment would have yielded if the plum pudding model had been correct; (b) Actual results 13

Rutherford’s Nuclear Model

    The atom contains a tiny dense center called the


– the volume is about 1/10 trillionth the volume of the atom The nucleus is essentially the entire mass of the atom The nucleus is positively charged – the amount of positive charge of the nucleus balances the negative charge of the electrons The electrons move around in the empty space of the atom surrounding the nucleus 14

Figure 4.9: A nuclear atom viewed in cross section 15

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Structure of the Nucleus

The nucleus was found to be composed of two kinds of particles Some of these particles are called


– – charge = +1 mass is about the same as a hydrogen atom Since protons and electrons have the same amount of charge, for the atom to be neutral there must be equal numbers of protons and electrons The other particle is called a


– has no charge – has a mass slightly more than a proton 16

The Modern Atom • • • •

We know atoms are composed of three main pieces - protons, neutrons and electrons The nucleus contains protons and neutrons The nucleus is only about 10 -13 average distance of about 10 -8 cm in diameter The electrons move outside the nucleus with an cm – therefore the radius of the atom is about 10 5 times larger than the radius of the nucleus 17

• • • • • •


All atoms of an element have the same number of protons The number of protons in an atom of a given element is the same as the

atomic number

– found on the Periodic Table Atoms of an element with different numbers of neutrons are called


All isotopes of an element are chemically identical – undergo the exact same chemical reactions Isotopes of an element have different masses Isotopes are identified by their

mass numbers

– mass number = protons + neutrons 18

Figure 4.10: Two isotopes of sodium


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Arranged in a pattern called the Periodic Table Position on the table allows us to predict properties of the element Metals – about 75% of all the elements – lustrous, malleable, ductile, conduct heat and electricity Nonmetals – dull, brittle, insulators Metalloids – also know as semi-metals – some properties of both metals & nonmetals 20

The Modern Periodic Table • • • •

Elements with similar chemical and physical properties are in the same column Columns are called Rows are called

Groups Periods



Each period shows the pattern of properties repeated in the next period 21

Figure 4.11: The periodic table


The Modern Periodic Table • • •

Main Group = Representative Elements – “A” columns Transition Elements – all metals Bottom rows = Inner Transition Elements = Rare Earth Elements – – metals really belong in Period 6 & 7 23

Important Groups

• • • • • Group 8 = Noble Gases He, Ne, Ar, Kr, Xe, Rn all colorless gases at room temperature very non-reactive, practically inert found in nature as a collection of separate atoms uncombined with other atoms • • • • • Noble Metals Ag, Au, Pt all solids at room temperature least reactive metals found in nature uncombined with other atoms 24

Important Groups - Halogens

• • • • Group 7A = Halogens very reactive nonmetals react with metals to form ionic compounds HX all acids • • • • Fluorine = F 2 – pale yellow gas Chlorine = Cl 2 – pale green gas Bromine = Br 2 – brown liquid that has lots of brown vapor over it – Only other liquid element at room conditions is the metal Hg Iodine = I 2 – lustrous, purple solid 25

Allotropes • • •

Many solid nonmetallic elements can exist in different forms with different physical properties, these are called


the different physical properties arise from the different arrangements of the atoms in the solid Allotropes of Carbon include – diamond – – graphite buckminsterfullerene 26

Figure 4.18a: The three solid elemental (allotropes) forms of carbon 27

Figure 4.18b: The three solid elemental (allotropes) forms of carbon 28

Figure 4.18c: The three solid elemental (allotropes) forms of carbon 29

Electrical Nature of Matter

• • • Most common pure substances are very poor conductors of electricity – with the exception of metals and graphite – Water is a very poor electrical conductor Some substances dissolve in water to form a solution that conducts well - these are called


When dissolved in water, electrolyte compounds break up into component


– ions are atoms or groups of atoms that have an electrical charge 30

Figure 4.20: (a) Pure water does not conduct a current; (b) Water containing a dissolved salt conducts electricity 31

• • • • • Ions

ions that have a positive charge are called


– form when an atom loses electrons ions that have a negative charge are called


– form when an atom gains electrons ions with opposite charges attract – therefore cations and anions attract each other moving ions conduct electricity compound must have no total charge, therefore we must balance the numbers of cations and anions in a compound to get 0 total charge 32

Figure 4.21a: The arrangement of sodium ions (Na + ) and chloride ions (Cl ) in the ionic compound sodium chloride.


Figure 4.21b: Solid sodium chloride highly magnified.


Atomic Structures of Ions

• • • • Metals form cations For each positive charge the ion has 1 less electron than the neutral atom – Na = 11 e , Na + = 10 e – Ca = 20 e , Ca +2 = 18 e Cations are named the same as the metal sodium calcium Na  Ca  Na Ca + +2 + 1e + 2e sodium ion calcium ion The charge on a cation can be determined from the Group number on the Periodic Table for Groups IA, IIA, IIIA – Group 1A  +1, Group 2A  +2, (Al, Ga, In)  +3 35

• • • •

Atomic Structures of Ions

Nonmetals form anions For each negative charge the ion has 1 more electron than the neutral atom – F = 9 e , F = 10 e – P = 15 e , P 3 = 18 e Anions are named by changing the ending of the name to


fluorine oxygen F + 1e O + 2e   F fluoride ion O 2 oxide ion The charge on an anion can be determined from the Group number on the Periodic Table – Group 7A  -1, Group 6A  -2 36