SIZING UP THE ATOM. Atoms are now known to be divisible!

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1 SIZING UP THE ATOM Atoms are now known to be divisible!

2 Chapter 4 Atomic Structure 4.1 Defining the Atom 4.2 Structure of the Nuclear Atom 4.3 Distinguishing Among Atoms

3 SUBATOMIC PARTICLES Subatomic particles are the most fundamental parts in an atom ØProtons: positively charged particles in the nucleus ØNeutrons: neutral particles in the nucleus ØElectrons: negatively charged & negligible mass (~1,800 times smaller than a proton or neutron) Discovered by J.J. Thomson using the cathode ray experiment ØQuarks: subnuclear particles that make up protons & neutrons

4 CATHODE RAY EXPERIMENT BY J.J. THOMSON

5 CATHODE RAY EXPERIMENT BY J.J. THOMSON Electrons must be negatively charged!

6 SUBATOMIC PARTICLES: ELECTRONS Discovered in 1897 by JJ Thomson using cathode-ray tube ØDeveloped the plum-pudding model of an atom ØFound charge-to-mass ratio to be constant and independent of type of gas used ØConcluded that electrons are a component of the atoms of all elements Charge and mass quantified by Millikan using oil-drop experiment

7 SUBATOMIC PARTICLES

8 RUTHERFORD S EXPERIMENT Determined that an atom is mostly empty space, in contrast to the plum-pudding model Positive charge must be concentrated, called this the nucleus NUCLEUS is the tiny central core of an atom, composed of protons and neutrons

9 THE NUCLEAR ATOM Rutherford s atomic model is known as the nuclear atom Protons and neutrons are located in the positively-charged nucleus Electrons are distributed around the nucleus and occupy almost all the volume of the atom If an atom were the size of a football stadium, the nucleus would be the size of a marble Rutherford s model was still slightly incomplete continues in Chapter 5!

10 Chapter 4 Atomic Structure 4.1 Defining the Atom 4.2 Structure of the Nuclear Atom 4.3 Distinguishing Among Atoms

11 DISTINGUISHING ATOMS OF DIFFERENT ELEMENTS Elements are different because they contain different numbers of protons ØProtons and electrons are the particles responsible for chemical behavior An element s ATOMIC NUMBER is equal to the number of protons in the nucleus of an atom of that element For example, the atomic number of hydrogen is 1, and all atoms of hydrogen contain just 1 proton Therefore, elements are distinguished by the number of protons in their atoms, which the atomic number is also determined from ØWe can find atomic numbers of elements on the period table!

12 Atoms are electrically neutral, so they must contain the same number of electrons as protons (negative charge = positive charge)

13 MASS NUMBER An atom s mass is concentrated in its nucleus Depends on the number of protons and neutrons Mass number = (# protons) + (# neutrons) ØEx. Helium has 2 protons & 2 neutrons, and its mass number = 4 ØEx. Carbon has 6 protons & 6 neutrons, and its mass number = 12 We can use the atomic number (# protons) and mass number to find the number of neutrons # neutrons = mass number atomic number # neutrons = (# protons + # neutrons) - (# protons)

14 INFORMATION OBTAINED FROM THE PERIODIC TABLE Atomic number Mass number #$Mn $$ Shorthand notation: ØWrite the mass number as a superscript (above) to the symbol ØWrite the atomic number as a subscript (below) to the symbol

15 ISOTOPES OF AN ELEMENT Atoms that have the same (normal) number of protons but different numbers of neutrons ØThis results in different mass numbers between isotopes ØStill chemically alike due to the same numbers of protons and electrons

16 ISOTOPES OF AN ELEMENT Atoms that have the same (normal) number of protons but different numbers of neutrons ØThis results in different mass numbers between isotopes ØStill chemically alike due to the same numbers of protons and electrons Hydrogen also has three known isotopes ØHydrogen: 1 1H has 0 neutrons ØDeuterium: 2 1H has 1 neutron ØTritium: 3 1H has 2 neutrons Isotopes of an elements are present in different abundances in nature

17 ATOMIC MASS & ATOMIC MASS UNIT (AMU) Atomic masses can be determined using a mass spectrometer Carbon-12 is the reference isotope: it has been assigned a mass of exactly 12 amu amu = atomic mass units ØOne amu is defined as 1/12 of the mass of a carbon-12 atom ØThe mass of 1 proton OR 1 neutron is approx. = 1 amu Carbon-12 has 6 protons + 6 neutrons = 12 amu (often will see 12 g) Because most elements occur as a mixture of two or more isotopes in nature, we use the natural percent abundance to determine the atomic mass

18 AVERAGE ATOMIC MASS: ON PERIODIC TABLE Atomic mass of an element is the weighted average mass of atoms in a naturally occurring sample of the element ØWhat is meant by weighted? To calculate, multiply the mass of each isotope by its natural abundance, expressed as a decimal, and then add the products Ø99.89% =

19 CRASH COURSE VIDEO The Histroy of Atomic Chemistry

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