Atoms and Elements. Elements each element has a unique number of protons in its nucleus the number of protons in the nucleus of an atom is called the

Atoms and Elements

Elementseach element has a unique number of

protons in its nucleusthe number of protons in the nucleus of an

atom is called the atomic numberthe elements are arranged on the Periodic

Table in order of their atomic numberseach element has a unique name and

symbolsymbol either one or two letters

one capital letter or one capital letter + one lowercase

Tro, Chemistry: A Molecular Approach 2

Structure of the Nucleus

Soddy discovered that the same element could have atoms with different masses, which he called isotopes

The observed mass is a weighted average of the weights of all the naturally occurring atomsthe percentage of an element that is 1 isotope is

called the isotope’s natural abundance


Isotopesall isotopes of an element are chemically

identicalundergo the exact same chemical reactions

all isotopes of an element have the same number of protons

isotopes of an element have different massesisotopes of an element have different numbers of

neutronsisotopes are identified by their mass numbers

protons + neutrons



• Atomic Number Number of protons Z

• Mass Number Protons + Neutrons Whole number A

• Abundance = relative amount found in a sample


9.25%221210Ne-22 or

0.27%211110Ne-21 or

90.48%201010Ne-20 or

Percent Natural Abundance

A, Mass Number

Number of Neutrons

Number of ProtonsSymbol

Ne2010

Ne2110

Ne2210

ExamplesWhat are the atomic number (Z), mass

number (A) and symbol for the carbon isotope with 7 neutrons

How many protons, electrons and neutron are present in an atom

Cr52

24

Reacting Atomswhen elements undergo chemical reactions,

the reacting elements do not turn into other elementsDalton’s Atomic Theory

since the number of protons determines the kind of element, the number of protons in the atom does not change in a chemical reaction

however, many reactions involve transferring electrons from one atom to another


Charged Atomswhen atoms gain or lose electrons, they acquire

a chargecharged particles are called ionswhen atoms gain electrons, they become

negatively charged ions, called anions (Cl-)when atoms lose electrons, they become

positively charged ions, called cations (Na+)ions behave much differently than the neutral

atome.g., The metal sodium, made of neutral Na atoms, is

highly reactive and quite unstable. However, the sodium cations, Na+, found in table salt are very nonreactive and stable


Atomic Structures of Ions

Nonmetals form anionsFor each negative charge, the ion has 1

more electron than the neutral atomF = 9 p+ and 9 e-, F─ = 9 p+ and 10 e-


•Metals form cations•For each positive charge, the ion has 1 less electron than the neutral atom

Na atom = 11 p+ and 11 e-, Na+ ion = 11 p+ and 10 e-

Mendeleevorder elements by atomic masssaw a repeating pattern of properties Periodic Law – When the elements are

arranged in order of increasing atomic mass, certain sets of properties recur periodically

put elements with similar properties in the same column

used pattern to predict properties of undiscovered elements

where atomic mass order did not fit other properties, he re-ordered by other propertiesTe & I


Mendeleev’s Predictions for Ekasilicon (Germanium)

12

Property Silicon’s Props

Tin’s Props

Predicted Value

Measured Value

Atomic Mass

28 118 72 72.6

Color Grey White metal

Grey Grey- White

Density 2.32 7.28 5.5 5.4

Reaction w/ Acid &

Base

Resists Acid, Reacts Base

Reacts Acid,

Resists Base

Resists Both

Resists Both

Oxide SiO2 SnO2 Eks1O2 GeO2


Metalssolids at room temperature, except

Hgreflective surface

shinyconduct heatconduct electricitymalleable

can be shapedductile

drawn or pulled into wireslose electrons and form cations in

reactionsabout 75% of the elements are metalslower left on the tableTro, Chemistry: A Molecular Approach 14

Nonmetalsfound in all 3 statespoor conductors of heatpoor conductors of electricitysolids are brittlegain electrons in reactions to

become anionsupper right on the table

except H


Sulfur, S(s)

Bromine, Br2(l)

Chlorine, Cl2(l)

Metalloidsshow some

properties of metals and some of nonmetals

also known as semiconductors


Properties of Siliconshiny

conducts electricitydoes not conduct heat well

brittle

= Metal

= Metalloid

= Nonmetal

The Modern Periodic TableElements with similar chemical and

physical properties are in the same columncolumns are called Groups or Families

designated by a number and letter at toprows are called Periodseach period shows the pattern of

properties repeated in the next period




= Alkali Metals

= Alkali Earth Metals

= Noble Gases

= Halogens

= Lanthanides

= Actinides

= Transition Metals

Important Groups - Hydrogennonmetalcolorless, diatomic gas

very low melting point and densityreacts with nonmetals to form molecular

compoundsHCl is acidic gasH2O is a liquid

reacts with metals to form hydridesmetal hydrides react with water to form H2

HX dissolves in water to form acidsTro, Chemistry: A Molecular Approach 21

Important Groups - Alkali Metals

Group IA = Alkali Metalshydrogen usually placed here,

though it doesn’t belongsoft, low melting points, low

densityflame tests Li = red, Na =

yellow, K = violetvery reactive, never find

uncombined in naturetend to form water-soluble

compounds, therefore crystallized from seawater then molten salt electrolyzed

colorless solutionsreact with water to form basic

(alkaline) solutions and H22 Na + 2 H2O 2 NaOH + H2 releases a lot of heat

22

lithium

sodium

potassium

rubidium

cesium

Important Groups - Alkali Earth MetalsGroup IIA = Alkali Earth Metalsharder, higher melting, and

denser than alkali metals Mg alloys used as structural

materialsflame tests Ca = red, Sr = red,

Ba = yellow-greenreactive, but less than

corresponding alkali metalform stable, insoluble oxides

from which they are normally extracted

oxides are basic = alkaline earthreactivity with water to form H2

Be = none; Mg = steam; Ca, Sr, Ba = cold water


magnesium

calcium

beryllium

strontium

barium

Important Groups - Halogens

Group VIIA = HalogensnonmetalsF2 and Cl2 gases; Br2 liquid; I2

solidall diatomicvery reactiveCl2, Br2 react slowly with water

Br2 + H2O HBr + HOBrreact with metals to form ionic

compoundsHX all acids

HF weak < HCl < HBr < HI


bromine

iodine

chlorine

fluorine

astatine

Important Groups - Noble Gases

Group VIIIA = Noble Gases

all gases at room temperature very low melting and boiling

pointsvery unreactive, practically

inertvery hard to remove

electron from or give an electron to


helium

neon

argon

krypton

xenon

Atomic Masswe previously learned that not all atoms of

an element have the same massisotopes

we generally use the average mass of all an element’s atoms found in a sample in calculations

we call the average mass the atomic mass


nn isotope of massisotope of abundance fractional MassAtomic

Mass Spectrometrymasses and abundances of isotopes are

measured with a mass spectrometeratoms or molecules are ionized, then

accelerated down a tubesome molecules into fragments are broken

during the ionization processthese fragments can be used to help determine

the structure of the moleculetheir path is bent by a magnetic field,

separating them by masssimilar to Thomson’s Cathode Ray Experiment


Mass Spectruma mass spectrum is a

graph that gives the relative mass and relative abundance of each particle

relative mass of the particle is plotted in the x-axis

relative abundance of the particle is plotted in the y-axis


ExampleIf copper is 69.17% Cu-63 with a mass of

62.9396 amu and the rest Cu-65 with a mass of 64.9278 amu, find copper’s atomic mass

Magnesium has three naturally occurring isotopes with masses of 23.99 amu, 24.99 amu, and 35.98 amu and natural abundances of 78.99%, 10.00% and 11.01% respectively. Calculate the atomic mass of magnesium

Counting Atoms by Moles

If we can find the mass of a particular number of atoms, we can use this information to convert the mass of an element sample into the number of atoms in the sample.

The number of atoms we will use is 6.022 x 1023 and we call this a mole

1 mole = 6.022 x 1023 things Like 1 dozen = 12 things


Chemical Packages - Moles

mole = number of particles equal to the number of atoms in 12 g of C-12

1 atom of C-12 weighs exactly 12 amu 1 mole of C-12 weighs exactly 12 g

The number of particles in 1 mole is called Avogadro’s Number = 6.0221421 x 1023

1 mole of C atoms weighs 12.01 g and has 6.022 x 1023 atoms

the average mass of a C atom is 12.01 amu


ExamplesCalculate the number of atoms in 2.45 mol

of copperA pure silver ring contains 2.80 x 1022

silver atoms. How many moles of silver atoms does it contain?

Relationship Between Moles and Mass

The mass of one mole of atoms is called the molar mass

The molar mass of an element, in grams, is numerically equal to the element’s atomic mass, in amu

The lighter the atom, the less a mole weighs The lighter the atom, the more atoms there

are in 1 g



Substance Weight of

1 atom Pieces in 1 mole

Weight of 1 mole

hydrogen 1.008 amu 6.022 x 1023 atoms 1.008 g

carbon 12.01 amu 6.022 x 1023 atoms 12.01 g

oxygen 16.00 amu 6.022 x 1023 atoms 16.00 g

sulfur 32.06 amu 6.022 x 1023 atoms 32.06 g

calcium 40.08 amu 6.022 x 1023 atoms 40.08 g

chlorine 35.45 amu 6.022 x 1023 atoms 35.45 g

copper 63.55 amu 6.022 x 1023 atoms 63.55 g

1 molesulfur

32.06 g

1 molecarbon12.01 g

Converting between mass, moles and atoms

g C mol C

mol C g C

g C mol C atoms

Calculate the moles of carbon in 0.0265 g of pencil lead

Calculate the amount of copper (in moles in a 35.8 g pure copper sheetHow many atoms are there?

Calculate the mass (in grams) of 0.473 moles of titanium

Documents

Atoms and Elements. Elements each element has a unique number of protons in its nucleus the number of protons in the nucleus of an atom is called the