- charged more electrons than protons

Chapter 1 Book Flashcards by Alexis Sprunger

Atoms

all matter is made of

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describe an atom

Nucleus made of proton and neutrons and electron cloud surrounding nucleus

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Atomic number

number of protons

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Cation

+ charged with less electrons than protons

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Anion

charged more electrons than protons

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Isotopes

2 atoms of same element with different number of neutrons

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Mass #

atoms total number of protons and neutrons in nucleus

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Atomic weight

particular element weight from average mass of isotopes

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What is the common H isotope and what is it called

1 proton with no neutrons is called deuterium

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periodic table

schematic arrangement arranged by increasing atomic number

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group number

column of periodic table

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properties similar in columns and rows

similar size
similar electronic and chemical properties

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orbitals and what are they named

region of space that is high electron density spdf

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Shape of S orbital

sphere

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Shape of P orbital

dumbell shape

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Common bonds of atoms

H 1 bond
C 4 bonds
N 3 bonds 1 lone pair
O 2 bonds 2 lone pairs
X 1 bond 3 lone pairs

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How many electrons can S orbital have

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How many electrons can p orbitals have

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Valence electrons

outmost electrons that bond to atoms

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Compounds

2 or more elements

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Octet rule

8 Valence electrons wanted

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Ionic bonds

transfer of electrons to another element

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Covalent bonds

sharing electrons between 2 nucei

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What do ionic bonds form

crystal lattices

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What bonds form molecules?

Covalent bonds

Lone pairs

unshared electrons

lewis structures

electrons dots representation for molecules

formal charge

charge assigned to single atoms in lewis structures

Formula for formal charge

# of VE- (unshared electrons+ 1/2 of bond electrons)

Isomers

more than 1 arrangement of atoms possible from same molecular formula

Constitutional isomers

same molecular formula but connectivity of atoms different

exceptions to the octet rule

H has 2 electrons B and Be not enough electrons P and S more than 8 electrons

resonance structures

2 lewis structures with same placement of atoms but different arrangement of electrons

double-headed arrow

separates 2 resonance structures

resonance hybrids

composite of both forms of resonance structures where electrons are delocalized and resonance stabilized

curved arrow notation

shows how electron positions differ

heteroatom

atom that is not C or H

major contributor

better resonance structure

minor contributor

not the better r structure

What makes a resonance structure better

more bonds fewer charges

Bond length

average distance between centers of 2 bonded nuclei

how does bond length decrease and increase and why?

bond length decreases across row as size of atom decreases bond length increases down a column as size of atom increases

Bond angle

determines shape around any atom bonded

VSEPR theory

electron pairs repel each other

2 groups of electrons around atom

linear 180 degrees

3 groups of electrons around atom

trigonal planar 120 degrees

4 groups of electrons around atom

tetrahedral 109 degrees

discuss lines on a molecule

solid line is in plane wedge is in front of plane dashed is behind plane

trigonal pyramidal

tetrahedral with 1 lone pair 107 degrees

Bent

tetrahedral 2 lone pairs 105 degrees

condensed structures

All atoms bond lines omitted with parenthesis around similar groups with same atoms

Skeletal structures

C is junction of 2 lines or at end of a line with C having enough H draw all heteroatoms charges take place of H with lone pairs

sigma bond

cylindrically symetrical

ground state

lowest energy arrangement

hybridization

2 or more atomic orbitals form some # of hybrid orbitals

sp3

2s1 and 2p3

sp2

2s1 2p2

2s12p1

pi bond

not concentrated on the axis and is weaker

Bond length vs bond strength

increase in bond length= decrease in bond strength decrease in bond length= increase in bond strength therefore short bonds are strong bonds

Joule

SI unit of energy

Calories

O chem energy value unit

Conversion of calories to Joules

1 cal= 4.18 J

percent S character

fraction of hybrid orbital

hybrid s characters percentage and why

sp is 1 2s/ 2 hybrid= 50% s characters sp2 is 1 2s/ 3 hybrid= 33% s character sp3 is 1 2s/ 4 hybrid= 25% s character

What happens to electrons as % s character increases and what about the bonds

As % s character increases, hybrid holds elections closer causing bonds to become shorter and stronger

Electronegativity and how it increases and decrease

measure of atoms attraction for electrons increases across row of PT as nuclear charge increases decreases down column of PT as atomic radius increases

Where is most electronegative element

upper right hand corner

dipole

partial sepration of charge

Polar bond

electronegativity difference between 2 atoms is very small

electrostatic potential map

distribution of electron density in a molecule where electron-rich area is red and electron-deficient is blue

What type of polarity is H2O and why

Polar because O is different than Hs

What type of polarity is CO2 and why

linear molecular cancels out polarity making it nonpolar

Chapter 1 Book Flashcards

(73 cards)