H Chemistry: Unit 4 Flashcards by kate finneman

periodicity

study of the trends on the periodic table

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octet rule

every element on the periodic table wants 8 electrons in their highest energy level(noble gas configuration) except hydrogen and helium

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oxidation number

charge an atom has when it acquires an octet; the oxidation number for transitional elements vary

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metals

solids and good conductors of heat and electricity

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non-metals

gases and poor conductors of heat and eletricity

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metalloid

moderate conductors of heat and electricity

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group 1 elements

alkali metals

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group 2 elements

alkaline earth metals

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group 6 elements

chalcogens

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group 7 elements

halogens

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group 8 elements

noble gases

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atomic radius

half the distance between the nuclei of 2 like atoms; measured in angstroms

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atomic radius trend

increases as you move down and left

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ionization energy

energy required to remove an electron from an atom; measured in volts

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ionization energy trend

increases as you move up and right

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electronegativity

ability of an atom to attract electrons to itself; measured in Paulings’

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electronegativity trend

increases as you move up and right

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shielding effect

electrons closer to the nucleus shield the outer electrons from the pull of the nucleus; increases with the number of electrons

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shielding effect trend

increases as you move down and right

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ionic radius

size of an atom compared to the atomic radius when a atom gains or loses electrons

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chemical bond

bond between atoms

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ionic bond

electrostatic force between atoms(cation and anion); formula unit or salt

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cation

positive

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anion

negative

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properties of an ionic compound

1.form a crystal lattice 2.high melting and boiling points 3.salts are solid, hard, and brittle 4.form an electrolyte

lattice energy

energy required to remove an ion from a crystal

electrolyte

substance that conducts electricity when dissolved

monatomic ion

ion made up of one atom; everything on periodic table

polyatomic ion

ion made of more than 1 atom

an ionic compound is

neutral

naming ionic compounds- cation first

-if the cation is an element on the periodic table, use its name -if the cation is polyatomic, use its unique name -if the cation is a transition metal with more than one share, use a Roman numeral to indicate its charge

naming ionic compounds- anion second

-if the anion is monatomic off the periodic table, use its root name and add the suffix "-ide" -if the anion is polyatomic, use its unique name on the periodic table

covalent bond

bond between atoms where electrons are shared; molecule

the covalent bond occurs when

attraction and repulsion forces are in balance

attraction forces

nucleus of 1 atom attracted to the electrons of the other

repulsion forces

nuclei of both atoms and the electrons of both atoms repel each other

single covalent bond

sigma bond; bond between atoms where one pair of electrons are shared

double covalent bond

1 sigma & 1 pi; bond between atoms where 2 pairs of electrons are shared

pi bond

bond between parallel orbitals that overlap

triple covalent bond

1 sigma & 2 pi; bond between atoms where 3 pairs of electrons are shared

bond length

distance between bonded nuclei; the shorter the bond, the stronger it is; multiple bonds are shorter and stronger

bond dissociation energy(BDE)

energy required to break a covalent bond

diatomic gases

7 elements on the periodic table that exist in nature in pairs; I H N Cl O Br F

resonance structure

lewis structure that can be drawn in more than one way to illustrate the sharing of a double bond; use a double arrow

expanded octet

center atom will occasionally bond with empty d orbitals and have more than 8 electrons in the highest energy level(s & p)

VSEPR(valence shell electron pair repulsion) theory

unshared pairs of electrons on the center atom in a lewis structure take up space

A.X.E Notation

A- center atom X- atoms that re bonded to the center atom E- unshared pairs of electrons

AX2

linear

AX3

trigonal planar

AX4

tetrahedral

AX3E

trigonal pyramidal

AX2E2

bent

AX5

trigonal bipyramidal

naming molecules- prefix method

prefixes indicate the number of atoms in the molecule

naming molecules- 1

mono

naming molecules- 2

naming molecules- 3

tri

naming molecules- 4

tetra

naming molecules- 5

penta

naming molecules- 6

hexa

naming molecules- 7

hepta

naming molecules- 8

octa

naming molecules- 9

nona

naming molecules- 10

deca

naming molecules

1. first element- use a prefix and its name off of the periodic table 2. second element- use a prefix and its root name off periodic table with the "-ide" suffix 3. omit "mono" from first element

acid

substance that donates hydrogen to a solution and lowers pH; anion determines acid name