Term 3- Chemistry Flashcards
element
one type of atom- can be a single atom or diatomic- differ from number of subatomic particles
atoms
basic unit of matter
nucleus
dense center of an atom surrounded by cloud of negatively charged behaviour
subatomic particles
particles within and surrounding nucleus
proton
positively charged particle
neutron
neutral particle
electron
negatively charged particle
Periodic Law
when elements are arranged in order of increasing atomic number, there is a periodic repetition of their physical and chemical properties
names for columns and rows in PT
columns > groups; rows > periods
classes in PT
metals, non-metals, and metalloids
similarity between elements in the same period
same number of shells
similarities between elements in the same group
same number of valence electrons and similar chemical properties
properties of metals
- good conductors of heat and electricity
- shiny
- ductile
- malleable
- reaction with water- corrosion
- solid at room temperature (except Mercury)
- sonorous
properties of non-metals
- poor conductors
- not ductile or malleable
- brittle
- dull in colour
- dull sound when hit
- many are gases
properties of metalloids
- properties of both metals and non-metals
- shiny or dull
- better conductors than non-metals; not as well as metals
- ductile and malleable
types of bonding
ionic, covalent, and metallic
ionic bonding
- between metals and non-metals
- transfer of electrons where opposite charged ions bond with each other (positive with negative) to balance charges
- crystalline structure
- solid state
covalent bonding
- between non-metals
- sharing valence electrons with each other
- molecular structure
- gases, liquids, or low melting points solids
metallic bonding
- between metals
- sea of electrons- valence electrons are shared among atoms, free to move between atoms
- crystalline structure
- solid state
cations
positively charged ion
anions
negatively charged ion
ions
atom or molecule with a net electrical charge due to the loss or gain of one or more electrons (they do this to gain a noble gas electron configuration)
how to name ionic compounds
- name cation first
- name anion second
- for single ions- elemental non-metal name + ‘ide’
- for polyatomic ions- name from the ions table
types of reactions
- synthesis
- decomposition
- single displacement
- double displacement
- combustion
- oxidation
- reduction
- precipitation
rules to determine products of decomposition
- all binary compounds break down into their elements
- carbonates- to oxide and carbon dioxide gas
- chlorates- to chloride and oxygen gas
- metal hydroxides- oxide and water
- oxy acids- non-metal oxide
types of matter
mixtures and pure substances
types of mixtures
heterogeneous and homogeneous mixtures
types of pure substances
elements and compounds
molecule
combination of more than one atom chemically bonded
compound
combination of more than one type of element chemically bonded
mixtures
two or more substances that are combined, and can be separated by physical means
solutions
mixture where one substance dissolves in another
number of electrons in shell order
2, 8, 18 (8 for the first 18 elements of the periodic table)
formula for electrons in shells
nth shell = 2(n^2)
atomic number
number of protons in the nucleus
mass number
number of protons plus neutrons in the nucleus
isotopes
element with the same number of protons but different number of neutrons
valency
the charge of an ion required for bonding
the charge an ion will form when it gains or loses electrons
which electrons have the most energy?
those furthest away
Bohr Diagrams
how-to-bohr-diagram.ppt
skeleton equation
which atoms, not how many molecules
balanced chemical equation
shows all atoms, including coefficients (how many)
precipitation reactions
two products during double displacement reaction form at least one solid
double displacement reactions
parts of two aqueous compounds switch places to form two new ones
AB + CD > AD + CB
decomposition reaction
a more complex substance breaks down into two or more simple parts
combination (synthesis) reaction
two or more reactants combine to form single product
single displacement reaction
a more reactive substance will displace a less reactive one
A + BC > B + AC
oxidation reaction
when oxygen is added (e.g. combustion and erosion); hydrogen is lost, electrons are lost, increase in oxidation number
reduction reaction
when oxygen is removed from an element; combine with hydrogen, gain electrons, decrease in oxidation number
combustion reaction
when a fuel combines with oxygen, to produce carbon dioxide and water
(e.g. cellular respiration)
rate of reaction
the speed at which a chemical reaction proceeds
what is rate of reaction influenced by (6 factors)
surface area of a solid reactant, concentration or pressure, temperature, catalyst, nature of reactants
CO3(^2-)
carbonate
Cl(^-)
chloride
OH(^-)
hydroxide
NO3(^-)
nitrate
NO2(^-)
nitrite
SO4(^2-)
sulfate
SO3(^2-)
sulfite
NH4(^+)
ammonium
