SCIENCE 9: 2nd Quarter Flashcards
Anything that has mass
Matter
Smallest unit of matter
Atom
A.P.E
Atomic # found on top of the element’s symbol is equivalent to the protons and electrons.
Greek Philosopher
Democritus
He named the smallest piece of matter “atomos” means not to be cut.
Democritus
He said that it is all small, hard particles that are made of same material but different shapes and sizes.
Democritus
He said that all elements are composed of atoms.
John Dalton
Atoms of the same elements are alike, atoms of different elements are different.
John Dalton
Introduced electron
Joseph John Thomson
His experiment is the “Plum Pudding”.
Joseph John Thomson
He said positive atoms (protons) are inside at the nucleus, and the negative charged are outside the nucleus scattered.
Ernest Rutherford
Proposed an improvement, each electron are in a specific energy level, it moved in definite orbits around the nucleus.
Niels Bohr
Modified Niels Bohr atomic theory to include elliptical orbits.
Arnold Sommerfeld
Father of quantum mechanics
Erwin Schrondinger
Today’s atomic model is based on the principles of wave mechanics. Electrons whirl, electrons don’t move around atom in definite path, it also does not move in random patterns.
Erwin Schrondinger
Discovered protons
Eugene Goldstein
Study of waves
Quantum Mechanics
Discovered Neutrons
James Chadwick
Smallest particle of an element
Atoms
Smallest amount of substance that can take part in any chemical reaction
Atom
He said that atoms are made of positively charged particle with negatively charge electrons
Joseph, John Thomson
When sodium and chlorine bond they make the ___ sodium chloride
Compound
When two or more elements bond they make a??
Compound
They have different properties than the elements that make them up
Compound
Sodium+ chlorine=
Sodium chloride= table salt
Compounds in ___ retain their individual properties
Mixtures
It is a substance composed of two or more elements chemically bonded together.
Compound
It is a combination of different substances that are not chemically bonded
Mixture
It can be separated by physical means
Mixture
Can only be separated by chemical means
Compounds
Are pure substances
Elements
Group, 14 to 17
Nonmetals
Nonmetals
Groups, 14 to 17
Metals
Group one to 13
Group 1to 13
Metals
Noble gas
Group 18
The group number will give you an idea of the
Number of valence electron
The __ will give you an idea of the number of valence electrons
Atomic number
S Block
Group one, and two
P block
Group, 13 to 18
Metals have __ valence electrons
Low
Non-metals have __ valence electron
High
All noble gas has __ valence electrons
Eight
What do you notice in the number of valence electrons of metals, nonmetals and noble gases?
Metals have lesser valence electrons than nonmetals. All noble gases have eight valence electron.
Electrons in the outermost energy level
Valence electron
Electrons that are transferred or shared when atoms bond together
Valence electron
Energy needed to remove outermost valance electrons
Ionization
Tendency of an atom to attract valence electrons
Electronegativity
What do you notice with the number of valence electrons, electronegativity values, and ionization energies of the element?
As the number of valence electron increases, electronegativity and ionization also increases
What kind of element has the greatest tendency to attract electrons why?
Nonmetals have the greatest tendency to attract electrons because they have high electronegativity
What kind of elementary was high energy to remove its valence electrons why?
Nonmetals have high energy requirements to pull its valence electron
It tells you that elements gain or loose or share electrons to achieve the electronic configuration of the nearest noble gas
The octet rule
After chemical bonding elements become __ with the nearest noble gas
Isoelectronic
Same electrons, even though different atomic numbers
Isoelectronic
Our areas within shells where the electrons are located
Orbitals
We know that electron is somewhere in the orbital, but we can’t know exactly where it is or how fast it is moving
Heinsberg’s uncertainty principle
Is the arrangement of electrons around the nucleus based on their energy level?
Electronic configuration
Electrons are added one at a time to the lowest energy level first
Aufbau principle
Two elections in same orbital have different spins
Pauli exclusion principle
When electrons are filling orbitals of the same energy, they prefer to enter empty, orbitals first. These electrons all have the same spin.
Hund’s Rule
The transfer of electrons
Ionic band
The form between metals and nonmetals
Ionic bond
It dissolves easily in water
Ionic compounds
It easily conduct electricity
Ionic compound
It tends to form crystals with high melting temperature
Ionic compound
Bonding by sharing
Covalent bonding
Two types of covalent bond
Polar and nonpolar
Non-identical atoms with electronegativity higher than 0.4 and lower than 1.9
Polar
Two identical, non-metallic atoms, such as nitrogen, oxygen, fluorine, and diatomic particles
Nonpolar
Diatomic elements
Have no fear of ice cold bromine
Compounds that are primarily composed of carbon atoms
Organic compounds
Are naturally produced by living organisms, but can also be produced artificially
Organic compounds
Carbon atoms have __ valence electrons
4
To identify organic compounds
Physical properties, boiling point density, color, smell, and stability
Organic compounds examples
Gasoline kerosene, LPG, ethanol, acetone and acetic acid
Low electronegativity
Metals
High electronegativity
Nonmetals
Metals have less than __ valence electrins
4
Nonmetals have more than __ valence electrons
4
Symbol with dot around
Lewis symbol
Ionization group trend
As you go down a column ionization energy decreases
Ionization period trend
As you go left or right, it increases
Electronegativity periodic trend
As you go, left or right electronegativity increases
Electronegativity group trend
As you go down a column electronegativity decreases
Atomic radius group trend
As you go down a column atomic radius increases
Atomic radius, periodic trend
As you go left or right atomic radius decreases
Unsaturated
Alkene and alkyne
Saturated
Alkane
Single bond
Alkane
Double bond
Alkene
Triple bond
Alkyne
Composed of hydrogen and carbon
Hydrocarbon
4 carbon to be stablr
Hydrocarbon
1 carbon
Meth
2 carbon
Eth
3 carbon
Prop
4 carbon
But
5 carbon
Pent
6 carbon
Hex
7 carbon
Hept
8 carbon
Oct
9 carbon
Non
10 carbon
Dec
