SCIENCE 9: 2nd Quarter Flashcards by Nur Amna Aisha Onsing

Anything that has mass

Matter

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Smallest unit of matter

Atom

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A.P.E

Atomic # found on top of the element’s symbol is equivalent to the protons and electrons.

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Greek Philosopher

Democritus

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He named the smallest piece of matter “atomos” means not to be cut.

Democritus

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He said that it is all small, hard particles that are made of same material but different shapes and sizes.

Democritus

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He said that all elements are composed of atoms.

John Dalton

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Atoms of the same elements are alike, atoms of different elements are different.

John Dalton

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Introduced electron

Joseph John Thomson

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His experiment is the “Plum Pudding”.

Joseph John Thomson

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He said positive atoms (protons) are inside at the nucleus, and the negative charged are outside the nucleus scattered.

Ernest Rutherford

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Proposed an improvement, each electron are in a specific energy level, it moved in definite orbits around the nucleus.

Niels Bohr

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Modified Niels Bohr atomic theory to include elliptical orbits.

Arnold Sommerfeld

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Father of quantum mechanics

Erwin Schrondinger

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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

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Discovered protons

Eugene Goldstein

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Study of waves

Quantum Mechanics

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Discovered Neutrons

James Chadwick

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Smallest particle of an element

Atoms

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Smallest amount of substance that can take part in any chemical reaction

Atom

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He said that atoms are made of positively charged particle with negatively charge electrons

Joseph, John Thomson

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When sodium and chlorine bond they make the ___ sodium chloride

Compound

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When two or more elements bond they make a??

Compound

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They have different properties than the elements that make them up

Compound

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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

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

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

Nonmetals have more than __ valence electrons

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