Chemistry P1

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Chemistry

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50 Terms

1
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What is matter?

Anything that occupies space and has mass

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What is an atom?

Smallest unit of matter

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What is physical properties?

Can be observed without changing the substance into something new; not changing its chemical formula

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What are some examples of physical properties of matter

Colour, hardness, density, malleability, melting point

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What are the 3 phases of matter?

Solid, liquid, gas

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What is a phase change?

When matter changes from one state to another

<p>When matter changes from one state to another</p>
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Describe solids

Fixed shape and volume

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Describe liquids

No definite shape

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Describe gases

No designed shape or colume

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What is chemical propeties?

How a substance behaves when it reacts to form a new substance; changing its chemical formula

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What are some examples of the chemical properties of matter?

Burning, toxicity, oxidation, etc

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What is a pure substance?

Matter that is only made up of one substance and cannot be physically separated into any other matter; elements and compounds

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What are the 2 types of pure substances and describe them

Elements - Can be found on the periodic table

ex)Helium, Hydrogen

Compounds - Found naturally, mix of elements together

Ex) H2O, NaCl

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What is a mixture?

The physical mixing of 2 or more components; Homogenous and heterogenous

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What are the 2 types of mixtures and describe them

Homogenous - Looks like one substance

Ex) Soda, Orange juice

Heterogenous - You can see the physical components it is made of

Ex) Salad, trail mix

16
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What is the Dalton’s Billiard Ball Model?

  • The foundation of Atomic theory

  • Atoms are spherical like billiard balls

  • Each atom has its own unique properties

  • Atoms are indivisible; they are the building blocks of life

  • Atoms can combine in many ways to create a wide variety of elements/compounds

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What is the Thomson’s Raisin Bun Model?

  • Thomson discovers the electron

  • The electron is 2000X smaller than the smallest atom and has a negative charge

  • Atoms must contain electrons

  • Electrons must be spread-out evenly throughout a positively charged atom like raisins in a bun

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What is Rutherford’s Gold Foil Experiment?

  • Alpha particles from radioactive polonium were fired at a thin piece of gold foil

  • Most alpha particles pass through the gold undeflected

  • Atoms have a very small nucleus where almost all of the mass is located. Since the nucleus is so small, the alpha particles had a small chance of actually hitting it

  • Rutherford discovered the nucleus was made up of protons and neutrons

  • Electrons orbit the outside of the nucleus, like planets around the son. Most volume of an atom is empty space

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What is the Bohr model of the atom?

  • Electrons exist at certain distances from the nucleus(called orbits, shells, or energy levels)

  • Max number for the 1st energy level = 2e-

  • Max number for the 2nd and 3rd energy level = 8e-

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What is the Electrons cloud model of an atom(Schrodinger&Heisenberg)?

  • We can’t exactly know where an electron is at any given time, but electrons are more likely to be in specific areas

  • E- are in a cloud

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Define elements

Made of atoms, atoms are made from subatomic particles

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What is the charge, mass, symbol, and location of a Electron?

Charge - Negative

Mass - No mass

Symbol - e-

Location - Cloud, around the nucleus

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What is the charge, mass, symbol, and location of a Proton?

Charge - positive

Mass - 1

Symbol - p/p+/H+

Location - In the nucleus

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What is the charge, mass, symbol, and location of a Neutron?

Charge - No charge, neutral

Mass - 1

Symbol - n

Location - In the nucleus

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What subatomic particle makes up most of the volume of an atom?

Electrons

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What subatomic particles makes up most of the mass of an atom?

Neutrons and protons

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What is the atomic number?

The # of protons and electrons in an element

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What is the atomic mass?

The average weight of one element = protons and neutrons

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What is an Ion?

When an electron is being added or taken away; an atom that has a positive or negative charge

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Why is Hydrogen so special?

  • Because it doesn’t belong to a specific group

  • It’s a non-metal that acts like a metal

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Describe metal and where is it located on the periodic table?

Located to the left of the “staircase” and typically gives electrons

  • Conductors of energy and heat

  • Malleable

  • Ductile

  • Luster

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Describe Non-Metals and where is it located on the periodic table?

Located to the right of the “staircase” and typically accepts electrons

  • Poor conductors

  • Brittle

  • Not ductile

  • Lack luster

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Describe metalloids and where is it located on the periodic table?

Is considered the “staircase” which separates metals and non-metals and typically gives electrons

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What are periods in the periodic table?

  • The rows of elements from left to right.

  • Total of 7 periods

  • The row number is equivalent to the energy levels

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What is groups/family in the periodic table?

  • The rows of elements from up to down

  • Total of 18 groups/families

  • Groups is numerical while family is names

  • The # of e- in the last energy level or valence e-, only works for g1-3, g13-18

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What is group1 in the periodic table?

It’s called the Alkali Metals and are very reactive with H2O(water)

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What is group2 in the periodic table?

It’s called the Alkaline Earth Metals and are less reactive with H2O(water)

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What is group17 in the periodic table?

It’s called the Halogens and are very reactive non-metals

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What is group18 in the periodic table?

It’s called the Noble Gases and are non-reactive

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What are naturally diatomic elements?

Elements that are paired when alone'

H O N Cl Br I F

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What are examples of polyatomic elements?

Sulfur has 8 and phosphorus has 4

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What are valence e-

The electrons in the outermost shell of an atom

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What can we learn about atoms from the Bohr energy level diagrams?

  • How many valence e- are in the last energy level

  • Tells us the reaction behavior of the atom; whether an atom is going to give or take e-

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How are ions formed?

By gaining or losing e-

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Describe and explain Ionic compounds

  • Bond between non-metal and metal

  • Transfer electrons

  • Solid at room temp

  • Can conduct in solutions as long as they can dissolve in water

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Describe and explain molecular compounds

  • Bond between non-metal and non-metal

  • Share electrons

  • Solid, liquid, and gas at room temp

  • Low to no conductivity in solutions

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What are compound subscripts?

They indicate the number of particular type of atom in the chemical formula for a molecule or a compound

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What are compound coefficients?

Coefficients appear in front of a compound formula to indicate how many compounds of that type are

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What are properties of ionic compounds?

  • High melting point

  • Retain their crystal shape

  • Vary in solubility

  • Are conductors when they dissolve in solutions. Ionic compounds that do dissolve and conduct electricity are called electrolytes

  • Form 3D grids called lattices

50
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What does IUPAC stand for?

International committee of pure and applied chemist