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Grade 10 Science > Chemistry Unit 1 > Flashcards

Chemistry Unit 1 Flashcards

1
Q

Define: Matter

A

anything that takes up space and mass

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2
Q

Define:Mixed substance or Mixture

A

made up of components not found on the periodic table i.e. a mixture

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3
Q

Define: Heterogeneous Micture

A

a mix f substances that have 2 or more phases (appears as more than one thing)

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4
Q

Define: Homogeneous Mixture

A

a mix of substances that have one phase and therefore it looks uniorm

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5
Q

Define: Pure Substance

A

made up of only type of atom found on the periodic table. It contains 1 phase and is homogeneous

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6
Q

Define: Element

A

only one particle that cannot be broken down any further and is straight off the periodic table

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7
Q

Define: Compound Molecule

A

contains two or more elements that move as a single unit

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8
Q

Define: Atom

A

the smallest particle of matter

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9
Q

Define:Atomic Theory

A

a theory describing the structure, behavior and other properties of an atom and it components/parts

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10
Q

Define: Proton

A

a subatomic particle that has a charge of +1, a mass of 1 amu and is found in the nucleus

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11
Q

Define:Neutron

A

a subatomic particle that has a neutral charge, has a mass of 1 amu and is found in the nucleus

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12
Q

Define: Electron

A

a subatomic particle that has a charge of -1, has a mass of approx. 0 amu and is found orbitting the nucleus in shells

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13
Q

Define:Nucleus

A

the very dense center of an atom which contains the protons and the neutrons of the atom.

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14
Q

Define:Shells

A

The rings around the nucleus where electrons orbit the nucleus and can be exchanged or shared among atoms

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15
Q

Define:Bohr-Rutherford Diagram

A

a diagram created to show the atom with its nucleus and all its electrons on their shells

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16
Q

Define: Valence Electrons

A

the electrons on the outermost shell. They are the extra or lacking atoms sitting on the outer shell.

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17
Q

Define: Valence Shell

A

the outermost shell in an atom containing electrons

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18
Q

Define: Periodic Table

A

a way of organizing all the elements in a realistic way where they can be organized by re-activity, state and mass

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19
Q

Define: Period

A

the horizontal rows on a periodic table

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20
Q

Define: Group / Family

A

the vertical columns in the periodic table. Elements of the same group have the same number of valence electrons

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21
Q

Define:Metal

A

conduct electricity well. These include all elements to the left of the “staircase” excluding hydrogen

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22
Q

Define: Non-metal

A

do not conduct electricity well and act as insulators. These include all elements to the right of the staircase plus hydrogen

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23
Q

Define: Metalloid/Semi-Metal

A

have properties of both metals and non-metals. They are the elements that make up the staircase

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24
Q

Define: Alkali Metal

A

are highly reactive because the atom is unstable. They have 1 valence electron so they lose one electron and have an overall charge of +1

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25
Q

Define: Alkaline Earth Metals

A

are reactive because they have 2 valence electrons so they lose 2 electrons to have an overall charge of +2

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26
Q

Define: Halogen

A

highly reactive non-metals because they have 7 valence electrons therefore they only need to gain one electron so they will gain 1 electron to have a charge of -1

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27
Q

Define: Noble Gas

A

gases that are very unreactive because they already have a full shell therefore cannot gain or lose electrons

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28
Q

Define: Atomic Number

A

is the number of protons or electrons

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29
Q

Define: Atomic Mass or Mass Number

A

the number of protons plus the number of neutrons

30
Q

Define: Ion

A

an atom that has gotten an electric charge from gaining or losing electrons

31
Q

Define: Anion

A

an ion that has gained electrons to have a negative charge (since all atoms start with a neutral charge)

32
Q

Define: Cation

A

an ion that has lots electrons t have an overall positive charge

33
Q

Define: Chemical Property

A

are those observed when a substance undergoes a chemical reaction.

34
Q

Define: Physical Property

A

are those that can be observed without chemically changing a substance. Ex. state, melting point, solubility, colour, odour, texture, etc.

35
Q

Define: Reactant

A

the elements and/or compounds that go into a chemical reaction

36
Q

Define: Product

A

the compounds/elements that are created by a chemical reaction

37
Q

Define: Chemical Equation

A

a representation of a chemical reaction by showing the reactants by their symbol and the products

38
Q

Define: Word Equation

A

a chemical reaction expressed in words rather than elemental symbols

39
Q

Define: Skeleton Equation

A

an equation that identifies the reactants and products but does not quantify them

40
Q

Define: Balanced Chemical Equation

A

an equation that identifies the reactants and products and also quantifies them so the number of atoms on both sides is equal

41
Q

Define: Law of Conservation of Mass

A

states that mass can not be created or destroyed so what goes into a chemical reaction must also come out of it as a product

42
Q

Define: Ionic Compound

A

a bond between a metal and a non metal where electrons are exchange so each ion has a full outer shell. They are held together because they have attracting (opposite) electrostatic charges

43
Q

Define: Multivalent Element

A

a metal element that can create more than 1 ion. Ex. iron can become Fe +2 or Fe+3

44
Q

Define: Polyatomic Ion

A

compounds of elements that act and work as a single unit. They consist of more than 2 elements, have no “ide” endings and are mainly negative

45
Q

Define: Covalent Compound

A

a bond between 2 non-metals where the electrons are shared between the atoms. They are held together by the shared electrons.

46
Q

Define: Diatomic Molecule

A

non-metal elements that naturally exist in pairs ex. H2

47
Q

Define: pH Scale

A

The scale that acids and bases are measured on. if a substance has a pH of less than 7 it is acidic, if the pH is 7 then it is neutral and if the pH is more than 7 it is basic

48
Q

Define: Neutral

A

is the value of 7 on the pH scale

49
Q

Define: Acid

A

has a value of less than 7 on the pH scale. This means that the substance has a sour taste, turns blue litmus paper red and contains hydrogen

50
Q

Define: Base

A

a substance with a pH of more than 7 on the pH scale when the substance is in an aqueous solution

51
Q

Define: Acid-Base Indicator

A

it is usually a strip of paper that changes colour when an acid or base is present

52
Q

Define: Precipitate

A

an insoluble solid that forms from a liquid solution

53
Q

Define: Synthesis Reaction

A

a reaction in which 2 elements combine to forma compound. Ex. element+element=compound

54
Q

Define: Decomposition Reaction

A

a reaction in which a compound breaks up to become separate atoms. Ex. Compound=element+element

55
Q

Define: Combustion Reaction

A

a reaction in which a fuel rapidly combines with oxygen to produce carbon dioxide+water (or carbon monoxide+water if it is an incomplete combustion)

56
Q

Define: Single Displacement Reaction

A

a reaction in which an element reacts with an ionic compound where the element replaces one part of the compound and leaves an element by itself. Ex. A+BC=AB+C

57
Q

Double Displacement Reaction

A

a chemical reaction in which the positive or negative ions in 2 ionic compounds switch places. Ex. AB+CD=CB+AD

58
Q

Define: Neutralization

A

a reaction between an acid and a base to produce a salt (ionic compound) and water. This balances the pH level and brings it closer to 7.

59
Q

What are the steps to writing the formula from the name of a Ionic Compound?

A
  1. look at the charges of both elements
  2. write down the metal ion’s symbol, then the non-metal
  3. apply the cross over rule and reduce if possible
60
Q

What are the steps to writing the name from the formula of an Ionic Compound?

A
  1. write the name of the metal
  2. write the name of the non-metal
  3. change the ending of the non-metal to “ide”
    * If there is a polyatomic ion instead of a non-metal, the ending does not change to “ide.”*
61
Q

What are the steps to write the name from the formula of a Multivalent Ionic Compound?

A
  1. write the name of the metal
  2. write the name of the negative ion (non-metal or polyatomic ion)
  3. place Roman numerals for te correct charge between the elements
    (To find the Roman Numeral:
  4. find the et charge of the non-metal
  5. divide the net charge by the num,ber of multivalent atoms
  6. place the result in roman numerals)
62
Q

What are the steps to write the formula from the name for Multivalen Ionic Compounds?

A
  1. find charges for both parts (roman numerals are teh charge for the metal)
  2. write both symbols
  3. apply cross over rule and reduce
63
Q

What are the steps to write the name from the formula of a Covalent Compound?

A
  1. write the first element (if there are more than 1 of that atom, put the correct prefix)
  2. write the second element with the correct prefix
64
Q

What are the steps to write the formula from the name of a Covalent Compound?

A
  1. write the symbol for the first element (if there us a prefix write out the correct number)
  2. write the symbol for the second element with the right number from the prefix
65
Q

What are the prefixes used in Covalent Compounds?

A 
1- mono
2- di 
3- tri
4- tetra 
5- penta 
6- hexa 
7- hepta 
8- octa 
9- non 
10- deca
66
Q

What are the things to remember when writing chemical equations?

A
  • remember diatomic elements if they are by themselves
  • you can’t change subscripts- only add numbers infront of elements
  • always keep states at the end of each compound and balanced equations
67
Q

What are the properties of Acids?

A
  • taste sour
  • don’t feel slippery
  • pH less than 7
  • blue litmus paper turns red
  • releases Hydrogen atoms in aqueous solution
  • corrodes metals
  • reacts with metals to produce a compound plus hydrogen gas
  • their chemical equation starts with hydrogen or ends with COOH
68
Q

What properties do both acids and bases share?

A
  • both dissolve in water
  • both conduct electricity
  • both burn and irritate your skin
69
Q

What are the properties of Bases?

A
  • taste bitter
  • Feel slippery
  • pH greater than 7
  • red litmus paper turns blue
  • release hydroxide ions in aqueous solution
  • do not corrode metals
  • do not react with metals to produce a compound and hydrogen gas
  • their chemical equation starts with a metal ion or ammonium and ends with hydroxide (OH)
70
Q

What is Neutralization and when does it occur?

A
  • occurs when an acid reacts with a base to produce a salt and water
  • it balances the pH and moves it closer to 7
71
Q

What are the steps to name acids?

A
  1. start with “hydro” (since it always starts with hydrogen)
  2. add non-metal and change ending to “ic”
  3. add the word “acid” after

Grade 10 Science (5 decks)

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