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Year 10 Science > Term 3- Chemistry > Flashcards

Term 3- Chemistry Flashcards

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1
Q

element

A

one type of atom- can be a single atom or diatomic- differ from number of subatomic particles

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2
Q

atoms

A

basic unit of matter

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3
Q

nucleus

A

dense center of an atom surrounded by cloud of negatively charged behaviour

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4
Q

subatomic particles

A

particles within and surrounding nucleus

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5
Q

proton

A

positively charged particle

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6
Q

neutron

A

neutral particle

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7
Q

electron

A

negatively charged particle

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8
Q

Periodic Law

A

when elements are arranged in order of increasing atomic number, there is a periodic repetition of their physical and chemical properties

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9
Q

names for columns and rows in PT

A

columns > groups; rows > periods

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10
Q

classes in PT

A

metals, non-metals, and metalloids

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11
Q

similarity between elements in the same period

A

same number of shells

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12
Q

similarities between elements in the same group

A

same number of valence electrons and similar chemical properties

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13
Q

properties of metals

A
  • good conductors of heat and electricity
  • shiny
  • ductile
  • malleable
  • reaction with water- corrosion
  • solid at room temperature (except Mercury)
  • sonorous
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14
Q

properties of non-metals

A
  • poor conductors
  • not ductile or malleable
  • brittle
  • dull in colour
  • dull sound when hit
  • many are gases
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15
Q

properties of metalloids

A
  • properties of both metals and non-metals
  • shiny or dull
  • better conductors than non-metals; not as well as metals
  • ductile and malleable
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16
Q

types of bonding

A

ionic, covalent, and metallic

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17
Q

ionic bonding

A
  • 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
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18
Q

covalent bonding

A
  • between non-metals
  • sharing valence electrons with each other
  • molecular structure
  • gases, liquids, or low melting points solids
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19
Q

metallic bonding

A
  • between metals
  • sea of electrons- valence electrons are shared among atoms, free to move between atoms
  • crystalline structure
  • solid state
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20
Q

cations

A

positively charged ion

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21
Q

anions

A

negatively charged ion

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22
Q

ions

A

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)

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23
Q

how to name ionic compounds

A
  1. name cation first
  2. name anion second
  • for single ions- elemental non-metal name + ‘ide’
  • for polyatomic ions- name from the ions table
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24
Q

types of reactions

A
  • synthesis
  • decomposition
  • single displacement
  • double displacement
  • combustion
  • oxidation
  • reduction
  • precipitation
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25
Q

rules to determine products of decomposition

A
  • 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
26
Q

types of matter

A

mixtures and pure substances

27
Q

types of mixtures

A

heterogeneous and homogeneous mixtures

28
Q

types of pure substances

A

elements and compounds

29
Q

molecule

A

combination of more than one atom chemically bonded

30
Q

compound

A

combination of more than one type of element chemically bonded

31
Q

mixtures

A

two or more substances that are combined, and can be separated by physical means

32
Q

solutions

A

mixture where one substance dissolves in another

33
Q

number of electrons in shell order

A

2, 8, 18 (8 for the first 18 elements of the periodic table)

34
Q

formula for electrons in shells

A

nth shell = 2(n^2)

35
Q

atomic number

A

number of protons in the nucleus

36
Q

mass number

A

number of protons plus neutrons in the nucleus

37
Q

isotopes

A

element with the same number of protons but different number of neutrons

38
Q

valency

A

the charge of an ion required for bonding

the charge an ion will form when it gains or loses electrons

39
Q

which electrons have the most energy?

A

those furthest away

40
Q

Bohr Diagrams

A

how-to-bohr-diagram.ppt

41
Q

skeleton equation

A

which atoms, not how many molecules

42
Q

balanced chemical equation

A

shows all atoms, including coefficients (how many)

43
Q

precipitation reactions

A

two products during double displacement reaction form at least one solid

44
Q

double displacement reactions

A

parts of two aqueous compounds switch places to form two new ones
AB + CD > AD + CB

45
Q

decomposition reaction

A

a more complex substance breaks down into two or more simple parts

46
Q

combination (synthesis) reaction

A

two or more reactants combine to form single product

47
Q

single displacement reaction

A

a more reactive substance will displace a less reactive one

A + BC > B + AC

48
Q

oxidation reaction

A

when oxygen is added (e.g. combustion and erosion); hydrogen is lost, electrons are lost, increase in oxidation number

49
Q

reduction reaction

A

when oxygen is removed from an element; combine with hydrogen, gain electrons, decrease in oxidation number

50
Q

combustion reaction

A

when a fuel combines with oxygen, to produce carbon dioxide and water
(e.g. cellular respiration)

51
Q

rate of reaction

A

the speed at which a chemical reaction proceeds

52
Q

what is rate of reaction influenced by (6 factors)

A

surface area of a solid reactant, concentration or pressure, temperature, catalyst, nature of reactants

53
Q

CO3(^2-)

A

carbonate

54
Q

Cl(^-)

A

chloride

55
Q

OH(^-)

A

hydroxide

56
Q

NO3(^-)

A

nitrate

57
Q

NO2(^-)

A

nitrite

58
Q

SO4(^2-)

A

sulfate

59
Q

SO3(^2-)

A

sulfite

60
Q

NH4(^+)

A

ammonium

Year 10 Science (2 decks)

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