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Chemistry 1A > Week One > Flashcards

Week One Flashcards

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1
Q

Atom

A

Chemical species with a central positively charged nucleus surrounded by negatively charged electrons

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2
Q

Free Atoms

A

Usually unstable

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3
Q

Molecules

A

Atoms with definite structure held together by chemical bonds

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4
Q

Molecules- electrical

A

Electrically neutral therefore uncharged

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5
Q

Covalent bonds

A

Sharing electrons between neighbouring atoms

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6
Q

Ions

A

Species that are either positively or negatively charged

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7
Q

Cations

A

Positively charged

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8
Q

Anions

A

Negatively charged

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9
Q

Compounds

A

Substances containing one or more molecules

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10
Q

Law of conservation of mass

A

No gain or loss occurs in chemical reactions, mass is conserved

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11
Q

Law of Definite proportions

A

In chemical compounds, elements are always combined in the same proportion by mass

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12
Q

Law of multiple proportion

A

When 2 elements form one or more compound, the different masses of one element that combine with the same mass of the other element are in ratio of small whole numbers

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13
Q

Daltons Atomic Theory

A

Matter consists of particles
Atoms are indestructible
Atoms of different elements differ in mass and properties

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14
Q

F block elements

A

Bottom two rows of periodic table

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15
Q

D block elements

A

Groups 3-12

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16
Q

S block elements

A

Groups 1-2

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17
Q

P block elements

A

Groups 13-18

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18
Q

Metals - properties

A

Good conductors of heat and electricity
Malleable
Ductile
Metallic lustre

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19
Q

Nonmetals - properties

A 
Poor conductors of heat and electric 
Not malleable
Not ductile 
No metallic lustre
Majority are gases at room temp
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20
Q

Metalliods - properties

A

Tend to be semi conductors

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21
Q

Excited state of electrons

A

Electron lies further from the nucleus, can be promoted to this state by absorption of energy

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22
Q

Redox reactions

A

Reactions in which one or more electrons are transferred between chemical species

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23
Q

Ground state

A

Lowest energy arrangement of electrons in the orbital

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24
Q

Pure substances

A

Have distinct composition and properties

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25
Q

Homogenous Mixtures

A

Can be solutions, consistent throughout, can’t distinguish individual regions

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26
Q

Heterogeneous mixtures

A

Composition varies through, consists of two or more identifiable regions

27
Q

Solids

A

Ordered arrangements, particles close together, low temp high pressure

28
Q

Liquid

A

Disordered wit particles free to move while remaining in close contact (intermediate temp and pressure)

29
Q

Gas

A

Total disorder, much empty space, intermolecular forces broken (high temp low pressure)

30
Q

Physical change

A

Reversible

31
Q

Chemical change

A

Irreversible

32
Q

Chemical property

A

Ability to undergo chemical change

33
Q

Physical property

A

Involves change in form but not chemical identity

34
Q

Isotopes

A

Same number of protons and electrons but different number of neutrons so different mass number

35
Q

Periods

A

Horizontal rows

36
Q

Groups

A

Vertical rows

37
Q

0 degrees

A

273.15 kelvin

38
Q

Exact numbers

A

Come from defined values or from counting objects

39
Q

Imexact numbers

A

Comes from measurement as there are always limitations

40
Q

Percentage uncertainty

A

(Absolute uncertainty/ measured quantity) x 100

41
Q

Significant figures - + and -

A

Result has same number of decimal places as the measurement with the fewest number of decimal places

42
Q

Significant numbers - x and /

A

Same number of significant figures as the measurement with the least figures

43
Q

Molecular Formalue

A

Chemical formula that refers to discrete molecule

44
Q

Naming - ionic compounds

A

Cation followed by anion

45
Q

Covalent compounds

A

Carbon first, followed by hydrogen then remaining elements in alphabetical order

46
Q

Naming - inorganic compounds

A

Element closest to the left of periodic table appears first

First element retains elemental name, second element has suffix ide

47
Q

Oxoanions

A

Root name from central atom

48
Q

Oxoanion with fewer molecules when 2 different

A

-ire

49
Q

Oxoanions with more atoms S uffix when 2 different oxoanions

A

-ate

50
Q

Alcohol

A

Functional group + oxygen + hydrgon

51
Q

Aldehydes

A

Functional group+ carbon=oxygen + hydrogen

52
Q

Ketone

A

Functional group+ carbon=oxygen + functional group

53
Q

Carboxylic Acids

A

Functional group + carbon=oxygen+ OH

54
Q

First she’ll

A

2 electrons

55
Q

Second she’ll

A

Up to 8 electrons

56
Q

Third she’ll

A

Up to 18 electrons

57
Q

Forth and other shells

A

Up to 32 electrons

58
Q

Covalent bond - energy

A

Very strong bonding so it takes a lot of energy to break

59
Q

Ionic attraction

A

Attraction of opposite charges

60
Q

Hydrogen bonds

A

Attraction between h+ and strongly electronegative atom

61
Q

Hydrophobic interactions

A

Interactions of non polar substances in the presence of polar substances

62
Q

Van der waals interactions

A

Interaction of electrons of non polar substances

63
Q

Sharing of electrons covalent bonds

A

If 2 of same atom then sharing is equal

If 2 different atoms then sharing isn’t equal and the one with the greater force will hold electrons closer

Chemistry 1A (12 decks)

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