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chemistry 1/2 > basic terms and concepts > Flashcards

basic terms and concepts Flashcards

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1
Q

what is an atom?

A

basic building block of matter; makes up everything

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2
Q

what is a proton?

A

a stable subatomic particle in the nucleus of an atom; positive electric charge equal to an electron

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3
Q

what is a neutron?

A

neutral subatomic particle found in nucleus; has mass

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4
Q

what is an electron?

A

negatively charged subatomic particle with negligible mass; outside the nucleus

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5
Q

what is an element?

A

made up of one type of atom

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6
Q

what is an atomic number?

A

the number of protons in the nucleus of an atom, determines an element’s place in the periodic table

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7
Q

what is the mass number?

A

sum of protons and neutrons in the nucleus

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8
Q

what is a compound?

A

any substance made of identical molecules consisting of 2 or more elements

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9
Q

what is isotope?

A

atoms with same number of protons but different numbers of neutrons

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10
Q

what is an ion?

A

any atom or group of atoms that has positive or negative charge (no. electrons and no. protons are different)

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11
Q

what is a cation?

A

positively charged ion

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12
Q

what is an anion?

A

negatively charged ion

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13
Q

what is an ionic compound?

A

compounds made up of ions that are held together by the attraction among oppositely charged ions

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14
Q

what is a polyatomic ion?

A

ion composed of two or more atoms, has either positive or negative charge

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15
Q

what is a solution?

A

homogenous mixture of 2 or more substances, consists of solute and solvent

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16
Q

what is dissociation?

A

when ionic compounds readily dissolve in water

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17
Q

what does soluble mean?

A

can be dissolved or liquified

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18
Q

what does insoluble mean?

A

cannot be dissolved or liquified

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19
Q

what is a precipitate?

A

a solid formed by change in solution, often due to a chemical reaction/change in temperature

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20
Q

what is the structure of an atom?

A
  • consists of 3 basic particles: protons, electrons, and neutrons
  • nucleus contains protons and neutrons
  • electron shells (outermost region) contain electrons
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21
Q

what do A, Z and X represent in an atomic symbol?

A

X - chemical symbol; for the element
Z - atomic number; no. of protons in the nucleus
A - mass number; no. of protons + neutrons in the nucleus (nucleons)
*neutron number: N = A -Z

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22
Q

electron configuration rule 1

A
  • each shell can only contain a maximum number of electrons
  • shell number n is filled by 2n^2
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23
Q

electron configuration rule 2

A
  • lower energy shells fill before higher energy shells
  • shells closer to the nucleus therefore fill up first
24
Q

electron configuration rule 3

A
  • electron shells fill in a particular order
  • outer shell can never contain more than 8 electrons, regardless of maximum possible number for that shell (octet rule)
  • the 3rd shell can hold a max of 18 electrons; however, it will not contain more than eight until there are at least 2 electrons in the 4th shell
25
Q

how are ions formed?

A
  • when an atom loses, gains or shares valence electrons to achieve eight electrons in their outer shell (octet rule)
  • metals tend to lose electrons and become positively charged (cations)
  • non-metals tend to gain electrons and so become negatively charged (anions)
26
Q

what is the ionic charge of zinc?

A

+2

27
Q

what is the ionic charge of silver?

A

+1

28
Q

what is the order of electronic charges in the periodic table?

A

+1, +2, transition metals, +3, +-4, -3, -2, -1, 0

29
Q

how are cations named for metals?

A
  • has the same name as the element
  • some metals form ions with multiple different charges (use roman numerals to tell the difference between these ions)
30
Q

how are non-metal anions named?

A
  • has a similar name as the element but ends in ‘-ide’ (usually means no oxygen - except for oxide)
    e.g. sulfide - no oxygen; sulfite - some oxygen; sulfate - max oxygen for the element
  • ‘-ite’ or ‘-ate’ - has oxygen
31
Q

how are ionic compounds formed?

A
  • they are made from the attraction between ions of metallic and non-metallic elements
  • large quantities of cations and anions join to form a regularly arranged 3D lattice, held together by electrostatic forces of attraction between the positive and negative ions
32
Q

what is the chemical formula for ammonium?

A

NH4+

33
Q

what is the chemical formula for hydroxide?

A

OH-

34
Q

what is the chemical formula for ethanoate?

A

CH3COOH

35
Q

what is the chemical formula for nitrate?

A

NO3-

36
Q

what is the chemical formula for sulphate?

A

SO4,2-

37
Q

what is the chemical formula for carbonate?

A

CO3,2-

38
Q

what is the chemical formula for phosphate?

A

PO4, 3-

39
Q

what does (aq) mean?

A

aqueous - means that the substance has dissolved in water

40
Q

what does (s) mean?

A

that the substance is still solid

41
Q

what are the SNAPE ions (ALWAYS SOLUBLE)?

A
  • sodium ion
  • nitrate ion
  • ammonium ion
  • potassium ion
  • ethanoate ion
42
Q

exceptions to nitrate that are insoluble

A

none

43
Q

exceptions to ethanoate (acetate) that are insoluble

A

none

44
Q

exceptions to sodium, potassium that are insoluble

A

none

45
Q

exceptions to ammonium that are insoluble

A

none

46
Q

exceptions to chloride that are insoluble

A
  • AgCl
  • HgCL2
  • PbCl2 (slightly soluble)
47
Q

exceptions to bromide that are insoluble

A
  • AgBr
  • HgBr2
  • PbBr2
48
Q

exceptions to iodide that are insoluble

A
  • AgI
  • HgI2
  • PbI2
49
Q

exceptions to sulfate that are insoluble

A
  • BaSO4
  • PbSO4
  • CaSO4 (slightly soluble)
50
Q

what are the insoluble ionic compounds?

A
  • sulfide
  • carbonate
  • phosphate
  • hydroxide
51
Q

exceptions to sulfide that are soluble

A
  • Na2S
  • K2S
  • Li2S
  • (NH4)2S
52
Q

exceptions to carbonate that are soluble

A
  • Na2CO3
  • K2CO3
  • Li2CO3
53
Q

exceptions to phosphate that are soluble

A
  • Na3PO4
  • K3PO4
  • Li3PO4
54
Q

exceptions to hydroxide that are soluble

A
  • NaOH
  • KOH
  • Ba(OH)2
  • Ca(OH)2 (slightly soluble)
55
Q

how to write balanced chemical equations

A
  1. identify reactants and products
  2. write the chemical formulae for each of the reactants and products
  3. identify the precipitate using solubility rules and write the state in brackets for all reactants and products
  4. balance the number and type of each atom on either side of the reaction arrow. This can only be done by adding a number IN FRONT of the chemical formulas
56
Q

how to predict precipitation reactions

A

use the solubility rules to identify what will be the solid

chemistry 1/2 (1 decks)

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